September 23, 2006 at 2:43 pm | Posted in History, Research, Science & Technology, United Kingdom | Leave a comment



Michael Faraday

Michael Faraday, FRS

(September 22, 1791August 25, 1867) was an English chemist and physicist (or natural philosopher, in the terminology of

that time) who contributed significantly to the fields of electromagnetism

and electrochemistry. He established that magnetism

could affect rays of light and that there was an underlying relationship between the two


Some historians of science refer to him as the best experimentalist

in the history of science. It was largely due to his efforts that electricity became viable for use in technology. The SI unit of capacitance, the farad, is named after him, as is the Faraday constant, the charge on a mole of electrons (about 96,485 coulombs). Faraday’s law of induction states that a magnetic field changing in time creates a proportional electromotive force.

He held the post of Fullerian Professor of Chemistry at the Royal Institution of Great Britain.

Faraday was the first, and most famous, holder of this position to which he was appointed for life


Published Works by Michael Faraday

  • Chemical Manipulation, being Instructions to Students in Chemistry
  • (1 vol., John

    Murray, 1st ed. 1827, 2nd 1830, 3rd 1842);

  • Experimental Researches in Electricity, vols. i. and ii., Richard and John Edward

    Taylor, vols. i. and ii. (1844 and 1847); vol. iii. (1844); vol. iii. Richard Taylor and

    William Francis (1855);

  • Experimental Researches in Chemistry and Physics, Taylor and Francis (1859);
  • A Course of Six Lectures on the Chemical History of a Candle
  • (edited by W. Crookes)

    (Griffin, Bohn & Co., 1861);

  • On the Various Forces in Nature
  • (edited by W. Crookes) (Chatto & Windus, 1873).

  • A Course of 6 lectures on the various forces of matter and their relations to each

    other. edited by William Crookes(1861).

  • His Diary edited by T. Martin was published in eight volumes (1932 – 36) The Chemical History Of A Candle, by Michael Faraday


    Title: The Chemical History Of A Candle

    Author: Michael Faraday












    From the primitive pine-torch to the paraffin candle, how wide an

    interval! between them how vast a contrast! The means adopted by man to

    illuminate his home at night, stamp at once his position in the scale of

    civilisation. The fluid bitumen of the far East, blazing in rude vessels

    of baked earth; the Etruscan lamp, exquisite in form, yet ill adapted to

    its office; the whale, seal, or bear fat, filling the hut of the Esquimaux

    or Lap with odour rather than light; the huge wax candle on the glittering

    altar, the range of gas lamps in our streets,–all have their stories to

    tell. All, if they could speak (and, after their own manner, they can),

    might warm our hearts in telling, how they have ministered to man’s

    comfort, love of home, toil, and devotion.

    Surely, among the millions of fire-worshippers and fire-users who have

    passed away in earlier ages, _some_ have pondered over the mystery of

    fire; perhaps some clear minds have guessed shrewdly near the truth. Think

    of the time man has lived in hopeless ignorance: think that only during a

    period which might be spanned by the life of one man, has the truth been


    Atom by atom, link by link, has the reasoning chain been forged. Some

    links, too quickly and too slightly made, have given way, and been

    replaced by better work; but now the great phenomena are known–the

    outline is correctly and firmly drawn–cunning artists are filling in the

    rest, and the child who masters these Lectures knows more of fire than

    Aristotle did.

    The candle itself is now made to light up the dark places of nature; the

    blowpipe and the prism are adding to our knowledge of the earth’s crust;

    but the torch must come first.

    Among the readers of this book some few may devote themselves to

    increasing the stores of knowledge: the Lamp of Science _must_ burn.

    “_Alere flammam._”






















    I purpose, in return for the honour you do us by coming to see what are

    our proceedings here, to bring before you, in the course of these

    lectures, the Chemical History of a Candle. I have taken this

    subject on a

    former occasion; and were it left to my own will, I should prefer to

    repeat it almost every year–so abundant is the interest that attaches

    itself to the subject, so wonderful are the varieties of outlet which it

    offers into the various departments of philosophy. There is not a law

    under which any part of this universe is governed which does not come into

    play, and is touched upon in these phenomena. There is no better, there is

    no more open door by which you can enter into the study of natural

    philosophy, than by considering the physical phenomena of a candle. I

    trust, therefore, I shall not disappoint you in choosing this for my

    subject rather than any newer topic, which could not be better, were it

    even so good.

    And before proceeding, let me say this also–that though our subject be so

    great, and our intention that of treating it honestly, seriously, and

    philosophically, yet I mean to pass away from all those who are seniors

    amongst us. I claim the privilege of speaking to juveniles as a juvenile

    myself. I have done so on former occasions–and, if you please, I shall do

    so again. And though I stand here with the knowledge of having the words I

    utter given to the world, yet that shall not deter me from speaking in the

    same familiar way to those whom I esteem nearest to me on this occasion.

    And now, my boys and girls, I must first tell you of what candles are

    made. Some are great curiosities. I have here some bits of timber,

    branches of trees particularly famous for their burning. And here you see

    a piece of that very curious substance taken out of some of the bogs in

    Ireland, called _candle-wood_,–a hard, strong, excellent wood, evidently

    fitted for good work as a resister of force, and yet withal burning so

    well that where it is found they make splinters of it, and torches, since

    it burns like a candle, and gives a very good light indeed. And in this

    wood we have one of the most beautiful illustrations of the general nature

    of a candle that I can possibly give. The fuel provided, the means of

    bringing that fuel to the place of chemical action, the regular and

    gradual supply of air to that place of action–heat and light–all

    produced by a little piece of wood of this kind, forming, in fact, a

    natural candle.

    But we must speak of candles as they are in commerce. Here are a couple of

    candles commonly called dips. They are made of lengths of cotton cut off,

    hung up by a loop, dipped into melted tallow, taken out again and cooled,

    then re-dipped until there is an accumulation of tallow round the cotton.

    In order that you may have an idea of the various characters of these

    candles, you see these which I hold in my hand–they are very small, and

    very curious. They are, or were, the candles used by the miners in coal

    mines. In olden times the miner had to find his own candles; and it was

    supposed that a small candle would not so soon set fire to the fire-damp

    in the coal mines as a large one; and for that reason, as well as for

    economy’s sake, he had candles made of this sort–20, 30, 40, or 60 to the

    pound. They have been replaced since then by the steel-mill, and then by

    the Davy-lamp, and other safety-lamps of various kinds. I have here a

    candle that was taken out of the _Royal George_[1], it is said, by Colonel

    Pasley. It has been sunk in the sea for many years, subject to the action

    of salt water. It shews you how well candles may be preserved; for though

    it is cracked about and broken a good deal, yet, when lighted, it goes on

    burning regularly, and the tallow resumes its natural condition as soon as

    it is fused.

    Mr. Field, of Lambeth, has supplied me abundantly with beautiful

    illustrations of the candle and its materials. I shall therefore now refer

    to them. And, first, there is the suet–the fat of the ox–Russian tallow,

    I believe, employed in the manufacture of these dips, which Gay Lussac, or

    some one who entrusted him with his knowledge, converted into that

    beautiful substance, stearin, which you see lying beside it. A candle, you

    know, is not now a greasy thing like an ordinary tallow candle, but a

    clean thing, and you may almost scrape off and pulverise the drops which

    fall from it without soiling anything. This is the process he

    adopted[2]:–The fat or tallow is first boiled with quick-lime, and made

    into a soap, and then the soap is decomposed by sulphuric acid, which

    takes away the lime, and leaves the fat re-arranged as stearic acid,

    whilst a quantity of glycerin is produced at the same time.

    Glycerin–absolutely a sugar, or a substance similar to sugar–comes out

    of the tallow in this chemical change. The oil is then pressed out of it;

    and you see here this series of pressed cakes, shewing how beautifully the

    impurities are carried out by the oily part as the pressure goes on

    increasing, and at last you have left that substance which is melted, and

    cast into candles as here represented. The candle I have in my hand is a

    stearin candle, made of stearin from tallow in the way I have told you.

    Then here is a sperm candle, which comes from the purified oil of the

    spermaceti whale. Here also are yellow bees-wax and refined bees-wax, from

    which candles are made. Here, too, is that curious substance called

    paraffin, and some paraffin candles made of paraffin obtained from the

    bogs of Ireland. I have here also a substance brought from Japan, since we

    have forced an entrance into that out-of-the-way place–a sort of wax

    which a kind friend has sent me, and which forms a new material for the

    manufacture of candles.

    And how are these candles made? I have told you about dips, and I will

    shew you how moulds are made. Let us imagine any of these candles to be

    made of materials which can be cast. “Cast!” you say. “Why, a candle is a

    thing that melts; and surely if you can melt it, you can cast it.” Not so.

    It is wonderful, in the progress of manufacture, and in the consideration

    of the means best fitted to produce the required result, how things turn

    up which one would not expect beforehand. Candles cannot always be cast. A

    wax candle can never be cast. It is made by a particular process, which I

    can illustrate in a minute or two: but I must not spend much time on it.

    Wax is a thing which, burning so well, and melting so easily in a candle,

    cannot be cast. However, let us take a material that can be cast. Here is

    a frame, with a number of moulds fastened in it. The first thing to be

    done is to put a wick through them. Here is one–a plaited wick, which

    does not require snuffing[3]–supported by a little wire. It goes to the

    bottom, where it is pegged in–the little peg holding the cotton tight,

    and stopping the aperture, so that nothing fluid shall run out. At the

    upper part there is a little bar placed across, which stretches the cotton

    and holds it in the mould. The tallow is then melted, and the moulds are

    filled. After a certain time, when the moulds are cool, the excess of

    tallow is poured off at one corner, and then cleaned off altogether, and

    the ends of the wick cut away. The candles alone then remain in the mould,

    and you have only to upset them, as I am doing, when out they tumble, for

    the candles are made in the form of cones, being narrower at the top than

    at the bottom; so that what with their form and their own shrinking, they

    only need a little shaking, and out they fall. In the same way are made

    these candles of stearin and of paraffin. It is a curious thing to see how

    wax candles are made. A lot of cottons are hung upon frames, as you see

    here, and covered with metal tags at the ends to keep the wax from

    covering the cotton in those places. These are carried to a heater, where

    the wax is melted. As you see, the frames can turn round; and as they

    turn, a man takes a vessel of wax and pours it first down one, and then

    the next and the next, and so on. When he has gone once round, if it is

    sufficiently cool, he gives the first a second coat, and so on until they

    are all of the required thickness. When they have been thus clothed, or

    fed, or made up to that thickness, they are taken off, and placed

    elsewhere. I have here, by the kindness of Mr. Field, several specimens of

    these candles. Here is one only half-finished. They are then taken down,

    and well rolled upon a fine stone slab, and the conical top is moulded by

    properly shaped tubes, and the bottoms cut off and trimmed. This is done

    so beautifully that they can make candles in this way weighing exactly

    four, or six, to the pound, or any number they please.

    We must not, however, take up more time about the mere manufacture, but go

    a little further into the matter. I have not yet referred you to luxuries

    in candles (for there is such a thing as luxury in candles). See how

    beautifully these are coloured: you see here mauve, magenta, and all the

    chemical colours recently introduced, applied to candles. You observe,

    also, different forms employed. Here is a fluted pillar most beautifully

    shaped; and I have also here some candles sent me by Mr. Pearsall, which

    are ornamented with designs upon them, so that as they burn you have as it

    were a glowing sun above, and a bouquet of flowers beneath. All, however,

    that is fine and beautiful is not useful. These fluted candles, pretty as

    they are, are bad candles; they are bad because of their external shape.

    Nevertheless, I shew you these specimens sent to me from kind friends on

    all sides, that you may see what is done, and what may be done in this or

    that direction; although, as I have said, when we come to these

    refinements, we are obliged to sacrifice a little in utility.

    Now, as to the light of the candle. We will light one or two, and set them

    at work in the performance of their proper functions. You observe a candle

    is a very different thing from a lamp. With a lamp you take a little oil,

    fill your vessel, put in a little moss or some cotton prepared by

    artificial means, and then light the top of the wick. When the flame runs

    down the cotton to the oil, it gets extinguished, but it goes on burning

    in the part above. Now, I have no doubt you will ask, how is it that the

    oil, which will not burn of itself, gets up to the top of the cotton,

    where it will burn? We shall presently examine that; but there is a much

    more wonderful thing about the burning of a candle than this. You have

    here a solid substance with no vessel to contain it; and how is it that

    this solid substance can get up to the place where the flame is? How is it

    that this solid gets there, it not being a fluid? or, when it is made a

    fluid, then how is it that it keeps together? This is a wonderful thing

    about a candle.

    We have here a good deal of wind, which will help us in some of our

    illustrations, but tease us in others; for the sake, therefore, of a

    little regularity, and to simplify the matter, I shall make a quiet

    flame–for who can study a subject when there are difficulties in the way

    not belonging to it? Here is a clever invention of some costermonger or

    street stander in the market-place for the shading of their candles on

    Saturday nights, when they are selling their greens, or potatoes, or fish.

    I have very often admired it. They put a lamp-glass round the candle,

    supported on a kind of gallery, which clasps it, and it can be slipped up

    and down as required. By the use of this lamp-glass, employed in the same

    way, you have a steady flame, which you can look at, and carefully

    examine, as I hope you will do, at home.

    You see, then, in the first instance, that a beautiful cup is formed. As

    the air comes to the candle it moves upwards by the force of the current

    which the heat of the candle produces, and it so cools all the sides of

    the wax, tallow, or fuel, as to keep the edge much cooler than the part

    within; the part within melts by the flame that runs down the wick as far

    as it can go before it is extinguished, but the part on the outside does

    not melt. If I made a current in one direction, my cup would be lop-sided,

    and the fluid would consequently run over,–for the same force of gravity

    which holds worlds together holds this fluid in a horizontal position, and

    if the cup be not horizontal, of course the fluid will run away in

    guttering. You see, therefore, that the cup is formed by this beautifully

    regular ascending current of air playing upon all sides, which keeps the

    exterior of the candle cool. No fuel would serve for a candle which has

    not the property of giving this cup, except such fuel as the Irish

    bogwood, where the material itself is like a sponge, and holds its own

    fuel. You see now why you would have had such a bad result if you were to

    burn these beautiful candles that I have shewn you, which are irregular,

    intermittent in their shape, and cannot therefore have that nicely-formed

    edge to the cup which is the great beauty in a candle. I hope you will now

    see that the perfection of a process–that is, its utility–is the better

    point of beauty about it. It is not the best looking thing, but the best

    acting thing, which is the most advantageous to us. This good-looking

    candle is a bad burning one. There will be a guttering round about it

    because of the irregularity of the stream of air and the badness of the

    cup which is formed thereby. You may see some pretty examples (and I trust

    you will notice these instances) of the action of the ascending current

    when you have A little gutter run down the side of a candle, making it

    thicker there than it is elsewhere. As the candle goes on burning, that

    keeps its place and forms a little pillar sticking up by the side,

    because, as it rises higher above the rest of the wax or fuel, the air

    gets better round it, and it is more cooled and better able to resist the

    action of the heat at a little distance. Now, the greatest mistakes and

    faults with regard to candles, as in many other things, often bring with

    them instruction which we should not receive if they had not occurred. We

    come here to be philosophers; and I hope you will always remember that

    whenever a result happens, especially if it be new, you should say, “What

    is the cause? Why does it occur?” and you will in the course of time find

    out the reason.

    Then, there is another point about these candles which will answer a

    question,–that is, as to the way in which this fluid gets out of the cup,

    up the wick, and into the place of combustion. You know that the flames on

    these burning wicks in candles made of beeswax, stearin, or spermaceti, do

    not run down to the wax or other matter, and melt it all away, but keep to

    their own right place. They are fenced off from the fluid below, and do

    not encroach on the cup at the sides. I cannot imagine a more beautiful

    example than the condition of adjustment under which a candle makes one

    part subserve to the other to the very end of its action. A combustible

    thing like that, burning away gradually, never being intruded upon by the

    flame, is a very beautiful sight; especially when you come to learn what a

    vigorous thing flame is–what power it has of destroying the wax itself

    when it gets hold of it, and of disturbing its proper form if it come only

    too near.

    But how does the flame get hold of the fuel? There is a beautiful point

    about that–_capillary attraction_[4]. “Capillary attraction!” you

    say,–“the attraction of hairs.” Well, never mind the name: it was given

    in old times, before we had a good understanding of what the real power

    was. It is by what is called capillary attraction that the fuel is

    conveyed to the part where combustion goes on, and is deposited there, not

    in a careless way, but very beautifully in the very midst of the centre of

    action which takes place around it. Now, I am going to give you one or two

    instances of capillary attraction. It is that kind of action or attraction

    which makes two things that do not dissolve in each other still hold

    together. When you wash your hands, you wet them thoroughly; you take a

    little soap to make the adhesion better, and you find your hand remains

    wet. This is by that kind of attraction of which I am about to speak. And,

    what is more, if your hands are not soiled (as they almost always are by

    the usages of life), if you put your finger into a little warm water, the

    water will creep a little way up the finger, though you may not stop to

    examine it. I have here a substance which is rather porous–a column of

    salt–and I will pour into the plate at the bottom, not water, as it

    appears, but a saturated solution of salt which cannot absorb more; so

    that the action which you see will not be due to its dissolving anything.

    We may consider the plate to be the candle, and the salt the wick, and

    this solution the melted tallow. (I have coloured the fluid, that you may

    see the action better.) You observe that, now I pour in the fluid, it

    rises and gradually creeps up the salt higher and higher; and provided the

    column does not tumble over, it will go to the top.

    [Illustration: Fig. 1.]

    If this blue solution were combustible, and we were to place a wick at the

    top of the salt, it would burn as it entered into the wick. It is a most

    curious thing to see this kind of action taking place, and to observe how

    singular some of the circumstances are about it. When you wash your hands,

    you take a towel to wipe off the water; and it is by that kind of wetting,

    or that kind of attraction which makes the towel become wet with water,

    that the wick is made wet with the tallow. I have known some careless boys

    and girls (indeed, I have known it happen to careful people as well) who,

    having washed their hands and wiped them with a towel, have thrown the

    towel over the side of the basin, and before long it has drawn all the

    water out of the basin and conveyed it to the floor, because it happened

    to be thrown over the side in such a way as to serve the purpose of a

    syphon.[5] That you may the better see the way in which the substances act

    one upon another, I have here a vessel made of wire gauze filled with

    water, and you may compare it in its action to the cotton in one respect,

    or to a piece of calico in the other. In fact, wicks are sometimes made of

    a kind of wire gauze. You will observe that this vessel is a porous thing;

    for if I pour a little water on to the top, it will run out at the bottom.

    You would be puzzled for a good while if I asked you what the state of

    this vessel is, what is inside it, and why it is there? The vessel is full

    of water, and yet you see the water goes in and runs out as if it were

    empty. In order to prove this to you, I have only to empty it. The reason

    is this,–the wire, being once wetted, remains wet; the meshes are so

    small that the fluid is attracted so strongly from the one side to the

    other, as to remain in the vessel although it is porous. In like manner

    the particles of melted tallow ascend the cotton and get to the top; other

    particles then follow by their mutual attraction for each other, and as

    they reach the flame they are gradually burned.

    Here is another application of the same principle. You see this bit of

    cane. I have seen boys about the streets, who are very anxious to appear

    like men, take a piece of cane, and light it and smoke it, as an imitation

    of a cigar. They are enabled to do so by the permeability of the cane in

    one direction, and by its capillarity. If I place this piece of cane on a

    plate containing some camphin (which is very much like paraffin in its

    general character), exactly in the same manner as the blue fluid rose

    through the salt will this fluid rise through the piece of cane. There

    being no pores at the side, the fluid cannot go in that direction, but

    must pass through its length. Already the fluid is at the top of the cane:

    now I can light it and make it serve as a candle. The fluid has risen by

    the capillary attraction of the piece of cane, just as it does through the

    cotton in the candle.

    Now, the only reason why the candle does not burn all down the side of the

    wick is, that the melted tallow extinguishes the flame. You know that a

    candle, if turned upside down, so as to allow the fuel to run upon the

    wick, will be put out. The reason is, that the flame has not had time to

    make the fuel hot enough to burn, as it does above, where it is carried in

    small quantities into the wick, and has all the effect of the heat

    exercised upon it.

    There is another condition which you must learn as regards the candle,

    without which you would not be able fully to understand the philosophy of

    it, and that is the vaporous condition of the fuel.  In order that you may

    understand that, let me shew you a very pretty, but very common-place

    experiment. If you blow a candle out cleverly, you will see the vapour

    rise from it. You have, I know, often smelt the vapour of a blown-out

    candle–and a very bad smell it is; but if you blow it out cleverly, you

    will be able to see pretty well the vapour into which this solid matter is

    transformed.  I will blow out one of these candles in such a way as not to

    disturb the air around it, by the continuing action of my breath; and now,

    if I hold a lighted taper two or three inches from the wick, you will

    observe a train of fire going through the air till it reaches the candle.

    I am obliged to be quick and ready, because, if I allow the vapour time to

    cool, it becomes condensed into a liquid or solid, or the stream of

    combustible matter gets disturbed.

    Now, as to the shape or form of the flame. It concerns us much to know

    about the condition which the matter of the candle finally assumes at the

    top of the wick–where you have such beauty and brightness as nothing but

    combustion or flame can produce.

    [Illustration: Fig. 2.]

    You have the glittering beauty of gold and silver, and the still higher

    lustre of jewels, like the ruby and diamond; but none of these rival the

    brilliancy and beauty of flame. What diamond can shine like flame? It owes

    its lustre at night-time to the very flame shining upon it. The flame

    shines in darkness, but the light which the diamond has is as nothing

    until the flame shine upon it, when it is brilliant again. The candle

    alone shines by itself, and for itself, or for those who have arranged the

    materials. Now, let us look a little at the form of the flame as you see

    it under the glass shade. It is steady and equal; and its general form is

    that which is represented in the diagram, varying with atmospheric

    disturbances, and also varying according to the size of the candle. It is

    a bright oblong–brighter at the top than towards the bottom–with the

    wick in the middle, and besides the wick in the middle, certain darker

    parts towards the bottom, where the ignition is not so perfect as in the

    part above.

    [Illustration: Fig. 3.]

    I have a drawing here, sketched many years ago by Hooker, when he made his

    investigations. It is the drawing of the flame of a lamp, but it will

    apply to the flame of a candle. The cup of the candle is the vessel or

    lamp, the melted spermaceti is the oil, and the wick is common to both.

    Upon that he sets this little flame, and then he represents what is

    true–a certain quantity of matter rising about it which you do not see,

    and which, if you have not been here before, or are not familiar with the

    subject, you will not know of. He has here represented the parts of the

    surrounding atmosphere that are very essential to the flame, and that are

    always present with it. There is a current formed, which draws the flame

    out–for the flame which you see is really drawn out by the current, and

    drawn upward to a great height–just as Hooker has here shewn you by that

    prolongation of the current in the diagram. You may see this by taking a

    lighted candle, and putting it in the sun so as to get its shadow thrown

    on a piece of paper. How remarkable it is that that thing which is light

    enough to produce shadows of other objects, can be made to throw its own

    shadow on a piece of white paper or card, so that you can actually see

    streaming round the flame something which is not part of the flame, but is

    ascending and drawing the flame upwards. Now, I am going to imitate the

    sunlight, by applying the voltaic battery to the electric lamp. You now

    see our sun, and its great luminosity; and by placing a candle between it

    and the screen, we get the shadow of the flame.

    [Illustration: Fig. 4.]

    You observe the shadow of the candle and of the wick; then there is a

    darkish part, as represented in the diagram, and then a part which is more

    distinct. Curiously enough, however, what we see in the shadow as the

    darkest part of the flame is, in reality, the brightest part; and here you

    see streaming upwards the ascending current of hot air, as shewn by

    Hooker, which draws out the flame, supplies it with air, and cools the

    sides of the cup of melted fuel.

    I can give you here a little further illustration, for the purpose of

    shewing you how flame goes up or down; according to the current. I have

    here a flame–it is not a candle flame–but you can, no doubt, by this

    time, generalise enough to be able to compare one thing with another. What

    I am about to do is to change the ascending current that takes the flame

    upwards into a descending current. This I can easily do by the little

    apparatus you see before me. The flame, as I have said, is not a candle

    flame, but it is produced by alcohol, so that it shall not smoke too much.

    I will also colour the flame with another substance[6], so that you may

    trace its course; for with the spirit alone you could hardly see well

    enough to have the opportunity of tracing its direction. By lighting this

    spirit-of-wine, we have then a flame produced; and you observe that when

    held in the air, it naturally goes upwards.

    [Illustration: Fig. 5]

    You understand now easily enough why flames go up under ordinary

    circumstances–it is because of the draught of air by which the combustion

    is formed. But now, by blowing the flame down, you see I am enabled to

    make it go downwards into this little chimney–the direction of the

    current being changed. Before we have concluded this course of lectures,

    we shall shew you a lamp in which the flame goes up and the smoke goes

    down, or the flame goes down and the smoke goes up. You see, then, that we

    have the power in this way of varying the flame in different directions.

    There are now some other points that I must bring before you. Many of the

    flames you see here vary very much in their shape by the currents of air

    blowing around them in different directions; but we can, if we like, make

    flames so that they will look like fixtures, and we can photograph

    them–indeed, we have to photograph them–so that they become fixed to us,

    if we wish to find out everything concerning them. That, however, is not

    the only thing I wish to mention. If I take a flame sufficiently large, it

    does not keep that homogeneous, that uniform condition of shape, but it

    breaks out with a power of life which is quite wonderful. I am about to

    use another kind of fuel, but one which is truly and fairly a

    representative of the wax or tallow of a candle. I have here a large ball

    of cotton, which will serve as a wick. And, now that I have immersed it in

    spirit and applied a light to it, in what way does it differ from an

    ordinary candle? Why, it differs very much in one respect, that we have a

    vivacity and power about it, a beauty and a life entirely different from

    the light presented by a candle. You see those fine tongues of flame

    rising up. You have the same general disposition of the mass of the flame

    from below upwards; but, in addition to that, you have this remarkable

    breaking out into tongues which you do not perceive in the case of a

    candle. Now, why is this? I must explain it to you, because when you

    understand that perfectly, you will be able to follow me better in what I

    have to say hereafter. I suppose some here will have made for themselves

    the experiment I am going to shew you. Am I right in supposing that

    anybody here has played at snapdragon? I do not know a more beautiful

    illustration of the philosophy of flame, as to a certain part of its

    history, than the game of snapdragon. First, here is the dish; and let me

    say, that when you play snapdragon properly, you ought to have the dish

    well-warmed; you ought also to have warm plums and warm brandy, which,

    however, I have not got. When you have put the spirit into the dish, you

    have the cup and the fuel; and are not the raisins acting like the wicks?

    I now throw the plums into the dish, and light the spirit, and you see

    those beautiful tongues of flame that I refer to. You have the air

    creeping in over the edge of the dish forming these tongues. Why? Because,

    through the force of the current and the irregularity of the action of the

    flame, it cannot flow in one uniform stream. The air flows in so

    irregularly that you have what would otherwise be a single image, broken

    up into a variety of forms, and each of these little tongues has an

    independent existence of its own. Indeed, I might say, you have here a

    multitude of independent candles. You must not imagine, because you see

    these tongues all at once, that the flame is of this particular shape. A

    flame of that shape is never so at any one time. Never is a body of flame,

    like that which you just saw rising from the ball, of the shape it appears

    to you. It consists of a multitude of different shapes, succeeding each

    other so fast that the eye is only able to take cognisance of them all at

    once. In former times, I purposely analysed a flame of that general

    character, and the diagram shews you the different parts of which it is

    composed. They do not occur all at once: it is only because we see these

    shapes in such rapid succession, that they seem to us to exist all at one


    [Illustration: Fig. 6.]

    It is too bad that we have not got further than my game of snapdragon; but

    we must not, under any circumstances, keep you beyond your time. It will

    be a lesson to me in future to hold you more strictly to the philosophy of

    the thing, than to take up your time so much with these illustrations.




    We were occupied the last time we met in considering the general character

    and arrangement as regards the fluid portion of a candle, and the way in

    which that fluid got into the place of combustion. You see, when we have a

    candle burning fairly in a regular, steady atmosphere, it will have a

    shape something like the one shewn in the diagram, and will look pretty

    uniform, although very curious in its character. And now, I have to ask

    your attention to the means by which we are enabled to ascertain what

    happens in any particular part of the flame–why it happens, what it does

    in happening, and where, after all, the whole candle goes to: because, as

    you know very well, a candle being brought before us and burned,

    disappears, if burned properly, without the least trace of dirt in the

    candlestick–and this is a very curious circumstance. In order, then, to

    examine this candle carefully, I have arranged certain apparatus, the use

    of which you will see as I go on. Here is a candle: I am about to put the

    end of this glass tube into the middle of the flame–into that part which

    old Hooker has represented in the diagram as being rather dark, and which

    you can see at any time, if you will look at a candle carefully, without

    blowing it about. We will examine this dark part first.

    [Illustration: Fig. 7.]

    Now, I take this bent glass tube, and introduce one end into that part of

    the flame, and you see at once that something is coming from the flame,

    out at the other end of the tube; and if I put a flask there, and leave it

    for a little while, you will see that something from the middle part of

    the flame is gradually drawn out, and goes through the tube and into that

    flask, and there behaves very differently from what it does in the open

    air. It not only escapes from the end of the tube, but falls down to the

    bottom of the flask like a heavy substance, as indeed it is. We find that

    this is the wax of the candle made into a vaporous fluid–not a gas. (You

    must learn the difference between a gas and a vapour: a gas remains

    permanent, a vapour is something that will condense.) If you blow out a

    candle, you perceive a very nasty smell, resulting from the condensation

    of this vapour. That is very different from what you have outside the

    flame; and, in order to make that more clear to you, I am about to produce

    and set fire to a larger portion of this vapour–for what we have in the

    small way in a candle, to understand thoroughly, we must, as philosophers,

    produce in a larger way, if needful, that we may examine the different

    parts. And now Mr. Anderson will give me a source of heat, and I am about

    to shew you what that vapour is. Here is some wax in a glass flask, and I

    am going to make it hot, as the inside of that candle-flame is hot, and

    the matter about the wick is hot. [The Lecturer placed some wax in a glass

    flask, and heated it over a lamp.] Now, I dare say that is hot enough for

    me. You see that the wax I put in it has become fluid, and there is a

    little smoke coming from it. We shall very soon have the vapour rising up.

    I will make it still hotter, and now we get more of it, so that I can

    actually pour the vapour out of the flask into that basin, and set it on

    fire there. This, then, is exactly the same kind of vapour as we have in

    the middle of the candle; and that you may be sure this is the case, let

    us try whether we have not got here, in this flask, a real combustible

    vapour out of the middle of the candle. [Taking the flask into which the

    tube from the candle proceeded, and introducing a lighted taper.] See how

    it burns. Now, this is the vapour from the middle of the candle, produced

    by its own heat; and that is one of the first things you have to consider

    with respect to the progress of the wax in the course of its combustion,

    and as regards the changes it undergoes. I will arrange another tube

    carefully in the flame, and I should not wonder if we were able, by a

    little care, to get that vapour to pass through the tube to the other

    extremity, where we will light it, and obtain absolutely the flame of the

    candle at a place distant from it.  Now, look at that. Is not that a very

    pretty experiment? Talk about laying on gas–why, we can actually lay on a

    candle! And you see from this that there are clearly two different kinds

    of action–one the _production_ of the vapour, and the other the

    _combustion_ of it–both of which take place in particular parts of the


    [Illustration: Fig. 8]

    I shall get no vapour from that part which is already burnt. If I raise

    the tube (fig. 7) to the upper part of the flame, so soon as the vapour

    has been swept out, what comes away will be no longer combustible: It is

    already burned. How burned? Why, burned thus:–In the middle of the flame,

    where the wick is, there is this combustible vapour; on the outside of the

    flame is the air which we shall find necessary for the burning of the

    candle; between the two, intense chemical action takes place, whereby the

    air and the fuel act upon each other, and at the very same time that we

    obtain light the vapour inside is destroyed. If you examine where the heat

    of a candle is, you will find it very curiously arranged. Suppose I take

    this candle, and hold a piece of paper close upon the flame, where is the

    heat of that flame? Do you not see that it is _not_ in the inside? It is

    in a ring, exactly in the place where I told you the chemical action was;

    and even in my irregular mode of making the experiment, if there is not

    too much disturbance, there will always be a ring. This is a good

    experiment for you to make at home. Take a strip of paper, have the air in

    the room quiet, and put the piece of paper right across the middle of the

    flame (I must not talk while I make the experiment), and you will find

    that it is burnt in two places, and that it is not burnt, or very little

    so, in the middle; and when you have tried the experiment once or twice,

    so as to make it nicely, you will be very interested to see where the heat

    is, and to find that it is where the air and the fuel come together.

    This is most important for us as we proceed with our subject. Air is

    absolutely necessary for combustion; and, what is more, I must have you

    understand that _fresh_ air is necessary, or else we should be imperfect

    in our reasoning and our experiments. Here is a jar of air. I place it

    over a candle, and it burns very nicely in it at first, shewing that what

    I have said about it is true; but there will soon be a change. See how the

    flame is drawing upwards, presently fading, and at last going out. And

    going out, why? Not because it wants air merely, for the jar is as full

    now as it was before; but it wants pure, fresh air. The jar is full of

    air, partly changed, partly not changed; but it does not contain

    sufficient of the fresh air which is necessary for the combustion of a

    candle. These are all points which we, as young chemists, have to gather

    up; and if we look a little more closely into this kind of action, we

    shall find certain steps of reasoning extremely interesting. For instance,

    here is the oil-lamp I shewed you–an excellent lamp for our

    experiments–the old Argand lamp. I now make it like a candle [obstructing

    the passage of air into the centre of the flame]; there is the cotton;

    there is the oil rising up it; and there is the conical flame. It burns

    poorly, because there is a partial restraint of air. I have allowed no air

    to get to it, save round the outside of the flame, and it does not burn

    well. I cannot admit more air from the outside, because the wick is large;

    but if, as Argand did so cleverly, I open a passage to the middle of the

    flame, and so let air come in there, you will see how much more

    beautifully it burns. If I shut the air off, look how it smokes; and why?

    We have now some very interesting points to study. We have the case of the

    combustion of a candle; we have the case of a candle being put out by the

    want of air; and we have now the case of imperfect combustion; and this is

    to us so interesting, that I want you to understand it as thoroughly as

    you do the case of a candle burning in its best possible manner. I will

    now make a great flame, because we need the largest possible

    illustrations. Here is a larger wick [burning turpentine on a ball of

    cotton]. All these things are the same as candles, after all. If we have

    larger wicks, we must have a larger supply of air, or we shall have less

    perfect combustion. Look now at this black substance going up into the

    atmosphere; there is a regular stream of it. I have provided means to

    carry off the imperfectly burned part, lest it should annoy you. Look at

    the soots that fly off from the flame: see what an imperfect combustion it

    is, because it cannot get enough air. What, then, is happening? Why,

    certain things which are necessary to the combustion of a candle are

    absent, and very bad results are accordingly produced; but we see what

    happens to a candle when it is burnt in a pure and proper state of air. At

    the time when I shewed you this charring by the ring of flame on the one

    side of the paper, I might have also shewn you, by turning to the other

    side, that the burning of a candle produces the same kind of

    soot–charcoal or carbon.

    But, before I shew that, let me explain to you–as it is quite necessary

    for our purpose–that, though I take a candle and give you, as the general

    result, its combustion in the form of a flame, we must see whether

    combustion is always in this condition, or whether there are other

    conditions of flame; and we shall soon discover that there are, and that

    they are most important to us. I think, perhaps, the best illustration of

    such a point to us, as juveniles, is to shew the result of strong

    contrast. Here is a little gunpowder. You know that gunpowder burns with

    flame–we may fairly call it flame. It contains carbon and other

    materials, which altogether cause it to burn with a flame. And here is

    some pulverised iron, or iron filings. Now, I purpose burning these two

    things together. I have a little mortar in which I will mix them. (Before

    I go into these experiments, let me hope that none of you, by trying to

    repeat them, for fun’s sake, will do any harm. These things may all be

    very properly used if you take care; but without that, much mischief will

    be done.) Well, then, here is a little gunpowder, which I put at the

    bottom of that little wooden vessel, and mix the iron filings up with it,

    my object being to make the gunpowder set fire to the filings and burn

    them in the air, and thereby shew the difference between substances

    burning with flame and not with flame. Here is the mixture; and when I set

    fire to it, you must watch the combustion, and you will see that it is of

    two kinds. You will see the gunpowder burning with a flame, and the

    filings thrown up. You will see them burning too, but without the

    production of flame.  They will each burn separately. [The Lecturer then

    ignited the mixture.] There is the gunpowder, which burns with a flame;

    and there are the filings–they burn with a different kind of combustion.

    You see, then, these two great distinctions; and upon these differences

    depend all the utility and all the beauty of flame which we use for the

    purpose of giving out light. When we use oil, or gas, or candle, for the

    purpose of illumination, their fitness all depends upon these different

    kinds of combustion.

    There are such curious conditions of flame, that it requires some

    cleverness and nicety of discrimination to distinguish the kinds of

    combustion one from another. For instance, here is a powder which is very

    combustible, consisting, as you see, of separate little particles. It is

    called _lycopodium_[7], and each of these particles can produce a vapour,

    and produce its own flame; but, to see them burning, you would imagine it

    was all one flame. I will now set fire to a quantity, and you will see the

    effect. We saw a cloud of flame, apparently in one body; but that rushing

    noise [referring to the sound produced by the burning] was a proof that

    the combustion was not a continuous or regular one. This is the lightning

    of the pantomimes, and a very good imitation. [The experiment was twice

    repeated by blowing lycopodium from a glass tube through a spirit-flame.]

    This is not an example of combustion like that of the filings I have been

    speaking of, to which we must now return.

    Suppose I take a candle, and examine that part of it which appears

    brightest to our eyes. Why, there I get these black particles, which

    already you have seen many times evolved from the flame, and which I am

    now about to evolve in a different way. I will take this candle and clear

    away the gutterage, which occurs by reason of the currents of air; and if

    I now arrange a glass tube so as just to dip into this luminous part, as

    in our first experiment, only higher, you see the result. In place of

    having the same white vapour that you had before, you will now have a

    black vapour. There it goes, as black as ink. It is certainly very

    different from the white vapour; and when we put a light to it, we shall

    find that it does not burn, but that it puts the light out. Well, these

    particles, as I said before, are just the smoke of the candle; and this

    brings to mind that old employment which Dean Swift recommended to

    servants for their amusement, namely, writing on the ceiling of a room

    with a candle. But what is that black substance? Why, it is the same

    carbon which exists in the candle. How comes it out of the candle? It

    evidently existed in the candle, or else we should not have had it here.

    And now I want you to follow me in this explanation. You would hardly

    think that all those substances which fly about London, in the form of

    soots and blacks, are the very beauty and life of the flame, and which are

    burned in it as those iron filings were burned here. Here is a piece of

    wire gauze, which will not let the flame go through it; and I think you

    will see, almost immediately, that when I bring it low enough to touch

    that part of the flame which is otherwise so bright, that it quells and

    quenches it at once, and allows a volume of smoke to rise up.

    I want you now to follow me in this point,–that whenever a substance

    burns, as the iron filings burnt in the flame of gunpowder, without

    assuming the vaporous state (whether it becomes liquid or remains solid),

    it becomes exceedingly luminous. I have here taken three or four examples

    apart from the candle, on purpose to illustrate this point to you; because

    what I have to say is applicable to all substances, whether they burn or

    whether they do not burn,–that they are exceedingly bright if they retain

    their solid state, and that it is to this presence of solid particles in

    the candle-flame that it owes its brilliancy.

    Here is a platinum-wire, a body which does not change by heat. If I heat

    it in this flame, see how exceedingly luminous it becomes. I will make the

    flame dim, for the purpose of giving a little light only, and yet you will

    see that the heat which it can give to that platinum-wire, though far less

    than the heat it has itself, is able to raise the platinum-wire to a far

    higher state of effulgence. This flame has carbon in it; but I will take

    one that has no carbon in it. There is a material, a kind of fuel–a

    vapour, or gas, whichever you like to call it–in that vessel, and it has

    no solid particles in it; so I take that because it is an example of flame

    itself burning without any solid matter whatever; and if I now put this

    solid substance in it, you see what an intense heat it has, and how

    brightly it causes the solid body to glow. This is the pipe through which

    we convey this particular gas, which we call hydrogen, and which you shall

    know all about next time we meet. And here is a substance called oxygen,

    by means of which this hydrogen can burn; and although we produce, by

    their mixture, far greater heat[8] than you can obtain from the candle,

    yet there is very little light. If, however, I take a solid substance, and

    put that into it, we produce an intense light If I take a piece of lime, a

    substance which will not burn, and which will not vaporise by the heat

    (and because it does not vaporise, remains solid, and remains heated), you

    will soon observe what happens as to its glowing. I have here a most

    intense heat, produced by the burning of hydrogen in contact with the

    oxygen; but there is as yet very little light–not for want of heat, but

    for want of particles which can retain their solid state; but when I hold

    this piece of lime in the flame of the hydrogen as it burns in the oxygen,

    see how it glows! This is the glorious lime-light, which rivals the

    voltaic-light, and which is almost equal to sunlight. I have here a piece

    of carbon or charcoal, which will burn and give us light exactly in the

    same manner as if it were burnt as part of a candle. The heat that is in

    the flame of a candle decomposes the vapour of the wax, and sets free the

    carbon particles–they rise up heated and glowing as this now glows, and

    then enter into the air. But the particles when burnt never pass off from

    a candle in the form of carbon. They go off into the air as a perfectly

    invisible substance, about which we shall know hereafter.

    Is it not beautiful to think that such a process is going on, and that

    such a dirty thing as charcoal can become so incandescent? You see it

    comes to this–that all bright flames contain these solid particles; all

    things that burn and produce solid particles, either during the time they

    are burning, as in the candle, or immediately after being burnt, as in the

    case of the gunpowder and iron-filings,–all these things give us this

    glorious and beautiful light.

    I will give you a few illustrations. Here is a piece of phosphorus, which

    burns with a bright flame. Very well; we may now conclude that phosphorus

    will produce, either at the moment that it is burning or afterwards, these

    solid particles. Here is the phosphorus lighted, and I cover it over with

    this glass for the purpose of keeping in what is produced. What is all

    that smoke? That smoke consists of those very particles which are produced

    by the combustion of the phosphorus. Here, again, are two substances. This

    is chlorate of potassa, and this other sulphuret of antimony. I shall mix

    these together a little, and then they may be burnt in many ways. I shall

    touch them with a drop of sulphuric acid, for the purpose of giving you an

    illustration of chemical action, and they will instantly burn[9]. [The

    Lecturer then ignited the mixture by means of sulphuric acid.] Now, from

    the appearance of things, you can judge for yourselves whether they

    produce solid matter in burning. I have given you the train of reasoning

    which will enable you to say whether they do or do not; for what is this

    bright flame but the solid particles passing off?

    [Illustration: Fig. 9.]

    Mr. Anderson has in the furnace a very hot crucible,–I am about to throw

    into it some zinc filings, and they will burn with a flame like gunpowder.

    I make this experiment because you can make it well at home. Now, I want

    you to see what will be the result of the combustion of this zinc. Here it

    is burning–burning beautifully like a candle, I may say. But what is all

    that smoke, and what are those little clouds of wool which will come to

    you if you cannot come to them, and make themselves sensible to you in the

    form of the old philosophic wool, as it was called? We shall have left in

    that crucible, also, a quantity of this woolly matter. But I will take a

    piece of this same zinc and make an experiment a little more closely at

    home, as it were. You will have here the same thing happening. Here is the

    piece of zinc, there [pointing to a jet of hydrogen] is the furnace, and

    we will set to work and try and burn the metal. It glows, you see: there

    is the combustion, and there is the white substance into which it burns.

    And so, if I take that flame of hydrogen as the representative of a

    candle, and shew you a substance like zinc burning in the flame, you will

    see that it was merely during the action of combustion that this substance

    glowed–while it was kept hot; and if I take a flame of hydrogen, and put

    this white substance from the zinc into it, look how beautifully it glows,

    and just because it is a solid substance.

    I will now take such a flame as I had a moment since, and set free from it

    the particles of carbon. Here is some camphine, which will burn with a

    smoke; but if I send these particles of smoke through this pipe into the

    hydrogen flame, you will see they will burn and become luminous, because

    we heat them a second time. There they are. Those are the particles of

    carbon re-ignited a second time. They are those particles which you can

    easily see by holding a piece of paper behind them, and which, whilst they

    are in the flame, are ignited by the heat produced, and, when so ignited,

    produce this brightness. When the particles are not separated, you get no

    brightness. The flame of coal-gas owes its brightness to the separation,

    during combustion, of these particles of carbon, which are equally in that

    as in a candle. I can very quickly alter that arrangement. Here, for

    instance, is a bright flame of gas. Supposing I add so much air to the

    flame as to cause it all to burn before those particles are set free, I

    shall not have this brightness; and I can do that in this way:–If I place

    over the jet this wire-gauze cap, as you see, and then light the gas over

    it, it burns with a non-luminous flame, owing to its having plenty of air

    mixed with it before it burns; and if I raise the gauze, you see it does

    not burn below[10]. There is plenty of carbon in the gas; but, because the

    atmosphere can get to it, and mix with it before it burns, you see how

    pale and blue the flame is. And if I blow upon a bright gas-flame, so as

    to consume all this carbon before it gets heated to the glowing point, it

    will also burn blue: [The Lecturer illustrated his remarks by blowing on

    the gas-light.] The only reason why I have not the same bright light when

    I thus blow upon the flame is, that the carbon meets with sufficient air

    to burn it before it gets separated in the flame in a free state. The

    difference is solely due to the solid particles not being separated before

    the gas is burnt.

    You observe that there are certain products as the result of the

    combustion of a candle, and that of these products one portion may be

    considered as charcoal, or soot; that charcoal, when afterwards burnt,

    produces some other product; and it concerns us very much now to ascertain

    what that other product is. We shewed that something was going away; and I

    want you now to understand how much is going up into the air; and for that

    purpose we will have combustion on a little larger scale. From that candle

    ascends heated air, and two or three experiments will shew you the

    ascending current; but, in order to give you a notion of the quantity of

    matter which ascends in this way, I will make an experiment by which I

    shall try to imprison some of the products of this combustion. For this

    purpose I have here what boys call a fire-balloon. I use this fire-balloon

    merely as a sort of measure of the result of the combustion we are

    considering; and I am about to make a flame in such an easy and simple

    manner as shall best serve my present purpose. This plate shall be the

    “cup,” we will so say, of the candle; this spirit shall be our fuel; and I

    am about to place this chimney over it, because it is better for me to do

    so than to let things proceed at random.

    [Illustration: Fig. 10.]

    Mr. Anderson will now light the fuel, and here at the top we shall get the

    results of the combustion. What we get at the top of that tube is exactly

    the same, generally speaking, as you get from the combustion of a candle;

    but we do not get a luminous flame here, because we use a substance which

    is feeble in carbon. I am about to put this balloon–not into action,

    because that is not my object–but to shew you the effect which results

    from the action of those products which arise from the candle, as they

    arise here from the furnace. [The balloon was held over the chimney, when

    it immediately commenced to fill.] You see how it is disposed to ascend;

    but we must not let it up, because it might come in contact with those

    upper gas-lights, and that would be very inconvenient. [The upper

    gas-lights were turned out, at the request of the Lecturer, and the

    balloon was allowed to ascend.] Does not that shew you what a large bulk

    of matter is being evolved? Now, there is going through this tube [placing

    a large glass tube over a candle] all the products of that candle, and you

    will presently see that the tube will become quite opaque. Suppose I take

    another candle, and place it under a jar, and then put a light on the

    other side, just to shew you what is going on. You see that the sides of

    the jar become cloudy, and the light begins to burn feebly. It is the

    products, you see, which make the light so dim, and this is the same thing

    which makes the sides of the jar so opaque. If you go home and take a

    spoon that has been in the cold air, and hold it over a candle–not so as

    to soot it–you will find that it becomes dim, just as that jar is dim. If

    you can get a silver dish, or something of that kind, you will make the

    experiment still better. And now, just to carry your thoughts forward to

    the time we shall next meet, let me tell you that it is _water_ which

    causes the dimness; and when we next meet. I will shew you that we can

    make it, without difficulty, assume the form of a liquid.




    I dare say you will remember that when we parted we had just mentioned the

    word “products” from the candle. For when a candle burns we found we were

    able, by nice adjustment, to get various products from it. There was one

    substance which was not obtained when the candle was burning properly,

    which was charcoal or smoke; and there was some other substance that went

    upwards from the flame which did not appear as smoke, but took some other

    form, and made part of that general current which, ascending from the

    candle upwards, becomes invisible, and escapes. There were also other

    products to mention. You remember that in that rising current having its

    origin at the candle, we found that one part was condensable against a

    cold spoon, or against a clean plate, or any other cold thing, and another

    part was incondensable.

    We will first take the condensable part, and examine it; and, strange to

    say, we find that that part of the product is just water–nothing but

    water. On the last occasion I spoke of it incidentally, merely saying that

    water was produced among the condensable products of the candle; but

    to-day I wish to draw your attention to water, that we may examine it

    carefully, especially in relation to this subject, and also with respect

    to its general existence on the surface of the globe.

    Now, having previously arranged an experiment for the purpose of

    condensing water from the products of the candle, my next point will be to

    shew you this water; and perhaps one of the best means that I can adopt

    for shewing its presence to so many at once, is to exhibit a very visible

    action of water, and then to apply that test to what is collected as a

    drop at the bottom of that vessel. I have here a chemical substance,

    discovered by Sir Humphrey Davy, which has a very energetic action upon

    water, which I shall use as a test of the presence of water. If I take a

    little piece of it–it is called potassium, as coming from potash,–if I

    take a little piece of it, and throw it into that basin, you see how it

    shews the presence of water by lighting up and floating about, burning

    with a violent flame. I am now going to take away the candle which has

    been burning beneath the vessel containing ice and salt, and you see a

    drop of water–a condensed product of the candle–hanging from under the

    surface of the dish.

    [Illustration: Fig. 11.]

    I will shew you that potassium has the same action upon it as upon the

    water in that basin in the experiment we have just tried. See, it takes

    fire, and burns in just the same manner. I will take another drop upon

    this glass slab, and when I put the potassium on to it, you see at once,

    from its taking fire, that there is water present. Now, that water was

    produced by the candle. In the same manner, if I put this spirit-lamp

    under that jar, you will soon see the latter become damp, from the dew

    which is deposited upon it–that dew being the result of combustion; and I

    have no doubt you will shortly see by the drops of water which fall upon

    the paper below, that there is a good deal of water produced from the

    combustion of the lamp. I will let it remain, and you can afterwards see

    how much water has been collected. So, if I take a gas-lamp, and put any

    cooling arrangement over it, I shall get water–water being likewise

    produced from the combustion of gas. Here, in this bottle, is a quantity

    of water–perfectly pure, distilled water, produced from the combustion of

    a gas-lamp–in no point different from the water that you distil from the

    river, or ocean, or spring, but exactly the same thing. Water is one

    individual thing–it never changes. We can add to it by careful

    adjustment, for a little while, or we can take it apart, and get other

    things from it; but water, as water, remains always the same, either in a

    solid, liquid, or fluid state. Here, again [holding another bottle], is

    some water produced by the combustion of an oil-lamp. A pint of oil, when

    burnt fairly and properly, produces rather more than a pint of water.

    Here, again, is some water, produced by a rather long experiment from a

    wax candle. And so we can go on with almost all combustible substances,

    and find that if they burn with a flame, as a candle, they produce water.

    You may make these experiments yourselves. The head of a poker is a very

    good thing to try with, and if it remains cold long enough over the

    candle, you may get water condensed in drops on it; or a spoon or ladle,

    or anything else may be used, provided it be clean, and can carry off the

    heat, and so condense the water.

    And now–to go into the history of this wonderful production of water from

    combustibles, and by combustion–I must first of all tell you that this

    water may exist in different conditions; and although you may now be

    acquainted with all its forms, they still require us to give a little

    attention to them for the present, so that we may perceive how the water,

    whilst it goes through its Protean changes, is entirely and absolutely the

    same thing, whether it is produced from a candle, by combustion, or from

    the rivers or ocean.

    First of all, water, when at the coldest, is ice. Now, we philosophers—I

    hope that I may class you and myself together in this case–speak of water

    as water, whether it be in its solid, or liquid, or gaseous state,–we

    speak of it chemically as water. Water is a thing compounded of two

    substances, one of which we have derived from the candle, and the other we

    shall find elsewhere. Water may occur as ice; and you have had most

    excellent opportunities lately of seeing this. Ice changes back into

    water–for we had on our last Sabbath a strong instance of this change, by

    the sad catastrophe which occurred in our own house, as well as in the

    houses of many of our friends,–ice changes back into water when the

    temperature is raised: water also changes into steam when it is warmed

    enough. The water which we have here before us is in its densest

    state[11], and although it changes in weight, in condition, in form, and

    in many other qualities, it still is water; and whether we alter it into

    ice by cooling, or whether we change it into steam by heat, it increases

    in volume,–in the one case very strangely and powerfully, and in the

    other case very largely and wonderfully. For instance, I will now take

    this tin cylinder, and pour a little water into it; and seeing how much

    water I pour in, you may easily estimate for yourselves how high it will

    rise in the vessel: it will cover the bottom about two inches. I am now

    about to convert the water into steam, for the purpose of shewing to you

    the different volumes which water occupies in its different states of

    water and steam.

    Let us now take the case of water changing into ice: we can effect that by

    cooling it in a mixture of salt and pounded ice[12]; and I shall do so to

    shew you the expansion of water into a thing of larger bulk when it is so

    changed. These bottles [holding one] are made of strong cast iron, very

    strong and very thick–I suppose they are the third of an inch in

    thickness; they are very carefully filled with water, so as to exclude all

    air, and then they are screwed down tight. We shall see that when we

    freeze the water in these iron vessels, they will not be able to hold the

    ice, and the expansion within them will break them in pieces as these

    [pointing to some fragments] are broken, which have been bottles of

    exactly the same kind. I am about to put these two bottles into that

    mixture of ice and salt, for the purpose of shewing that when water

    becomes ice, it changes in volume in this extraordinary way.

    In the mean time look at the change which has taken place in the water to

    which we have applied heat–it is losing its fluid state. You may tell

    this by two or three circumstances. I have covered the mouth of this glass

    flask, in which water is boiling, with a watch-glass. Do you see what

    happens? It rattles away like a valve chattering, because the steam rising

    from the boiling water sends the valve up and down, and forces itself out,

    and so makes it clatter. You can very easily perceive that the flask is

    quite full of steam, or else it would not force its way out. You see,

    also, that the flask contains a substance very much larger than the water,

    for it fills the whole of the flask over and over again, and there it is

    blowing away into the air; and yet you cannot observe any great diminution

    in the bulk of the water, which shews you that its change of bulk is very

    great when it becomes steam.

    I have put our iron bottles containing water into this freezing mixture,

    that you may see what happens. No communication will take place, you

    observe, between the water in the bottles and the ice in the outer vessel.

    But there will be a conveyance of heat from the one to the other; and if

    we are successful–we are making our experiment in very great haste–I

    expect you will by-and-by, so soon as the cold has taken possession of the

    bottles and their contents, hear a pop on the occasion of the bursting of

    the one bottle or the other; and, when we come to examine the bottles, we

    shall find their contents masses of ice, partly enclosed by the covering

    of iron which is too small for them, because the ice is larger in bulk

    than the water. You know very well that ice floats upon water: if a boy

    falls through a hole into the water, he tries to get on the ice again to

    float him up. Why does the ice float?–think of that, and philosophise.

    Because the ice is larger than the quantity of water which can produce it;

    and therefore the ice weighs the lighter, and the water is the heavier.

    To return now to the action of heat on water. See what a stream of vapour

    is issuing from this tin vessel! You observe, we must have made it quite

    full of steam to have it sent out in that great quantity. And now, as we

    can convert the water into steam by heat, we convert it back into liquid

    water by the application of cold. And if we take a glass, or any other

    cold thing, and hold it over this steam, see how soon it gets damp with

    water; it will condense it until the glass is warm–it condenses the water

    which is now running down the sides of it.  I have here another experiment

    to shew the condensation of water from a vaporous state back into a liquid

    state, in the same way as the vapour, one of the products of the candle,

    was condensed against the bottom of the dish, and obtained in the form of

    water; and to shew you how truly and thoroughly these changes take place,

    I will take this tin flask, which is now full of steam, and close the top.

    We shall see what takes place when we cause this water or steam to return

    back to the fluid state by pouring some cold water on the outside. [The

    Lecturer poured the cold water over the vessel, when it immediately

    collapsed.]  You see what has happened.  If I had closed the stopper, and

    still kept the heat applied to it, it would have burst the vessel; yet,

    when the steam returns to the state of water, the vessel collapses, there

    being a vacuum produced inside by the condensation of the steam. I shew

    you these experiments for the purpose of pointing out that in all these

    occurrences there is nothing that changes the water into any other

    thing–it still remains water; and so the vessel is obliged to give way,

    and is crushed inwards, as in the other case, by the further application

    of heat, it would have been blown outwards.

    [Illustration: Fig. 12.]

    And what do you think the bulk of that water is when it assumes the

    vaporous condition? You see that cube [pointing to a cubic foot]. There,

    by its side, is a cubic inch, exactly the same shape as the cubic foot,

    and that bulk of water [the cubic inch] is sufficient to expand into that

    bulk [the cubic foot] of steam; and, on the contrary, the application of

    cold will contract that large quantity of steam into this small quantity

    of water.

    [Illustration: Fig. 13.]

    [One of the iron bottles burst at that moment.] Ah! There is one of our

    bottles burst, and here you see is a crack down one side an eighth of an

    inch in width. [The other now exploded, sending the freezing mixture in

    all directions.] This other bottle is also broken; although the iron was

    nearly half-an-inch thick, the ice has burst it asunder. These changes

    always take place in water: they do not require to be always produced by

    artificial means,–we only use them here because we want to produce a

    small winter round that little bottle, instead of a long and severe one.

    But if you go to Canada, or to the North, you will find the temperature

    there out of doors will do the same thing as has been done here by the

    freezing mixture.

    To return to our quiet philosophy. We shall not in future be deceived,

    therefore, by any changes that are produced in water. Water is the same

    everywhere, whether produced from the ocean or from the flame of the

    candle. Where, then, is this water which we get from a candle? I must

    anticipate a little, and tell you. It evidently comes, as to part of it,

    from the candle; but is it within the candle beforehand? No. It is not in

    the candle; and it is not in the air round about the candle which is

    necessary for its combustion. It is neither in one nor the other, but it

    comes from their conjoint action, a part from the candle, a part from the

    air; and this we have now to trace, so that we may understand thoroughly

    what is the chemical history of a candle when we have it burning on our

    table. How shall we get at this? I myself know plenty of ways, but I want

    _you_ to get at it from the association in your own minds of what I have

    already told you.

    I think you can see a little in this way. We had just now the case of a

    substance which acted upon the water in the way that Sir Humphrey Davy

    shewed us[13], and which I am now going to recall to your minds by making

    again an experiment upon that dish. It is a thing which we have to handle

    very carefully, for you see, if I allow a little splash of water to come

    upon this mass, it sets fire to part of it; and if there were free access

    of air, it would quickly set fire to the whole. Now, this is a metal–a

    beautiful and bright metal–which rapidly changes in the air, and, as you

    know, rapidly changes in water. I will put a piece on the water, and you

    see it burns beautifully, making a floating lamp, using the water in the

    place of air. Again, if we take a few iron filings or turnings, and put

    them in water, we find that they likewise undergo an alteration. They do

    not change so much as this potassium does, but they change somewhat in the

    same way; they become rusty, and shew an action upon the water, though in

    a different degree of intensity to what this beautiful metal does: but

    they act upon the water in the same manner generally as this potassium. I

    want you to put these different facts together in your minds. I have

    another metal here [zinc], and when we examined it with regard to the

    solid substance produced by its combustion, we had an opportunity of

    seeing that it burned; and I suppose, if I take a little strip of this

    zinc and put it over the candle, you will see something half-way, as it

    were, between the combustion of potassium on the water and the action of

    iron,–you see there is a sort of combustion. It has burned, leaving a

    white ash or residuum, and here also we find that the metal has a certain

    amount of action upon water.

    By degrees we have learned how to modify the action of these different

    substances, and to make them tell us what we want to know. And now, first

    of all, I take iron. It is a common thing in all chemical reactions, where

    we get any result of this kind, to find that it is increased by the action

    of heat; and if we want to examine minutely and carefully the action of

    bodies one upon another, we often have to refer to the action of heat. You

    are aware, I believe, that iron-filings burn beautifully in the air; but I

    am about to shew you an experiment of this kind, because it will impress

    upon you what I am going to say about iron in its action on water. If I

    take a flame and make it hollow;–you know why, because I want to get air

    to it and into it, and therefore I make it hollow–and then take a few

    iron-filings and drop them into the flame, you see how well they burn.

    That combustion results from the chemical action which is going on when we

    ignite those particles. And so we proceed to consider these different

    effects, and ascertain what iron will do when it meets with water. It will

    tell us the story so beautifully, so gradually and regularly, that I think

    it will please you very much.

    I have here a furnace with a pipe going through it like an iron

    gun-barrel, and I have stuffed that barrel full of bright iron-turnings,

    and placed it across the fire, to be made red-hot. We can either send air

    through the barrel to come in contact with the iron, or we can send steam

    from this little boiler at the end of the barrel. Here is a stop-cock

    which shuts off the steam from the barrel until we wish to admit it. There

    is some water in these glass jars, which I have coloured blue, so that you

    may see what happens. Now, you know very well that any steam I might send

    through that barrel, if it went through into the water, would be

    condensed; for you have seen that steam cannot retain its gaseous form if

    it be cooled down.

    [Illustration: Fig. 14.]

    You saw it here [pointing to the tin flask] crushing itself into a small

    bulk, and causing the flask holding it to collapse; so that if I were to

    send steam through that barrel, it would be condensed–supposing the

    barrel were cold: it is, therefore, heated to perform the experiment I am

    now about to shew you. I am going to send the steam through the barrel in

    small quantities; and you shall judge for yourselves, when you see it

    issue from the other end, whether it still remains steam. Steam is

    condensible into water, and when you lower the temperature of steam, you

    convert it back into fluid water; but I have lowered the temperature of

    the gas which I have collected in this jar, by passing it through water

    after it has traversed the iron barrel, and still it does not change back

    into water. I will take another test and apply to this gas. (I hold the

    jar in an inverted position, or my substance would escape.) If I now apply

    a light to the mouth of the jar, it ignites with a slight noise. That

    tells you that it is not steam. Steam puts out a fire–it does not burn;

    but you saw that what I had in that jar burnt. We may obtain this

    substance equally from water produced from the candle-flame as from any

    other source. When it is obtained by the action of the iron upon the

    aqueous vapour, it leaves the iron in a state very similar to that in

    which these filings were after they were burnt. It makes the iron heavier

    than it was before. So long as the iron remains in the tube and is heated,

    and is cooled again without the access of air or water, it does not change

    in its weight; but after having had this current of steam passed over it,

    it then comes out heavier that it was before, having taken something out

    of the steam, and having allowed something else to pass forth, which we

    see here. And now, as we have another jar full, I will shew you something

    most interesting. It is a combustible gas; and I might at once take this

    jar and set fire to the contents, and shew you that it is combustible; but

    I intend to shew you more if I can. It is also a very light substance.

    Steam will condense: this body will rise in the air, and not condense.

    [Illustration: Fig. 15]

    Suppose I take another glass jar, empty of all but air: if I examine it

    with a taper, I shall find that it contains nothing but air. I will now

    take this jar full of the gas that I am speaking of, and deal with it as

    though it were a light body. I will hold both upside-down, and turn the

    one up under the other; and that which did contain the gas procured from

    the steam, what does it contain now? You will find it now only contains

    air. But look! Here is the combustible substance [taking the other jar]

    which I have poured out of the one jar into the other. It still preserves

    its quality, and condition, and independence, and therefore is the more

    worthy of our consideration, as belonging to the products of a candle.

    Now, this substance which we have just prepared by the action of iron on

    the steam or water, we can also get by means of those other things which

    you have already seen act so well upon the water. If I take a piece of

    potassium, and make the necessary arrangements, it will produce this gas;

    and if, instead, a piece of zinc, I find, when I come to examine it very

    carefully, that the main reason why this zinc cannot act upon the water

    continuously as the other metal does, is because the result of the action

    of the water envelopes the zinc in a kind of protecting coat. We have

    learned in consequence, that if we put into our vessel only the zinc and

    water, they by themselves do not give rise to much action, and we get no

    result. But suppose I proceed to dissolve off this varnish–this

    encumbering substance–which I can do by a little acid; the moment I do

    this, I find the zinc acting upon the water exactly as the iron did, but

    at the common temperature. The acid in no way is altered, except in its

    combination with the oxide of zinc, which is produced. I have now poured

    the acid into the glass, and the effect is as though I were applying heat

    to cause this boiling up. There is something coming off from the zinc very

    abundantly, which is not steam. There is a jar full of it; and you will

    find that I have exactly the same combustible substance remaining in the

    vessel, when I hold it upside-down, that I produced during the experiment

    with the iron barrel. This is what we get from water–the same substance

    which is contained in the candle.

    [Illustration: Fig. 16.]

    Let us now trace distinctly the connection between these two points. This

    is hydrogen–a body classed among those things which in Chemistry we call

    elements, because we can get nothing else out of them. A candle is not an

    elementary body, because we can get carbon out of it; we can get this

    hydrogen out of it, or at least out of the water which it supplies. And

    this gas has been so named hydrogen, because it is that element which, in

    association with another, generates water. [Footnote: [greek: hudos],

    “water,” and [greek: gennao], “I generate.”] Mr. Anderson having now


    able to get two or three jars of gas, we shall have a few experiments to

    make, and I want to shew you the best way of making these experiments. I

    am not afraid to shew you, for I wish you to make experiments, if you will

    only make them with care and attention, and the assent of those around

    you. As we advance in Chemistry, we are obliged to deal with substances

    which are rather injurious, if in their wrong places–the acids, and heat,

    and combustible things we use, might do harm if carelessly employed. If

    you want to make hydrogen, you can make it easily from bits of zinc, and

    sulphuric or muriatic acid. Here is what in former times was called the

    “philosopher’s candle.” It is a little phial with a cork, and a tube or

    pipe passing through it.

    [Illustration: Fig. 17.]

    And I am now putting a few little pieces of zinc into it. This little

    instrument I am going to apply to a useful purpose in our

    demonstrations–for I want to shew you that you can prepare hydrogen, and

    make some experiments with it as you please at your own homes. Let me here

    tell you why I am so careful to fill this phial nearly, and yet not quite

    full. I do it because the evolved gas, which, as you have seen, is very

    combustible, is explosive to a considerable extent when mixed with air,

    and might lead to harm, if you were to apply a light to the end of that

    pipe before all the air had been swept out of the space above the water. I

    am now about to pour in the sulphuric acid. I have used very little zinc,

    and more sulphuric acid and water, because I want to keep it at work for

    some time. I therefore take care in this way to modify the proportions of

    the ingredients, so that I may have a regular supply–not too quick, and

    not too slow. Supposing I now take a glass and put it upside-down over the

    end of the tube, because the hydrogen is light I expect that it will

    remain in that vessel a little while. We will now test the contents of our

    glass to see if there be hydrogen in it. I think I am safe in saying we

    have caught some [applying a light]. There it is, you see. I will now

    apply a light to the top of the tube. There is the hydrogen burning. There

    is our philosophical candle. It is a foolish feeble sort of a flame, you

    may say; but it is so hot that scarcely any common flame gives out so much

    heat. It goes on burning regularly, and I am now about to put that flame

    to burn under a certain arrangement, in order that we may examine its

    results and make use of the information which we may thereby acquire.

    Inasmuch as the candle produces water, and this gas comes out of the

    water, let us see what this gives us by the same process of combustion

    that the candle went through when it burnt in the atmosphere; and for that

    purpose I am going to put the lamp under this apparatus, in order to

    condense whatever may arise from the combustion within it In the course of

    a short time you will see moisture appearing in the cylinder, and you will

    get the water running down the side; and the water from this hydrogen

    flame will have absolutely the same effect upon all our tests, being

    obtained by the same general process as in the former case. This hydrogen

    is a very beautiful substance. It is so light that it carries things up:

    it is far lighter than the atmosphere; and I dare say I can shew you this

    by an experiment which, if you are very clever, some of you may even have

    skill enough to repeat. Here is our generator of hydrogen, and here are

    some soap-suds. I have an india-rubber tube connected with the hydrogen

    generator, and at the end of the tube is a tobacco-pipe.

    [Illustration: Fig. 18.]

    I can thus put the pipe into the suds, and blow bubbles by means of the

    hydrogen. You observe how the bubbles fall downwards when I blow them with

    my warm breath; but notice the difference when I blow them with hydrogen.

    [The Lecturer here blew bubbles with hydrogen, which rose to the roof of

    the theatre.] It shews you how light this gas must be in order to carry

    with it not merely the ordinary soap-bubble, but the larger portion of a

    drop hanging to the bottom of it. I can shew its lightness in a better way

    than this; larger bubbles than these may be so lifted up; indeed, in

    former times balloons used to be filled with this gas. Mr. Anderson will

    fasten this tube on to our generator, and we shall have a stream of

    hydrogen here with which we can charge this balloon made of collodion. I

    need not even be very careful to get all the air out, for I know the power

    of this gas to carry it up. [Two collodion balloons were inflated, and

    sent up, one being held by a string.] Here is another larger one made of

    thin membrane, which we will fill and allow to ascend. You will see they

    will all remain floating about until the gas escapes.

    What, then, are the comparative weights of these substances? I have a

    table here which will shew you the proportion which their weights bear to

    each other. I have taken a pint and a cubic foot as the measures, and have

    placed opposite to them the respective figures. A pint measure of this

    hydrogen weighs three-quarters of our smallest weight (a grain), and a

    cubic foot weighs one-twelfth of an ounce; whereas a pint of water weighs

    8,750 grains, and a cubic foot of water weighs almost 1,000 ounces. You

    see, therefore, what a vast difference there is between the weight of a

    cubic foot of water and a cubic foot of hydrogen.

    Hydrogen gives rise to no substance that can become solid, either during

    combustion or afterwards as a product of its combustion. But when it

    burns, it produces water only; and if we take a cold glass and put it over

    the flame, it becomes damp, and you have water, produced immediately in

    appreciable quantity; and nothing is produced by its combustion but the

    same water which you have seen the flame of the candle produce. It is

    important to remember that this hydrogen is the only thing in nature which

    furnishes water as the sole product of combustion.

    And now we must endeavour to find some additional proof of the general

    character and composition of water; and for this purpose I will keep you a

    little longer, so that at our next meeting we may be better prepared for

    the subject. We have the power of arranging the zinc which you have seen

    acting upon the water by the assistance of an acid, in such a manner as to

    cause all the power to be evolved in the place where we require it I have

    behind me a voltaic pile, and I am just about to shew you, at the end of

    this lecture, its character and power, that you may see what we shall have

    to deal with when next we meet. I hold here the extremities of the wires

    which transport the power from behind me, and which I shall cause to act

    on the water.

    We have previously seen what a power of combustion is possessed by the

    potassium, or the zinc, or the iron-filings; but none of them shew such

    energy as this. [The Lecturer here made contact between the two terminal

    wires of the battery, when a brilliant flash of light was produced.] This

    light is, in fact, produced by a forty-zinc power of burning: it is a

    power that I can carry about in my hands, through these wires, at

    pleasure–although, if I applied it wrongly to myself, it would destroy me

    in an instant, for it is a most intense thing, and the power you see here

    put forth while you count five [bringing the poles in contact, and

    exhibiting the electric light] is equivalent to the power of several

    thunder-storms, so great is its force[14]. And that you may see what

    intense energy it has, I will take the ends of the wires which convey the

    power from the battery, and with it I dare say I can burn this iron file.

    Now, this is a chemical power, and one which, when we next meet, I shall

    apply to water, and shew you what results we are able to produce.



    I see you are not tired of the candle yet, or I am sure you would not be

    interested in the subject in the way you are. When our candle was burning,

    we found it produced water exactly like the water we have around us; and

    by further examination of this water we found in it that curious body,

    hydrogen–that light substance of which there is some in this jar. We

    afterwards saw the burning powers of that hydrogen, and that it produced

    water. And I think I introduced to your notice an apparatus which I very

    briefly said was an arrangement of chemical force, or power, or energy, so

    adjusted as to convey its power to us in these wires; and I said I should

    use that force to pull the water to pieces, to see what else there was in

    the water besides hydrogen; because, you remember, when we passed the

    water through the iron tube, we by no means got the weight of water back

    which we put in, in the form of steam, though we had a very large quantity

    of gas evolved. We have now to see what is the other substance present.

    That you may understand the character and use of this instrument, let us

    make an experiment or two. Let us put together, first of all, some

    substances, knowing what they are, and then see what that instrument does

    to them. There is some copper (observe the various changes which it can

    undergo), and here is some nitric acid, and you will find that this, being

    a strong chemical agent, will act very powerfully when I add it to the

    copper. It is now sending forth a beautiful red vapour; but as we do not

    want that vapour, Mr. Anderson will hold it near the chimney for a short

    time, that we may have the use and beauty of the experiment without the

    annoyance. The copper which I have put into the flask will dissolve: it

    will change the acid and the water into a blue fluid, containing copper

    and other things; and I propose then shewing you how this voltaic battery

    deals with it; and in the mean-time we will arrange another kind of

    experiment for you to see what power it has. This is a substance which is

    to us like water–that is to say, it contains bodies which we do not know

    of as yet, as water contains a body which we do not know as yet. Now, this

    solution of a salt[15] I will put upon paper, and spread about, and apply

    the power of the battery to it, and observe what will happen. Three or

    four important things will happen which we shall take advantage of. I

    place this wetted paper upon a sheet of tinfoil, which is convenient for

    keeping all clean, and also for the advantageous application of the power;

    and this solution, you see, is not at all affected by being put upon the

    paper or tinfoil, nor by anything else I have brought in contact with it

    yet, and which, therefore, is free to us to use as regards that

    instrument. But first let us see that our instrument is in order. Here are

    our wires. Let us see whether it is in the state in which it was last

    time. We can soon tell. As yet, when I bring them together, we have no

    power, because the conveyers–what we call the electrodes–the passages or

    ways for the electricity–are stopped; but now Mr. Anderson by that

    [referring to a sudden flash at the ends of the wires] has given me a

    telegram to say that it is ready. Before I begin our experiment I will get

    Mr. Anderson to break contact again at the battery behind me, and we will

    put a platinum-wire across to connect the poles, and then if I find I can

    ignite a pretty good length of this wire, we shall be safe in our

    experiment. Now you will see the power. [The connection was established,

    and the intermediate wire became red-hot.] There is the power running

    beautifully through the wire, which I have made thin on purpose to shew

    you that we have those powerful forces; and now, having that power, we

    will proceed with it to the examination of water.

    I have here two pieces of platinum, and if I lay them down upon this piece

    of paper [the moistened paper on the tinfoil], you will see no action; and

    if I take them up, there is no change that you can see, but the

    arrangement remains just as it was before. But, now, see what happens: if

    I take these two poles and put either one or the other of them down

    separately on the platinum-plates, they do nothing for me, both are

    perfectly without action; but if I let them both be in contact at the same

    moment, see what happens [a brown spot appeared under each pole of the

    battery]. Look here at the effect that takes place, and see how I have

    pulled something apart from the white–something brown; and I have no

    doubt, if I were to arrange it thus, and were to put one of the poles to

    the tinfoil on the other side of the paper–why, I get such a beautiful

    action upon the paper, that I am going to see whether I cannot write with

    it–a telegram, if you please. [The Lecturer here traced the word

    “juvenile” on the paper with one of the terminal wires.] See there how

    beautifully we can get our results!

    You see we have here drawn something, which we have not known about

    before, out of this solution. Let us now take that flask from Mr.

    Andersen’s hands, and see what we can draw out of that. This, you know, is

    a liquid which we have just made up from copper and nitric acid, whilst

    our other experiments were in hand; and though I am making this experiment

    very hastily, and may bungle a little, yet I prefer to let you see what I

    do rather than prepare it beforehand.

    Now, see what happens. These two platinum-plates are the two ends (or I

    will make them so immediately) of this apparatus; and I am about to put

    them in contact with that solution just as we did a moment ago on the

    paper. It does not matter to us whether the solution be on the paper or

    whether it be in the jar, so long as we bring the ends of the apparatus to

    it. If I put the two platinums in by themselves, they come out as clean

    and as white as they go in [inserting them into the fluid without

    connecting them with the battery]; but when we take the power and lay that

    on [the platinums were connected with the battery and again dipped into

    the solution], this, you see [exhibiting one of the platinums], is at once

    turned into copper, as it were: it has become like a plate of copper; and

    that [exhibiting the other piece of platinum] has come out quite clean. If

    I take this coppered piece and change sides, the copper will leave the

    right-hand side and come over to the left side; what was before the

    coppered plate comes out clean, and the plate which was clean comes out

    coated with copper; and thus you see that the same copper we put into this

    solution we can also take out of it by means of this instrument.

    Putting that solution aside, let us now see what effect this instrument

    will have upon water. Here are two little platinum-plates which I intend

    to make the ends of the battery, and this (C) is a little vessel so shaped

    as to enable me to take it to pieces, and shew you its construction. In

    these two cups (A and B) I pour mercury, which touches the ends of the

    wires connected with the platinum-plates. In the vessel (C) I pour some

    water containing a little acid (but which is put only for the purpose of

    facilitating the action; it undergoes no change in the process), and

    connected with the top of the vessel is a bent glass tube (D), which may

    remind you of the pipe which was connected with the gun barrel in our

    furnace experiment, and which now passes under the jar (F).  I have now

    adjusted this apparatus, and we will proceed to affect the water in some

    way or other. In the other case, I sent the water through a tube which was

    made red-hot; I am now going to pass the electricity through the contents

    of this vessel.  Perhaps I may boil the water; if I do boil the water, I

    shall get steam; and you know that steam condenses when it gets cold, and

    you will therefore see by that whether I do boil the water or not.

    Perhaps, however, I shall not boil the water, but produce some other

    effect.  You shall have the experiment and see. There is one wire which I

    will put to this side (A), and here is the other wire which I will put to

    the other side (B), and you will soon see whether any disturbance takes

    place. Here it is seeming to boil up famously; but does it boil? Let us

    see whether that which goes out is steam or not. I think you will soon see

    the jar (F) will be filled with vapour, if that which rises from the water

    is steam. But can it be steam? Why, certainly not; because there it

    remains, you see, unchanged.  There it is standing over the water, and it

    cannot therefore be steam, but must be a permanent gas of some sort What

    is it? Is it hydrogen? Is it anything else? Well, we will examine it. If

    it is hydrogen, it will burn. [The Lecturer then ignited a portion of the

    gas collected, which burnt with an explosion.]

    [Illustration: Fig. 19]

    It is certainly something combustible, but not combustible in the way that

    hydrogen is. Hydrogen would not have given you that noise; but the colour

    of that light, when the thing did burn, was like that of hydrogen: it

    will, however, burn without contact with the air. That is why I have

    chosen this other form of apparatus, for the purpose of pointing out to

    you what are the particular circumstances of this experiment. In place of

    an open vessel I have taken one that is closed (our battery is so

    beautifully active that we are even boiling the mercury, and getting all

    things right–not wrong, but vigorously right); and I am going to shew you

    that that gas, whatever it may be, can burn without air, and in that

    respect differs from a candle, which cannot burn without the air. And our

    manner of doing this is as follows:–I have here a glass vessel (G) which

    is fitted with two platinum-wires (IK), through which I can apply

    electricity; and we can put the vessel on the air-pump and exhaust the

    air, and when we have taken the air out we can bring it here and fasten it

    on to this jar (F), and let into the vessel that gas which was formed by

    the action of the voltaic battery upon the water, and which we have

    produced by changing the water into it,–for I may go as far as this, and

    say we have really, by that experiment, changed the water into that gas.

    We have not only altered its condition, but we have changed it really and

    truly into that gaseous substance, and all the water is there which was

    decomposed by the experiment. As I screw this vessel (GH) on here (H), and

    make the tubes well connected, and when I open the stop-cocks (HHH), if

    you watch the level of the water (in F), you will see that the gas will

    rise. I will now close the stop-cocks, as I have drawn up as much as the

    vessel can hold, and being safely conveyed into that chamber, I will pass

    into it an electric spark from this Leyden jar (L), when the vessel, which

    is now quite clear and bright, will become dim. There will be no sound,

    for the vessel is strong enough to confine the explosion. [A spark was

    then passed through the jar, when the explosive mixture was ignited.] Did

    you see that brilliant light? If I again screw the vessel on to the jar,

    and open these stop-cocks, you will see that the gas will rise a second

    time. [The stop-cocks were then opened.] Those gases [referring to the

    gases first collected in the jar, and which had just been ignited by the

    electric spark] have disappeared, as you see: their place is vacant, and

    fresh gas has gone in. Water has been formed from them; and if we repeat

    our operation [repeating the last experiment], I shall have another

    vacancy, as you will see by the water rising. I always have an empty

    vessel after the explosion, because the vapour or gas into which that

    water has been resolved by the battery explodes under the influence of the

    spark, and changes into water; and by-and-by you will see in this upper

    vessel some drops of water trickling down the sides and collecting at the


    We are here dealing with water entirely, without reference to the

    atmosphere. The water of the candle had the atmosphere helping to produce

    it; but in this way it can be produced independently of the air. Water,

    therefore, ought to contain that other substance which the candle takes

    from the air, and which, combining with the hydrogen, produces water.

    Just now you saw that one end of this battery took hold of the copper,

    extracting it from the vessel which contained the blue solution. It was

    effected by this wire; and surely we may say, if the battery has such

    power with a metallic solution which we made and unmade, may we not find

    that it is possible to split asunder the component parts of the water, and

    put them into this place and that place? Suppose I take the poles–the

    metallic ends of this battery–and see what will happen with the water in

    this apparatus (fig. 20), where we have separated the two ends far apart.

    [Illustration: Fig. 20.]

    I place one here (at A), and the other there (at B), and I have little

    shelves with holes which I can put upon each pole, and so arrange them

    that whatever escapes from the two ends of the battery will appear as

    separate gases; for you saw that the water did not become vaporous, but

    gaseous. The wires are now in perfect and proper connection with the

    vessel containing the water; and you see the bubbles rising: let us

    collect these bubbles and see what they are. Here is a glass cylinder (O);

    I fill it with water and put it over one end (A) of the pile; and I will

    take another (H) and put it over the other end (B) of the pile. And so now

    we have a double apparatus, with both places delivering gas.  Both these

    jars will fill with gas. There they go, that to the right (H) filling very

    rapidly; the one to the left (O) filling not so rapidly; and though I have

    allowed some bubbles to escape, yet still the action is going on pretty

    regularly; and were it not that one is rather smaller than the other, you

    would see that I should have twice as much in this (H) as I have in that

    (O).  Both these gases are colourless; they stand over the water without

    condensing; they are alike in all things–I mean in all _apparent_ things;

    and we have here an opportunity of examining these bodies and ascertaining

    what they are. Their bulk is large, and we can easily apply experiments to

    them. I will take this jar (H) first, and will ask you to be prepared to

    recognise hydrogen.

    Think of all its qualities–the light gas which stood well in inverted

    vessels, burning with a pale flame at the mouth of the jar–and see

    whether this gas does not satisfy all these conditions. If it be hydrogen,

    it will remain here while I hold this jar inverted.  [A light was then

    applied, when the hydrogen burnt] What is there now in the other jar?  You

    know that the two together made an explosive mixture.  But what can this

    be which we find as the other constituent in water, and which must

    therefore be that substance which made the hydrogen burn? We know that the

    water we put into the vessel consisted of the two things together. We find

    one of these is hydrogen: what must that other be which was in the water

    before the experiment, and which we now have by itself?  I am about to put

    this lighted splinter of wood into the gas.  The gas itself will not burn,

    but it will make the splinter of wood burn.  [The Lecturer ignited the end

    of the wood, and introduced it into the jar of gas.]  See how it

    invigorates the combustion of the wood, and how it makes it burn far

    better than the air would make it burn; and now you see by itself that

    every other substance which is contained in the water, and which, when the

    water was formed by the burning of the candle, must have been taken from

    the atmosphere. What shall we call it, A, B, or C? Let us call it O–call

    it “Oxygen:” it is a very good distinct-sounding name. This, then, is the

    oxygen which was present in the water, forming so large a part of it.

    We shall now begin to understand more clearly our experiments and

    researches; because, when we have examined these things once or twice, we

    shall soon see why a candle burns in the air. When we have in this way

    analysed the water–that is to say, separated, or electrolysed its parts

    out of it–we get two volumes of hydrogen, and one of the body that burns

    it. And these two are represented to us on the following diagram, with

    their weights also stated; and we shall find that the oxygen is a very

    heavy body by comparison with the hydrogen. It is the other element in


    I had better, perhaps, tell you now how we get this oxygen abundantly,

    having shewn you how we can separate it from the water. Oxygen, as you

    will immediately imagine, exists in the atmosphere; for how should the

    candle burn to produce water without it?


    |           |


    |     1     |    8


    |           |


    |           | Oxygen. | Oxygen, . . . .


    |           |


    |           |_________| Hydrogen, . . .


    | Hydrogen. |


    |           |    9

    Water,. . . . . 100.0

    |           |

    |           |

    |           |


    Such a thing would be absolutely impossible, and chemically impossible,

    without oxygen.

    [Illustration: Fig. 21.]

    Can we get it from the air? Well, there are some very complicated and

    difficult processes by which we can get it from the air; but we have

    better processes. There is a substance called the black oxide of

    manganese: it is a very black-looking mineral, but very useful, and when

    made red-hot it gives out oxygen. Here is an iron bottle which has had

    some of this substance put into it, and there is a tube fixed to it, and a

    fire ready made, and Mr. Anderson will put that retort into the fire, for

    it is made of iron, and can stand the heat. Here is a salt called chlorate

    of potassa, which is now made in large quantities for bleaching, and

    chemical and medical uses, and for pyrotechnic and other purposes. I will

    take some and mix it with some of the oxide of manganese (oxide of copper,

    or oxide of iron would do as well); and if I put these together in a

    retort, far less than a red heat is sufficient to evolve this oxygen from

    the mixture. I am not preparing to make much, because we only want

    sufficient for our experiments; only, as you will see immediately, if I

    use too small a charge, the first portion of the gas will be mixed with

    the air already in the retort, and I should be obliged to sacrifice the

    first portion of the gas, because it would be so much diluted with air;

    the first portion must therefore be thrown away. You will find in this

    case, that a common spirit-lamp is quite sufficient for me to get the

    oxygen, and so we shall have two processes going on for its preparation.

    See how freely the gas is coming over from that small portion of the

    mixture. We will examine it, and see what are its properties. Now, in this

    way we are producing, as you will observe, a gas just like the one we had

    in the experiment with the battery, transparent, undissolved by water, and

    presenting the ordinary visible properties of the atmosphere. (As this

    first jar contains the air, together with the first portions of the oxygen

    set free during the preparation, we will carry it out of the way, and be

    prepared to make our experiments in a regular, dignified manner.) And,

    inasmuch as that power of making wood, wax, or other things burn, was so

    marked in the oxygen we obtained by means of the voltaic battery from

    water, we may expect to find the same property here. We will try it You

    see there is the combustion of a lighted taper in air, and here is its

    combustion in this gas [lowering the taper into the jar]. See how brightly

    and how beautifully it burns! You can also see more than this,–you will

    perceive it is a heavy gas, whilst the hydrogen would go up like a

    balloon, or even faster than a balloon, when not encumbered with the

    weight of the envelope.

    [Illustration: Fig. 22.]

    You may easily see that although we obtained from water twice as much in

    volume of the hydrogen as of oxygen, it does not follow that we have twice

    as much in weight–because one is heavy, and the other a very light gas.

    We have means of weighing gases or air; but without stopping to explain,

    that, let me just tell you what their respective weights are. The weight

    of a pint of hydrogen is three-quarters of a grain; the weight of the same

    quantity of oxygen is nearly twelve grains. This is a very great

    difference. The weight of a cubit foot of hydrogen is one-twelfth of an

    ounce; and the weight of a cubit foot of oxygen is one ounce and a third.

    And so on we might come to masses of matter which may be weighed in the

    balance, and which we can take account of as to hundredweights and as to

    tons, as you will see almost immediately.

    Now, as regards this very property of oxygen supporting combustion, which

    we may compare to air, I will take a piece of candle to shew it you in a

    rough way, and the result will be rough. There is our candle burning in

    the air: how will it burn in oxygen? I have here a jar of this gas, and I

    am about to put it over the candle for you to compare the action of this

    gas with that of the air. Why, look at it: it looks something like the

    light you saw at the poles of the voltaic battery. Think how vigorous that

    action must be! And yet, during all that action, nothing more is produced

    than what is produced by the burning of the candle in air. We have the

    same production of water, and the same phenomena exactly, when we use this

    gas instead of air, as we have when the candle is burnt in air.

    But now we have got a knowledge of this new substance, we can look at it a

    little more distinctly, in order to satisfy ourselves that we have got a

    good general understanding of this part of the product of a candle. It is

    wonderful how great the supporting powers of this substance are as regards

    combustion. For instance, here is a lamp which, simple though it be, is

    the original, I may say, of a great variety of lamps which are constructed

    for divers purposes–for light-houses, microscopic illuminations, and

    other uses; and if it were proposed to make it burn very brightly, you

    would say, “If a candle burnt better in oxygen, will not a lamp do the

    same?” Why, it will do so. Mr. Anderson will give me a tube coming from

    our oxygen reservoir, and I am about to apply it to this flame, which I

    will previously make burn badly on purpose. There comes the oxygen: what a

    combustion that makes! But if I shut it off, what becomes of the lamp? [The

    flow of oxygen was stopped, and the lamp relapsed to its former dimness.]

    It is wonderful how, by means of oxygen, we get combustion accelerated.

    But it does not affect merely the combustion of hydrogen, or carbon, or

    the candle; but it exalts all combustions of the common kind. We will take

    one which relates to iron, for instance, as you have already seen iron

    burn a little in the atmosphere. Here is a jar of oxygen, and this is a

    piece of iron wire; but if it were a bar as thick as my wrist, it would

    burn the same.

    [Illustration: Fig. 23.]

    I first attach a little piece of wood to the iron, I then set the wood on

    fire and let them both down together into the jar. The wood is now alight,

    and there it burns as wood should burn in oxygen; but it will soon

    communicate its combustion to the iron. The iron is now burning

    brilliantly, and will continue so for a long time. As long as we supply

    oxygen, so long can we carry on the combustion of the iron, until the

    latter is consumed.

    We will now put that on one side, and take some other substance; but we

    must limit our experiments, for we have not time to spare for all the

    illustrations you would have a right to if we had more time. We will take

    a piece of sulphur–you know how sulphur burns in the air–well, we put it

    into the oxygen, and you will see that whatever can burn in air, can burn

    with a far greater intensity in oxygen, leading you to think that perhaps

    the atmosphere itself owes all its power of combustion to this gas. The

    sulphur is now burning very quietly in the oxygen; but you cannot for a

    moment mistake the very high and increased action which takes place when

    it is so burnt, instead of being burnt merely in common air.

    [Illustration: Fig. 24.]

    I am now about to shew you the combustion of another

    substance–phosphorus. I can do it better for you here than you can do it

    at home. This is a very combustible substance; and if it be so combustible

    in air, what might you expect it would be in oxygen? I am about to shew it

    to you not in its fullest intensity, for if I did so we should almost blow

    the apparatus up–I may even now crack the jar, though I do not want to

    break things carelessly. You see how it burns in the air. But what a

    glorious light it gives out when I introduce it into oxygen! [Introducing

    the lighted phosphorus into the jar of oxygen.] There you see the solid

    particles going off which cause that combustion to be so brilliantly


    Thus far we have tested this power of oxygen, and the high combustion it

    produces by means of other substances. We must now, for a little while

    longer, look at it as respects the hydrogen. You know, when we allowed the

    oxygen and the hydrogen derived from the water to mix and burn together,

    we had a little explosion. You remember, also, that when I burnt the

    oxygen and the hydrogen in a jet together, we got very little light, but

    great heat. I am now about to set fire to oxygen and hydrogen, mixed in

    the proportion in which they occur in water. Here is a vessel containing

    one volume of oxygen and two volumes of hydrogen. This mixture is exactly

    of the same nature as the gas we just now obtained from the voltaic

    battery: it would be far too much to burn at once; I have therefore

    arranged to blow soap-bubbles with it, and burn those bubbles, that we may

    see by a general experiment or two how this oxygen supports the combustion

    of the hydrogen. First of all, we will see whether we can blow a bubble.

    Well, there goes the gas [causing it to issue through a tobacco-pipe into

    some soap-suds]. Here I have a bubble. I am receiving them on my hand: and

    you will perhaps think I am acting oddly in this experiment; but it is to

    shew you that we must not always trust to noise and sounds, but rather to

    real facts. [Exploding a bubble on the palm of his hand.] I am afraid to

    fire a bubble from the end of the pipe, because the explosion would pass

    up into the jar and blow it to pieces. This oxygen then will unite with

    the hydrogen, as you see by the phenomena, and hear by the sound, with the

    utmost readiness of action, and all its powers are then taken up in its

    neutralisation of the qualities of the hydrogen.

    So now I think you will perceive the whole history of water with reference

    to oxygen and the air, from what we have before said. Why does a piece of

    potassium decompose water? Because it finds oxygen in the water. What is

    set free when I put it in the water, as I am about to do again? It sets

    free hydrogen, and the hydrogen burns; but the potassium itself combines

    with oxygen; and this piece of potassium, in taking the water apart–the

    water, you may say, derived from the combustion of the candle–takes away

    the oxygen which the candle took from the air, and so sets the hydrogen

    free; and even if I take a piece of ice, and put a piece of potassium upon

    it, the beautiful affinities by which the oxygen and the hydrogen are

    related are such, that the ice will absolutely set fire to the potassium.

    I shew this to you to-day, in order to enlarge your ideas of these things,

    and that you may see how greatly results are modified by circumstances.

    There is the potassium on the ice, producing a sort of volcanic action.

    It will be my place, when next we meet, having pointed out these anomalous

    actions, to shew you that none of these extra and strange effects are met

    with by us–that none of these strange and injurious actions take place

    when we are burning, not merely a candle, but gas in our streets, or fuel

    in our fireplaces, so long as we confine ourselves within the laws that

    Nature has made for our guidance.




    We have now seen that we can produce hydrogen and oxygen from the water

    that we obtained from the candle. Hydrogen, you know, comes from the

    candle, and oxygen, you believe, comes from the air. But then you have a

    right to ask me, “How is it that the air and the oxygen do not equally

    well burn the candle?” If you remember what happened when I put a jar of

    oxygen over a piece of candle, you recollect there was a very different

    kind of combustion to that which took place in the air. Now, why is this?

    It is a very important question, and one I shall endeavour to make you

    understand: it relates most intimately to the nature of the atmosphere,

    and is most important to us.

    We have several tests for oxygen besides the mere burning of bodies. You

    have seen a candle burnt in oxygen, or in the air; you have seen

    phosphorus burnt in the air, or in oxygen; and you have seen iron-filings

    burnt in oxygen. But we have other tests besides these, and I am about to

    refer to one or two of them for the purpose of carrying your conviction

    and your experience further. Here we have a vessel of oxygen. I will shew

    its presence to you: if I take a little spark and put it into that oxygen,

    you know, by the experience you gained the last time we met, what will

    happen; if I put that spark into the jar, it will tell you whether we have

    oxygen here or not. Yes! We have proved it by combustion; and now here is

    another test for oxygen, which is a very curious and useful one. I have

    here two jars full of gas, with a plate between them to prevent their

    mixing; I take the plate away, and the gases are creeping one into the

    other. “What happens?” say you: “they together produce no such combustion

    as was seen in the case of the candle.” But see how the presence of oxygen

    is told by its association with this other substance[14]. What a

    beautifully coloured gas I have obtained in this way, shewing me the

    presence of the oxygen! In the same way we can try this experiment by

    mixing common air with this test-gas. Here is a jar containing air–such

    air as the candle would burn in–and here is a jar or bottle containing

    the test-gas. I let them come together over water, and you see the result:

    the contents of the test-bottle are flowing into the jar of air, and you

    see I obtain exactly the same kind of action as before, and that shews me

    that there is oxygen in the air–the very same substance that has been

    already obtained by us from the water produced by the candle. But then,

    beyond that, how is it that the candle does not burn in air as well as in

    oxygen? We will come to that point at once. I have here two jars; they are

    filled to the same height with gas, and the appearance to the eye is alike

    in both, and I really do not know at present which of these jars contains

    oxygen and which contains air, although I know they have previously been

    filled with these gases. But here is our test-gas, and I am going to work

    with the two jars, in order to examine whether there is any difference

    between them in the quality of reddening this gas. I am now going to turn

    this test-gas into one of the jars, and observe what happens. There is

    reddening, you see; there is then oxygen present. We will now test the

    other jar; but you see this is not so distinctly red as the first: and,

    further, this curious thing happens,–if I take these two gases and shake

    them well together with water, we shall absorb the red gas; and then, if I

    put in more of this test-gas and shake again, we shall absorb more; and I

    can go on as long as there be any oxygen present to produce that effect.

    If I let in air, it will not matter; but the moment I introduce water, the

    red gas disappears; and I may go on in this way, putting in more and more

    of the test-gas, until I come to something left behind which will not

    redden any longer by the use of that particular body that rendered the air

    and the oxygen red. Why is that? You see in a moment it is because there

    is, besides oxygen, something else present which is left behind. I will

    let a little more air into the jar, and if it turns red you will know that

    some of that reddening gas is still present, and that consequently it was

    not for the want of this producing body that that air was left behind.

    Now, you will begin to understand what I am about to say. You saw that

    when I burnt phosphorus in a jar, as the smoke produced by the phosphorus

    and the oxygen of the air condensed, it left a good deal of gas unburnt,

    just as this red gas left something untouched,–there was, in fact, this

    gas left behind, which the phosphorus cannot touch, which the reddening

    gas cannot touch, and this something is not oxygen, and yet is part of the


    So that is one way of opening out air into the two things of which it is

    composed–oxygen, which burns our candles, our phosphorus, or anything

    else; and this other substance–nitrogen–which will not burn them. This

    other part of the air is by far the larger proportion, and it is a very

    curious body, when we come to examine it; it is remarkably curious, and

    yet you say, perhaps, that it is very uninteresting. It is uninteresting

    in some respects because of this–that it shews no brilliant effects of

    combustion.  If I test it with a taper as I do oxygen and hydrogen, it

    does not burn like hydrogen, nor does it make the taper burn like oxygen.

    Try it in any way I will, it does neither the one thing nor the other: it

    will not take fire; it will not let the taper burn; it puts out the

    combustion of everything. There is nothing that will burn in it in common

    circumstances. It has no smell; it is not sour; it does not dissolve in

    water; it is neither an acid nor an alkali; it is as indifferent to all

    our organs as it is possible for a thing to be. And you might say, “It is

    nothing; it is not worth chemical attention; what does it do in the air?”

    Ah! then come our beautiful and fine results shewn us by an observant

    philosophy.  Suppose, in place of having nitrogen, or nitrogen and oxygen,

    we had pure oxygen as our atmosphere; what would become of us? You know

    very well that a piece of iron lit in a jar of oxygen goes on burning to

    the end. When you see a fire in an iron grate, imagine where the grate

    would go to if the whole of the atmosphere were oxygen. The grate would

    burn up more powerfully than the coals–for the iron of the grate itself

    is even more combustible than the coals which we burn in it. A fire put

    into the middle of a locomotive would be a fire in a magazine of fuel, if

    the atmosphere were oxygen. The nitrogen lowers it down and makes it

    moderate and useful for us, and then, with all that, it takes away with it

    the fumes that you have seen produced from the candle, disperses them

    throughout the whole of the atmosphere, and carries them away to places

    where they are wanted to perform a great and glorious purpose of good to

    man, for the sustenance of vegetation; and thus does a most wonderful

    work, although you say, on examining it, “Why, it is a perfectly

    indifferent thing.” This nitrogen in its ordinary state is an inactive

    element; no action short of the most intense electric force, and then in

    the most infinitely small degree, can cause the nitrogen to combine

    directly with the other element of the atmosphere, or with other things

    round about it; it is a perfectly indifferent, and therefore to say, a

    safe substance.

    But before I take you to that result, I must tell you about the atmosphere

    itself. I have written on this diagram the composition of one hundred

    parts of atmospheric air:–



    Oxygen, . . . . .   20    22.3

    Nitrogen, . . . .   80    77.7





    It is a true analysis of the atmosphere, so far as regards the quantity of

    oxygen and the quantity of nitrogen present. By our analysis, we find that

    5 pints of the atmosphere contain only 1 pint of oxygen, and 4 pints, or 4

    parts, of nitrogen by bulk. That is our analysis of the atmosphere. It

    requires all that quantity of nitrogen to reduce the oxygen down, so as to

    be able to supply the candle properly with fuel, so as to supply us with

    an atmosphere which our lungs can healthily and safely breathe; for it is

    just as important to make the oxygen right for us to breathe, as it is to

    make the atmosphere right for the burning of the fire and the candle.

    But now for this atmosphere. First of all, let me tell you the weight of

    these gases. A pint of nitrogen weighs 10-4/10 grains, or a cubic foot

    weighs 1-1/6 ounce. That is the weight of the nitrogen. The oxygen is

    heavier: a pint of it weighs 11-9/10 grains, and a cubic foot weighs 1-3/4

    ounce. A pint of air weighs about 10-7/10 grains, and a cubic foot 1-1/5


    [Illustration: Fig. 25.]

    You have asked me several times, and I am very glad you have, “How do you

    weigh gases?” I will shew you; it is very simple, and easily done. Here is

    a balance, and here a copper bottle, made as light as we can consistent

    with due strength, turned very nicely in the lathe, and made perfectly

    air-tight, with a stop-cock, which we can open and shut, which at present

    is open, and therefore allows the bottle to be full of air. I have here a

    nicely-adjusted balance, in which I think the bottle, in its present

    condition, will be balanced by the weight on the other side. And here is a

    pump by which we can force the air into this bottle, and with it we will

    force in a certain number of volumes of air, as measured by the pump.

    [Twenty measures were pumped in.] We will shut that in and put it in the

    balance. See how it sinks: it is much heavier than it was. By what?  By

    the air that we have forced into it by the pump. There is not a greater

    _bulk_ of air, but there is the same bulk of _heavier_ air, because we

    have forced in air upon it. And that you may have a fair notion in your

    mind as to how much this air measures, here is a jar full of water. We

    will open that copper vessel into this jar, and let the air return to its

    former state. All I have to do now is to screw them tightly together, and

    to turn the taps, when there, you see, is the bulk of the twenty pumps of

    air which I forced into the bottle; and to make sure that we have been

    quite correct in what we have been doing, we will take the bottle again to

    the balance, and, if it is now counterpoised by the original weight, we

    shall be quite sure we have made our experiment correctly.

    [Illustration: Fig. 26.]

    It is balanced; so, you see, we can find out the weight of the extra

    volumes of air forced in, in that way, and by that means we are able to

    ascertain that a cubic foot of air weighs 1-1/5 ounce. But that small

    experiment will by no means convey to your mind the whole literal truth of

    this matter. It is wonderful how it accumulates when you come to larger

    volumes. This bulk of air [a cubic foot] weighs 1-1/5 ounce. What do you

    think of the contents of that box above there, which I have had made for

    the purpose? The air which is within that box weighs one pound–a full

    pound; and I have calculated the weight of the air in this room,–you

    would hardly imagine it, but it is above a ton. So rapidly do the weights

    rise up, and so important is the presence of the atmosphere, and of the

    oxygen and the nitrogen in it, and the use it performs in conveying things

    to and fro from place to place, and carrying bad vapours to places where

    they will do good instead of harm.

    Having given you that little illustration with respect to the weight of

    the air, let me shew you certain consequences of it. You have a right to

    them, because you would not understand so much without it. Do you remember

    this kind of experiment? Have you ever seen it? Suppose I take a pump

    somewhat similar to the one I had a little while ago to force air into the

    bottle, and suppose I place it in such a manner that by certain

    arrangements I can apply my hand to it: my hand moves about in the air so

    easily that it seems to feel nothing, and I can hardly get velocity enough

    by any motion of my own in the atmosphere to make sure that there is much

    resistance to it.

    [Illustration: Fig. 27.]

    But, when I put my hand here [on the air-pump receiver, which was

    afterwards exhausted], you see what happens. Why is my hand fastened to

    this place, and why am I able to pull this pump about? And see! how is it

    that I can hardly get my hand away? Why is this? It is the weight of the

    air–the weight of the air that is above. I have another experiment here,

    which I think will explain to you more about it. When the air is pumped

    from underneath the bladder which is stretched over this glass, you will

    see the effect in another shape: the top is quite flat at present, but I

    will make a very little motion with the pump, and now look at it–see how

    it has gone down, see how it is bent in. You will see the bladder go in

    more and more, until at last I expect it will be driven in and broken by

    the force of the atmosphere pressing upon it.

    [Illustration: Fig. 28.]

    [The bladder at last broke with a loud report.] Now, that was done

    entirely by the weight of the air pressing on it, and you can easily

    understand how that is. The particles that are piled up in the atmosphere

    stand upon each other, as these five cubes do. You can easily conceive

    that four of these five cubes are resting upon the bottom one, and if I

    take that away, the others will all sink down. So it is with the

    atmosphere: the air that is above is sustained by the air that is beneath;

    and when the air is pumped away from beneath them, the change occurs which

    you saw when I placed my hand on the air-pump, and which you saw in the

    case of the bladder, and which you shall see better here. I have tied over

    this jar a piece of sheet india-rubber, and I am now about to take away

    the air from the inside of the jar; and if you will watch the

    india-rubber–which acts as a partition between the air below and the air

    above–you will see, when I pump, how the pressure shews itself. See where

    it is going to–I can actually put my hand into the jar; and yet this

    result is only caused by the great and powerful action of the air above.

    How beautifully it shews this curious circumstance!

    Here is something that you can have a pull at, when I have finished

    to-day. It is a little apparatus of two hollow brass hemispheres, closely

    fitted together, and having connected with it a pipe and a cock, through

    which we can exhaust the air from the inside; and although the two halves

    are so easily taken apart, while the air is left within, yet you will see,

    when we exhaust it by-and-by, no power of any two of you will be able to

    pull them apart. Every square inch of surface that is contained in the

    area of that vessel sustains fifteen pounds by weight, or nearly so, when

    the air is taken out; and you may try your strength presently in seeing

    whether you can overcome that pressure of the atmosphere.

    Here is another very pretty thing–the boys’ sucker, only refined by the

    philosopher. We young ones have a perfect right to take toys, and make

    them into philosophy, inasmuch as now-a-days we are turning philosophy

    into toys. Here is a sucker, only it is made of india-rubber: if I clap it

    upon the table, you see at once it holds. Why does it hold? I can slip it

    about, and yet if I try to pull it up, it seems as if it would pull the

    table with it I can easily make it slip about from place to place; but

    only when I bring it to the edge of the table can I get it off. It is only

    kept down by the pressure of the atmosphere above. We have a couple of

    them; and if you take these two and press them together, you will see how

    firmly they stick. And, indeed, we may use them as they are proposed to be

    used, to stick against windows, or against walls, where they will adhere

    for an evening, and serve to hang anything on that you want. I think,

    however, that you boys ought to be shewn experiments that you can make at

    home; and so here is a very pretty experiment in illustration of the

    pressure of the atmosphere. Here is a tumbler of water. Suppose I were to

    ask you to turn that tumbler upside-down, so that the water should not

    fall out, and yet not be kept in by your hand, but merely by using the

    pressure of the atmosphere. Could you do that? Take a wine-glass, either

    quite full or half-full of water, and put a flat card on the top, turn it

    upside-down, and then see what becomes of the card and of the water. The

    air cannot get in because the water by its capillary attraction round the

    edge keeps it out.

    I think this will give you a correct notion of what you may call the

    materiality of the air; and when I tell you that the box holds a pound of

    it, and this room more than a ton, you will begin to think that air is

    something very serious. I will make another experiment, to convince you of

    this positive resistance. There is that beautiful experiment of the

    popgun, made so well and so easily, you know, out of a quill, or a tube,

    or anything of that kind,–where we take a slice of potato, for instance,

    or an apple, and take the tube and cut out a pellet, as I have now done,

    and push it to one end. I have made that end tight; and now I take another

    piece and put it in: it will confine the air that is within the tube

    perfectly and completely for our purpose; and I shall now find it

    absolutely impossible by any force of mine to drive that little pellet

    close up to the other. It cannot be done. I may press the air to a certain

    extent, but if I go on pressing, long before it comes to the second, the

    confined air will drive the front one out with a force something like that

    of gunpowder; for gunpowder is in part dependent upon the same action that

    you see here exemplified.

    I saw the other day an experiment which pleased me much, as I thought it

    would serve our purpose here. (I ought to have held my tongue for four or

    five minutes before beginning this experiment, because it depends upon my

    lungs for success.) By the proper application of air I expect to be able

    to drive this egg out of one cup into the other by the force of my breath;

    but if I fail, it is in a good cause; and I do not promise success,

    because I have been talking more than I ought to do to make the experiment


    [The Lecturer here tried the experiment, and succeeded in blowing the egg

    from one egg-cup to the other.]

    You see that the air which I blow goes downwards between the egg and the

    cup, and makes a blast under the egg, and is thus able to lift a heavy

    thing–for a full egg is a very heavy thing for air to lift. If you want

    to make the experiment, you had better boil the egg quite hard first, and

    then you may very safely try to blow it from one cup to the other, with a

    little care.

    I have now kept you long enough upon this property of the weight of the

    air, but there is another thing I should like to mention. You saw the way

    in which, in this popgun, I was able to drive the second piece of potato

    half or two-thirds of an inch before the first piece started, by virtue of

    the elasticity of the air–just as I pressed into the copper bottle the

    particles of air by means of the pump. Now, this depends upon a wonderful

    property in the air, namely, its elasticity; and I should like to give you

    a good illustration of this. If I take anything that confines the air

    properly, as this membrane, which also is able to contract and expand so

    as to give us a measure of the elasticity of the air, and confine in this

    bladder a certain portion of air; and then, if we take the atmosphere off

    from the outside of it, just as in these cases we put the pressure on–if

    we take the pressure off, you will see how it will then go on expanding

    and expanding, larger and larger, until it will fill the whole of this

    bell-jar, shewing you that wonderful property of the air, its elasticity,

    its compressibility, and expansibility, to an exceedingly large extent,

    and which is very essential for the purposes and services it performs in

    the economy of creation.

    We will now turn to another very important part of our subject,

    remembering that we have examined the candle in its burning, and have

    found that it gives rise to various products. We have the products, you

    know, of soot, of water, and of something else which you have not yet

    examined. We have collected the water, but have allowed the other things

    to go into the air. Let us now examine some of these other products.

    Here is an experiment which I think will help you in part in this way. We

    will put our candle there, and place over it a chimney, thus. I think my

    candle will go on burning, because the air-passage is open at the bottom

    and the top. In the first place, you see the moisture appearing–that you

    know about. It is water produced from the candle by the action of the air

    upon its hydrogen. But, besides that, something is going out at the top:

    it is not moisture–it is not water–it is not condensible; and yet, after

    all, it has very singular properties. You will find that the air coming

    out of the top of our chimney is nearly sufficient to blow the light out I

    am holding to it; and if I put the light fairly opposed to the current, it

    will blow it quite out. You will say that is as it should be; and I am

    supposing that you think it ought to do so, because the nitrogen does not

    support combustion, and ought to put the candle out, since the candle will

    not burn in nitrogen.

    [Illustration: Fig. 29.]

    But is there nothing else there than nitrogen? I must now anticipate–that

    is to say, I must use my own knowledge to supply you with the means that

    we adopt for the purpose of ascertaining these things, and examining such

    gases as these. I will take an empty bottle–here is one–and if I hold it

    over this chimney, I shall get the combustion of the candle below sending

    its results into the bottle above; and we shall soon find that this bottle

    contains, not merely an air that is bad as regards the combustion of a

    taper put into it, but having other properties.

    Let me take a little quick-lime and pour some common water on to it–the

    commonest water will do. I will stir it a moment, then pour it upon a

    piece of filtering paper in a funnel, and we shall very quickly have a

    clear water proceeding to the bottle below, as I have here. I have plenty

    of this water in another bottle; but, nevertheless, I should like to use

    the lime-water that was prepared before you, so that you may see what its

    uses are. If I take some of this beautiful clear lime-water, and pour it

    into this jar, which has collected the air from the candle, you will see a

    change coming about. Do you see that the water has become quite milky?

    Observe, that will not happen with air merely. Here is a bottle filled

    with air; and if I put a little lime-water into it, neither the oxygen nor

    the nitrogen, nor anything else that is in that quantity of air, will make

    any change in the lime-water. It remains perfectly clear, and no shaking

    of that quantity of lime-water with that quantity of air in its common

    state will cause any change; but if I take this bottle with the

    lime-water, and hold it so as to get the general products of the candle in

    contact with it, in a very short time we shall have it milky. There is the

    chalk, consisting of the lime which we used in making the lime-water,

    combined with something that came from the candle–that other product

    which we are in search of, and which I want to tell you about to-day. This

    is a substance made visible to us by its action, which is not the action

    of the lime-water either upon the oxygen or upon the nitrogen, nor upon

    the water itself, but it is something new to us from the candle. And then

    we find this white powder, produced by the lime-water and the vapour from

    the candle, appears to us very much like whitening or chalk, and, when

    examined, it does prove to be exactly the same substance as whitening or

    chalk. So we are led, or have been led, to observe upon the various

    circumstances of this experiment, and to trace this production of chalk to

    its various causes, to give us the true knowledge of the nature of this

    combustion of the candle–to find that this substance, issuing from the

    candle, is exactly the same as that substance which would issue from a

    retort, if I were to put some chalk into it with a little moisture, and

    make it red-hot: you would then find that exactly the same substance would

    issue from it as from the candle.

    But we have a better means of getting this substance, and in greater

    quantity, so as to ascertain what its general characters are. We find this

    substance in very great abundance in a multitude of cases where you would

    least expect it. All limestones contain a great deal of this gas which

    issues from the candle, and which we call _carbonic acid_. All chalks, all

    shells, all corals contain a great quantity of this curious air. We find

    it fixed in these stones; for which reason Dr. Black called it “fixed

    air”–finding it in these fixed things like marble and chalk. He called it

    fixed air, because it lost its quality of air, and assumed the condition

    of a solid body. We can easily get this air from marble.  Here is a jar

    containing a little muriatic acid, and here is a taper which, if I put it

    into that jar, will shew only the presence of common air. There is, you

    see, pure air down to the bottom; the jar is full of it  Here is a

    substance–marble[17], a very beautiful and superior marble–and if I put

    these pieces of marble into the jar, a great boiling apparently goes on.

    That, however, is not steam–it is a gas that is rising up; and if I now

    search the jar by a candle, I shall have exactly the same effect produced

    upon the taper as I had from the air which issued from the end of the

    chimney over the burning candle. It is exactly the same action, and caused

    by the very same substance that issued from the candle; and in this way we

    can get carbonic acid in great abundance–we have already nearly filled

    the jar.  We also find that this gas is not merely contained in marble.

    Here is a vessel in which I have put some common whitening–chalk, which

    has been washed in water and deprived of its coarser particles, and so

    supplied to the plasterer as whitening.  Here is a large jar containing

    this whitening and water, and I have here some strong sulphuric acid,

    which is the acid you might have to use if you were to make these

    experiments (only, in using this acid with limestone, the body that is

    produced is an insoluble substance, whereas the muriatic acid produces a

    soluble substance that does not so much thicken the water). And you will

    seek out a reason why I take this kind of apparatus for the purpose of

    shewing this experiment. I do it because you may repeat in a small way

    what I am about to do in a large one. You will have here just the same

    kind of action; and I am evolving in this large jar carbonic acid, exactly

    the same in its nature and properties as the gas which we obtained from

    the combustion of the candle in the atmosphere. And no matter how

    different the two methods by which we prepare this carbonic acid, you will

    see, when we get to the end of our subject, that it is all exactly the

    same, whether prepared in the one way or in the other.

    We will now proceed to the next experiment with regard to this gas. What

    is its nature? Here is one of the vessels full, and we will try it, as we

    have done so many other gases, by combustion. You see it is not

    combustible, nor does it support combustion. Neither, as we know, does it

    dissolve much in water, because we collect it over water very easily.

    Then, you know that it has an effect, and becomes white in contact with

    lime-water; and when it does become white in that way, it becomes one of

    the constituents to make carbonate of lime or limestone.

    The next thing I must shew you is, that it really does dissolve a little

    in water, and  therefore that it is unlike oxygen and hydrogen in that

    respect I have here an apparatus by which we can produce this solution. In

    the lower part of this apparatus is marble and acid, and in the upper part

    cold water. The valves are so arranged that the gas can get from one to

    the other. I will set it in action now, and you can see the gas bubbling

    up through the water, as it has been doing all night long, and by this

    time we shall find that we have this substance dissolved in the water. If

    I take a glass and draw off some of the water, I find that it tastes a

    little acid to the mouth: it is impregnated with carbonic acid; and if I

    now apply a little lime-water to it, that will give us a test of its

    presence. This water will make the lime-water turbid and white, which is

    proof of the presence of carbonic acid.

    Then it is a very weighty gas–it is heavier than the atmosphere. I have

    put their respective weights at the lower part of this table, along with,

    for comparison, the weights of the other gases we have been examining:–


    Cubic Foot.

    Hydrogen, .  .  .  .  3/4 grains. 1/12 ounce.

    Oxygen,   .  .  .  .  11-9/10 ”   1-1/2

    Nitrogen, .  .  .  .  10-1/10 ”   1-1/4  ”

    Air,.  .  .  .  .  .  10-7/16 ”   1-3/8

    Carbonic acid,  .  .  16-1/3  ”   1-9/10 “

    A pint of it weighs 16-1/3 grains, and a cubic foot weighs 1-9/10 ounce,

    almost two ounces. You can see by many experiments that this is a heavy

    gas. Suppose I take a glass containing nothing else but air, and from this

    vessel containing the carbonic acid I attempt to pour a little of this gas

    into that glass; I wonder whether any has gone in or not. I cannot tell by

    the appearance, but I can in this way [introducing the taper]. Yes, there

    it is, you see; and if I were to examine it by lime-water, I should find

    it by that test also. I will take this little bucket, and put it down into

    the well of carbonic acid–indeed, we too often have real wells of

    carbonic acid–and now, if there is any carbonic acid, I must have got to

    it by this time, and it will be in this bucket, which we will examine with

    a taper. There it is, you see; it is full of carbonic acid.

    [Illustration: Fig. 30.]

    There is another experiment by which I will shew you its weight. I have

    here a jar suspended at one end of a balance–it is now equipoised; but

    when I pour this carbonic acid into the jar on the one side which now

    contains air, you will see it sink down at once, because of the carbonic

    acid that I pour into it. And now, if I examine this jar with the lighted

    taper, I shall find that the carbonic acid has fallen into it, and it no

    longer has any power of supporting the combustion. If I blow a

    soap-bubble, which of course will be filled with air, and let it fall into

    this jar of carbonic acid, it will float.

    [Illustration: Fig. 31.]

    But I shall first of all take one of these little balloons filled with

    air.  I am not quite sure where the carbonic acid is; we will just try the

    depth, and see whereabouts is its level. There, you see, we have this

    bladder floating on the carbonic acid; and if I evolve some more of the

    carbonic acid, the bladder will be lifted up higher. There it goes–the

    jar is nearly full; and now I will see whether I can blow a soap-bubble on

    that, and float it in the same way. [The Lecturer here blew a soap-bubble,

    and allowed it to fall into the jar of carbonic acid, when it floated in

    it midway.] It is floating, as the balloon floated, by virtue of the

    greater weight of the carbonic acid than of the air. And now, having so

    far given you the history of the carbonic acid–as to its sources in the

    candle, as to its physical properties and weight–when we next meet I

    shall shew you of what it is composed, and where it gets its elements





    A lady, who honours me by her presence at these Lectures, has conferred a

    still further obligation by sending me these two candles, which are from

    Japan, and, I presume, are made of that substance to which I referred in a

    former lecture. You see that they are even far more highly ornamented than

    the French candles; and, I suppose, are candles of luxury, judging from

    their appearance. They have a remarkable peculiarity about them–namely, a

    hollow wick,–that beautiful peculiarity which Argand introduced into the

    lamp, and made so valuable. To those who receive such presents from the

    East, I may just say that this and such like materials gradually undergo a

    change which gives them on the surface a dull and dead appearance; but

    they may easily be restored to their original beauty, if the surface be

    rubbed with a clean cloth or silk handkerchief, so as to polish the little

    rugosity or roughness: this will restore the beauty of the colours. I have

    so rubbed one of these candles, and you see the difference between it and

    the other which has not been polished, but which may be restored by the

    same process. Observe, also, that these moulded candles from Japan are

    made more conical than the moulded candles in this part of the world.

    I told you, when we last met, a good deal about carbonic acid. We found,

    by the lime-water test, that when the vapour from the top of the candle or

    lamp was received into bottles, and tested by this solution of lime-water

    (the composition of which I explained to you, and which you can make for

    yourselves), we had that white opacity which was in fact calcareous

    matter, like shells and corals, and many of the rocks and minerals in the

    earth. But I have not yet told you fully and clearly the chemical history

    of this substance–carbonic acid–as we have it from the candle, and I

    must now resume that subject. We have seen the products, and the nature of

    them, as they issue from the candle.  We have traced the water to its

    elements, and now we have to see where are the elements of the carbonic

    acid supplied by the candle. A few experiments will shew this. You

    remember that when a candle burns badly, it produces smoke; but if it is

    burning well, there is no smoke. And you know that the brightness of the

    candle is due to this smoke, which becomes ignited. Here is an experiment

    to prove this: so long as the smoke remains in the flame of the candle and

    becomes ignited, it gives a beautiful light, and never appears to us in

    the form of black particles. I will light some fuel, which is extravagant

    in its burning. This will serve our purpose–a little turpentine on a

    sponge. You see the smoke rising from it, and floating into the air in

    large quantities; and, remember now, the carbonic acid that we have from

    the candle is from such smoke as that. To make that evident to you, I will

    introduce this turpentine burning on the sponge into a flask where I have

    plenty of oxygen, the rich part of the atmosphere, and you now see that

    the smoke is all consumed. This is the first part of our experiment; and

    now, what follows? The carbon which you saw flying off from the turpentine

    flame in the air is now entirely burned in this oxygen, and we shall find

    that it will, by this rough and temporary experiment, give us exactly the

    same conclusion and result as we had from the combustion of the candle.

    The reason why I make the experiment in this manner is solely that I may

    cause the steps of our demonstration to be so simple that you can never

    for a moment lose the train of reasoning, if you only pay attention. All

    the carbon which is burned in oxygen, or air, comes out as carbonic acid,

    whilst those particles which are not so burned shew you the second

    substance in the carbonic acid–namely, the carbon–that body which made

    the flame so bright whilst there was plenty of air, but which was thrown

    off in excess when there was not oxygen enough to burn it.

    I have also to shew you a little more distinctly the history of carbon and

    oxygen, in their union to make carbonic acid. You are now better able to

    understand this than before, and I have prepared three or four experiments

    by way of illustration. This jar is filled with oxygen, and here is some

    carbon which has been placed in a crucible, for the purpose of being made

    red-hot. I keep my jar dry, and venture to give you a result imperfect in

    some degree, in order that I may make the experiment brighter. I am about

    to put the oxygen and the carbon together.  That this is carbon (common

    charcoal pulverised), you will see by the way in which it burns in the air

    [letting some of the red-hot charcoal fall out of the crucible]. I am now

    about to burn it in oxygen gas, and look at the difference. It may appear

    to you at a distance as if it were burning with a flame; but it is not so.

    Every little piece of charcoal is burning as a spark, and whilst it so

    burns it is producing carbonic acid. I specially want these two or three

    experiments to point out what I shall dwell upon more distinctly

    by-and-by–that carbon burns in this way, and not as a flame.

    Instead of taking many particles of carbon to burn, I will take a rather

    large piece, which will enable you to see the form and size; and to trace

    the effects very decidedly. Here is the jar of oxygen, and here is the

    piece of charcoal, to which I have fastened a little piece of wood, which

    I can set fire to, and so commence the combustion, which I could not

    conveniently do without. You now see the charcoal burning, but not as a

    flame (or if there be a flame, it is the smallest possible one, which I

    know the cause of–namely, the formation of a little carbonic oxide close

    upon the surface of the carbon). It goes on burning, you see, slowly

    producing carbonic acid by the union of this carbon or charcoal (they are

    equivalent terms) with the oxygen. I have here another piece of charcoal,

    a piece of bark, which has the quality of being blown to pieces–exploding

    as it burns. By the effect of the heat, we shall reduce the lump of carbon

    into particles that will fly off; still every particle, equally with the

    whole mass, burns in this peculiar way: it burns as a coal, and not like a

    flame. You observe a multitude of little combustions going on, but no

    flame. I do not know a finer experiment than this, to shew that carbon

    burns with a spark.

    Here, then, is carbonic acid formed from its elements. It is produced at

    once; and if we examined it by lime-water, you will see that we have the

    same substance which I have previously described to you. By putting

    together 6 parts of carbon by weight (whether it comes from the flame of a

    candle or from powdered charcoal) and 16 parts of oxygen by weight, we

    have 22 parts of carbonic acid; and, as we saw last time, the 22 parts of

    carbonic acid, combined with 28 parts of lime, produced common carbonate

    of lime.  If you were to examine an oyster-shell, and weigh the component

    parts, you would find that every 50 parts would give 6 of carbon and 16 of

    oxygen, combined with 28 of lime. However, I do not want to trouble you

    with these minuti?–it is only the general philosophy of the matter that

    we can now go into. See how finely the carbon is dissolving away [pointing

    to the lump of charcoal burning quietly in the jar of oxygen]. You may say

    that the charcoal is actually dissolving in the air round about; and if

    that were perfectly pure charcoal, which we can easily prepare, there

    would be no residue whatever. When we have a perfectly cleansed and

    purified piece of carbon, there is no ash left. The carbon burns as a

    solid dense body, that heat alone cannot change as to its solidity, and

    yet it passes away into vapour that never condenses into solid or liquid

    under ordinary circumstances; and what is more curious still, is the fact

    that the oxygen does not change in its bulk by the solution of the carbon

    in it. Just as the bulk is at first, so it is at last, only it has become

    carbonic acid.

    There is another experiment which I must give you before you are fully

    acquainted with the general nature of carbonic acid. Being a compound

    body, consisting of carbon and oxygen, carbonic acid is a body that we

    ought to be able to take asunder. And so we can. As we did with water, so

    we can with carbonic acid–take the two parts asunder. The simplest and

    quickest way is to act upon the carbonic acid by a substance that can

    attract the oxygen from it, and leave the carbon behind. You recollect

    that I took potassium and put it upon water or ice, and you saw that it

    could take the oxygen from the hydrogen. Now, suppose we do something of

    the same kind here with this carbonic acid. You know carbonic acid to be a

    heavy gas. I will not test it with lime-water, as that will interfere with

    our subsequent experiments; but I think the heaviness of the gas and the

    power of extinguishing flame will be sufficient for our purpose. I

    introduce a flame into the gas, and you will see whether it will be put

    out. You see the light is extinguished. Indeed, the gas may, perhaps, put

    out phosphorus, which, you know, has a pretty strong combustion. Here is a

    piece of phosphorus heated to a high degree. I introduce it into gas, and

    you observe the light is put out; but it will take fire again in the air,

    because there it re-enters into combustion. Now, let me take a piece of

    potassium, a substance which, even at common temperatures, can act upon

    carbonic acid, though not sufficiently for our present purpose, because it

    soon gets covered with a protecting coat; but if we warm it up to the

    burning point in air, as we have a fair right to do, and as we have done

    with phosphorus, you will see that it can burn in carbonic acid; and if it

    burns, it will burn by taking oxygen, so that you will see what is left

    behind. I am going, then, to burn this potassium in the carbonic acid, as

    a proof of the existence of oxygen in the carbonic acid. [In the

    preliminary process of heating, the potassium exploded.] Sometimes we get

    an awkward piece of potassium that explodes, or something like it, when it

    burns. I will take another piece; and now that it is heated, I introduce

    it into the jar, and you perceive that it burns in the carbonic acid–not

    so well as in the air, because the carbonic acid contains the oxygen

    combined; but it does burn, and takes away the oxygen. If I now put this

    potassium into water, I find that, besides the potash formed (which you

    need not trouble about), there is a quantity of carbon produced. I have

    here made the experiment in a very rough way; but I assure you that if I

    were to make it carefully, devoting a day to it, instead of five minutes,

    we should get all the proper amount of charcoal left in the spoon, or in

    the place where the potassium was burned, so that there could be no doubt

    as to the result. Here, then, is the carbon obtained from the carbonic

    acid, as a common black substance; so that you have the entire proof of

    the nature of carbonic acid as consisting of carbon and oxygen. And now, I

    may tell you, that _whenever_ carbon burns under common circumstances, it

    produces carbonic acid.

    Suppose I take this piece of wood, and put it into a bottle with

    lime-water. I might shake that lime-water up with wood and the atmosphere

    as long as I pleased, it would still remain clear as you see it; but

    suppose I burn the piece of wood in the air of that bottle. You, of

    course, know I get water. Do I get carbonic acid? [The experiment was

    performed.] There it is, you see–that is to say, the carbonate lime,

    which results from carbonic acid, and that carbonic acid must be formed

    from the carbon which comes from the wood, from the candle, or any other

    thing.  Indeed, you have yourselves frequently tried a very pretty

    experiment, by which you may see the carbon in wood. If you take a piece

    of wood, and partly burn it, and then blow it out, you have carbon left.

    There are things that do not shew carbon in this way. A candle does not

    shew it, but it contains carbon. Here also is a jar of coal-gas, which

    produces carbonic acid abundantly. You do not see the carbon, but we can

    soon shew it to you. I will light it, and as long as there is any gas in

    this cylinder it will go on burning. You see no carbon, but you see a

    flame; and because that is bright, it will lead you to guess that there is

    carbon in the flame. But I will shew it to you by another process. I have

    some of the same gas in another vessel, mixed with a body that will burn

    the hydrogen of the gas, but will not burn the carbon. I will light them

    with a burning taper, and you perceive the hydrogen is consumed, but not

    the carbon, which is left behind as a dense black smoke. I hope that by

    these three or four experiments you will learn to see when carbon is

    present, and understand what are the products of combustion, when gas or

    other bodies are thoroughly burned in the air.

    Before we leave the subject of carbon, let us make a few experiments and

    remarks upon its wonderful condition as respects ordinary combustion. I

    have shewn you that the carbon in burning burns only as a solid body, and

    yet you perceive that, after it is burned, it ceases to be a solid. There

    are very few fuels that act like this. It is, in fact, only that great

    source of fuel, the carbonaceous series, the coals, charcoals, and woods,

    that can do it. I do not know that there is any other elementary substance

    besides carbon that burns with these conditions; and if it had not been

    so, what would happen to us? Suppose all fuel had been like iron, which,

    when it burns, burns into a solid substance. We could not then have such a

    combustion as you have in this fire-place. Here also is another kind of

    fuel which burns very well–as well as, if not better, than carbon–so

    well, indeed, as to take fire of itself when it is in the air, as you see

    [breaking a tube full of lead pyrophorus]. This substance is lead, and you

    see how wonderfully combustible it is. It is very much divided, and is

    like a heap of coals in the fireplace; the air can get to its surface and

    inside, and so it burns. But why does it not burn in that way now, when it

    is lying in a mass? [emptying the contents of the tube in a heap on to a

    plate of iron]. Simply because the air cannot get to it. Though it can

    produce a great heat, the great heat which we want in our furnaces and

    under our boilers, still that which is produced cannot get away from the

    portion which remains unburned underneath, and that portion, therefore, is

    prevented from coming in contact with the atmosphere, and cannot be

    consumed. How different is that from carbon. Carbon burns just in the same

    way as this lead does, and so gives an intense fire in the furnace, or

    wherever you choose to burn it; but then the body produced by its

    combustion passes away, and the remaining carbon is left clear. I shewed

    you how carbon went on dissolving in the oxygen, leaving no ash; whereas

    here [pointing to the heap of pyrophorus] we have actually more ash than

    fuel, for it is heavier by the amount of the oxygen which has united with

    it. Thus you see the difference between carbon and lead or iron: if we

    choose iron, which gives so wonderful a result in our application of this

    fuel, either as light or heat. If, when the carbon burnt, the product went

    off as a solid body, you would have had the room filled with an opaque

    substance, as in the case of the phosphorus; but when carbon burns,

    everything passes up into the atmosphere. It is in a fixed, almost

    unchangeable condition before the combustion; but afterwards it is in the

    form of gas, which it is very difficult (though we have succeeded) to

    produce in a solid or a liquid state.

    Now, I must take you to a very interesting part of our subject–to the

    relation between the combustion of a candle and that living kind of

    combustion which goes on within us. In every one of us there is a living

    process of combustion going on very similar to that of a candle; and I

    must try to make that plain to you. For it is not merely true in a

    poetical sense–the relation of the life of man to a taper; and if you

    will follow, I think I can make this clear. In order to make the relation

    very plain, I have devised a little apparatus which we can soon build up

    before you. Here is a board and a groove cut in it, and I can close the

    groove at the top part by a little cover. I can then continue the groove

    as a channel by a glass tube at each end, there being a free passage

    through the whole. Suppose I take a taper or candle (we can now be liberal

    in our use of the word “candle,” since we understand what it means), and

    place it in one of the tubes; it will go on, you see, burning very well.

    You observe that the air which feeds the flame passes down the tube at one

    end, then goes along the horizontal tube, and ascends the tube at the

    other end in which the taper is placed.

    [Illustration: Fig. 32]

    If I stop the aperture through which the air enters, I stop combustion, as

    you perceive. I stop the supply of air, and consequently the candle goes

    out. But, now, what will you think of this fact? In a former experiment I

    shewed you the air going from one burning candle to a second candle. If I

    took the air proceeding from another candle, and sent it down by a

    complicated arrangement into this tube, I should put this burning candle

    out. But what will you say when I tell you that my breath will put out

    that candle? I do not mean by blowing at all, but simply that the nature

    of my breath is such that a candle cannot burn in it. I will now hold my

    mouth over the aperture, and without blowing the flame in any way, let no

    air enter the tube but what comes from my mouth. You see the result. I did

    not blow the candle out. I merely let the air which I expired pass into

    the aperture, and the result was that the light went out for want of

    oxygen, and for no other reason. Something or other–namely, my lungs–had

    taken away the oxygen from the air, and there was no more to supply the

    combustion of the candle. It is, I think, very pretty to see the time it

    takes before the bad air which I throw into this part of the apparatus has

    reached the candle. The candle at first goes on burning, but so soon as

    the air has had time to reach it, it goes out. And, now, I will shew you

    another experiment, because this is an important part of our philosophy.

    Here is a jar which contains fresh air, as you can see by the circumstance

    of a candle or gas-light burning it. I make it close for a little time,

    and by means of a pipe I get my mouth over it so that I can inhale the

    air. By putting it over water, in the way that you see, I am able to draw

    up this air (supposing the cork to be quite tight), take it into my lungs,

    and throw it back into the jar.

    [Illustration: Fig. 33.]

    We can then examine it, and see the result. You observe, I first take up

    the air, and then throw it back, as is evident from the ascent and descent

    of the water; and now, by putting a taper into the air, you will see the

    state in which it is, by the light being extinguished. Even one

    inspiration, you see, has completely spoiled this air, so that it is no

    use my trying to breathe it a second time. Now, you understand the ground

    of the impropriety of many of the arrangements among the houses of the

    poorer classes, by which the air is breathed over and over again, for the

    want of a supply, by means of proper ventilation, sufficient to produce a

    good result. You see how bad the air becomes by a single breathing; so

    that you can easily understand how essential fresh air is to us.

    To pursue this a little further, let us see what will happen with

    lime-water. Here is a globe which contains a little lime-water, and it is

    so arranged as regards the pipes, as to give access to the air within, so

    that we can ascertain the effect of respired or unrespired air upon it. Of

    course, I can either draw in air (through A), and so make the air that

    feeds my lungs go through the lime-water, or I can force the air out of my

    lungs through the tube (B), which goes to the bottom, and so shew its

    effect upon the lime-water.

    [Illustration: Fig. 34.]

    You will observe that, however long I draw the external air into the

    lime-water, and then through it to my lungs, I shall produce no effect

    upon the water–it will not make the lime-water turbid; but if I throw the

    air _from_ my lungs through the lime-water, several times in succession,

    you see how white and milky the water is getting, shewing the effect which

    expired air has had upon it; and now you begin to know that the atmosphere

    which we have spoiled by respiration is spoiled by carbonic acid, for you

    see it here in contact with the lime-water.

    I have here two bottles, one containing lime-water and the other common

    water, and tubes which pass into the bottles and connect them. The

    apparatus is very rough, but it is useful notwithstanding.

    [Illustration: Fig. 35.]

    If I take these two bottles, inhaling here and exhaling there, the

    arrangement of the tubes will prevent the air going backwards. The air

    coming in will go to my mouth and lungs, and in going out, will pass

    through the lime-water, so that I can go on breathing and making an

    experiment, very refined in its nature, and very good in its results. You

    will observe that the good air has done nothing to the lime-water; in the

    other case nothing has come to the lime-water but my respiration, and you

    see the difference in the two cases.

    Let us now go a little further. What is all this process going on within

    us which we cannot do without, either day or night, which is so provided

    for by the Author of all things that He has arranged that it shall be

    independent of all will? If we restrain our respiration, as we can to a

    certain extent, we should destroy ourselves. When we are asleep, the

    organs of respiration, and the parts that are associated with them, still

    go on with their action–so necessary is this process of respiration to

    us, this contact of the air with the lungs. I must tell you, in the

    briefest possible manner, what this process is. We consume food: the food

    goes through that strange set of vessels and organs within us, and is

    brought into various parts of the system, into the digestive parts

    especially; and alternately the portion which is so changed is carried

    through our lungs by one set of vessels, while the air that we inhale and

    exhale is drawn into and thrown out of the lungs by another set of

    vessels, so that the air and the food come close together, separated only

    by an exceedingly thin surface: the air can thus act upon the blood by

    this process, producing precisely the same results in kind as we have seen

    in the case of the candle. The candle combines with parts of the air,

    forming carbonic acid, and evolves heat; so in the lungs there is this

    curious, wonderful change taking place. The air entering, combines with

    the carbon (not carbon in a free state, but, as in this case, placed ready

    for action at the moment), and makes carbonic acid, and is so thrown out

    into the atmosphere, and thus this singular result takes place: we may

    thus look upon the food as fuel. Let me take that piece of sugar, which

    will serve my purpose. It is a compound of carbon, hydrogen, and oxygen,

    similar to a candle, as containing the same elements, though not in the

    same proportion–the proportions being as shewn in this table:–


    Carbon, . . . . 72


    Hydrogen, . . . 11 |



    Oxygen, . . . . 88_|

    This is, indeed, a very curious thing, which you can well remember, for

    the oxygen and hydrogen are in exactly the proportions which form water,

    so that sugar may be said to be compounded of 72 parts of carbon and 99

    parts of water; and it is the carbon in the sugar that combines with the

    oxygen carried in by the air in the process of respiration–so making us

    like candles–producing these actions, warmth, and far more wonderful

    results besides, for the sustenance of the system, by a most beautiful and

    simple process. To make this still more striking, I will take a little

    sugar; or, to hasten the experiment, I will use some syrup, which contains

    about three-fourths of sugar and a little water. If I put a little oil of

    vitriol on it, it takes away the water, and leaves the carbon in a black

    mass. [The Lecturer mixed the two together.] You see how the carbon is

    coming out, and before long we shall have a solid mass of charcoal, all of

    which has come out of sugar. Sugar, as you know, is food, and here we have

    absolutely a solid lump of carbon where you would not have expected it.

    And if I make arrangements so as to oxidize the carbon of sugar, we shall

    have a much more striking result Here is sugar, and I have here an

    oxidizer–a quicker one than the atmosphere; and so we shall oxidize this

    fuel by a process different from respiration in its form, though not

    different in its kind. It is the combustion of the carbon by the contact

    of oxygen which the body has supplied to it. If I set this into action at

    once, you will see combustion produced. Just what occurs in my

    lungs–taking in oxygen from another source, namely, the atmosphere–takes

    place here by a more rapid process.

    You will be astonished when I tell you what this curious play of carbon

    amounts to. A candle will burn some four, five, six, or seven hours. What,

    then, must be the daily amount of carbon going up into the air in the way

    of carbonic acid! What a quantity of carbon must go from each of us in

    respiration! What a wonderful change of carbon must take place under these

    circumstances of combustion or respiration! A man in twenty-four hours

    converts as much as seven ounces of carbon into carbonic acid; a milch cow

    will convert seventy ounces, and a horse seventy-nine ounces, solely by

    the act of respiration. That is, the horse in twenty-four hours burns

    seventy-nine ounces of charcoal, or carbon, in his organs of respiration,

    to supply his natural warmth in that time. All the warm-blooded animals

    get their warmth in this way, by the conversion of carbon, not in a free

    state, but in a state of combination. And what an extraordinary notion

    this gives us of the alterations going on in our atmosphere. As much as

    5,000,000 pounds, or 548 tons, of carbonic acid is formed by respiration

    in London alone in twenty-four hours. And where does all this go? Up into

    the air. If the carbon had been like the lead which I shewed you, or the

    iron which, in burning, produces a solid substance, what would happen?

    Combustion could not go on. As charcoal burns, it becomes a vapour and

    passes off into the atmosphere, which is the great vehicle, the great

    carrier for conveying it away to other places. Then, what becomes of it?

    Wonderful is it to find that the change produced by respiration, which

    seems so injurious to us (for we cannot breathe air twice over), is the

    very life and support of plants and vegetables that grow upon the surface

    of the earth. It is the same also under the surface, in the great bodies

    of water; for fishes and other animals respire upon the same principle,

    though not exactly by contact with the open air.

    Such fish as I have here [pointing to a globe of gold-fish] respire by the

    oxygen which is dissolved from the air by the water, and form carbonic

    acid; and they all move about to produce the one great work of making the

    animal and vegetable kingdoms subservient to each other. And all the

    plants growing upon the surface of the earth, like that which I have

    brought here to serve as an illustration, absorb carbon. These leaves are

    taking up their carbon from the atmosphere, to which we have given it in

    the form of carbonic acid, and they are growing and prospering. Give them

    a pure air like ours, and they could not live in it; give them carbon with

    other matters, and they live and rejoice. This piece of wood gets all its

    carbon, as the trees and plants get theirs, from the atmosphere, which, as

    we have seen, carries away what is bad for us and at the same time good

    for them,–what is disease to the one being health to the other. So are we

    made dependent, not merely upon our fellow-creatures, but upon our

    fellow-existers, all Nature being tied together by the laws that make one

    part conduce to the good of another.

    There is another little point which I must mention before we draw to a

    close–a point which concerns the whole of these operations, and most

    curious and beautiful it is to see it clustering upon and associated with

    the bodies that concern us–oxygen, hydrogen, and carbon, in different

    states of their existence. I shewed you just now some powdered lead, which

    I set burning[18]; and you saw that the moment the fuel was brought to the

    air, it acted, even before it got out of the bottle–the moment the air

    crept in, it acted. Now, there is a case of chemical affinity by which all

    our operations proceed. When we breathe, the same operation is going on

    within us. When we burn a candle, the attraction of the different parts

    one to the other is going on. Here it is going on in this case of the

    lead; and it is a beautiful instance of chemical affinity. If the products

    of combustion rose off from the surface, the lead would take fire, and go

    on burning to the end; but you remember that we have this difference

    between charcoal and lead–that, while the lead can start into action at

    once, if there be access of air to it, the carbon will remain days, weeks,

    months, or years. The manuscripts of Herculaneum were written with

    carbonaceous ink, and there they have been for 1,800 years or more, not

    having been at all changed by the atmosphere, though coming in contact

    with it under various circumstances. Now, what is the circumstance which

    makes the lead and carbon differ in this respect? It is a striking thing

    to see that the matter which is appointed to serve the purpose of fuel

    _waits_ in its action: it does not start off burning, like the lead and

    many other things that I could shew you; but which I have not encumbered

    the table with; but it waits for action. This waiting is a curious and

    wonderful thing. Candles–those Japanese candles, for instance–do not

    start into action at once, like the lead or iron (for iron finely divided

    does the same thing as lead), but there they wait for years, perhaps for

    ages, without undergoing any alteration. I have here a supply of coal-gas.

    The jet is giving forth the gas, but you see it does not take fire–it

    comes out into the air, but it waits till it is hot enough before it

    burns. If I make it hot enough, it takes fire. If I blow it out, the gas

    that is issuing forth waits till the light is applied to it again. It is

    curious to see how different substances wait–how some will wait till the

    temperature is raised a little, and others till it is raised a good deal.

    I have here a little gunpowder and some gun-cotton; even these things

    differ in the conditions under which they will burn. The gunpowder is

    composed of carbon and other substances, making it highly combustible; and

    the gun-cotton is another combustible preparation. They are both waiting,

    but they will start into activity at different degrees of heat, or under

    different conditions. By applying a heated wire to them, we shall see

    which will start first [touching the gun-cotton with the hot iron]. You

    see the gun-cotton has gone off, but not even the hottest part of the wire

    is now hot enough to fire the gunpowder. How beautifully that shews you

    the difference in the degree in which bodies act in this way! In the one

    case the substance will wait any time until the associated bodies are made

    active by heat; but in the other, as in the process of respiration, it

    waits no time. In the lungs, as soon as the air enters, it unites with the

    carbon; even in the lowest temperature which the body can bear short of

    being frozen, the action begins at once, producing the carbonic acid of

    respiration: and so all things go on fitly and properly. Thus you see the

    analogy between respiration and combustion is rendered still more

    beautiful and striking. Indeed, all I can say to you at the end of these

    lectures (for we must come to an end at one time or other) is to express a

    wish that you may, in your generation, be fit to compare to a candle; that

    you may, like it, shine as lights to those about you; that, in all your

    actions, you may justify the beauty of the taper by making your deeds

    honourable and effectual in the discharge of your duty to your fellow-men.


    [_Delivered before the_ ROYAL INSTITUTION, _on Friday, February 22,


    Whether I was to have the honour of appearing before you this evening or

    not, seemed to be doubtful upon one or two points. One of these I will

    mention immediately; the other may or may not appear during the course of

    the hour that follows. The first point is this. When I was tempted to

    promise this subject for your attention this evening, it was founded upon

    a promise, and a full intent of performing that promise, on the part of my

    friend Deville, of Paris, to come here to shew before you a phenomenon in

    metallurgic chemistry not common. In that I have been disappointed. His

    intention was to have fused here some thirty or forty pounds of platinum,

    and so to have made manifest, through my mouth and my statement, the

    principles of a new process in metallurgy, in relation to this beautiful,

    magnificent, and valuable metal; but circumstances over which neither he

    nor I, nor others concerned, have sufficient control, have prevented the

    fulfilment of that intention; and the period at which I learned the fact

    was so recent, that I could hardly leave my place here to be filled by

    another, or permit you, who in your kindness have come to hear what might

    be said, to remain unreceived in the best manner possible to me under the

    circumstances. I therefore propose to state, as well as I can, what the

    principles are on which M. Deville proceeds, by means of drawings, and

    some subordinate or inferior experiments. The metal platinum, of which you

    see some very fine specimens on the table, has been known to us about a

    hundred years. It has been wrought in a beautiful way in this country, in

    France, and elsewhere, and supplied to the consumer in ingots of this

    kind, or in plates, such as we have here, or in masses, that by their very

    fall upon the table indicate the great weight of the substance, which is,

    indeed, nearly at the head of all substances in that respect. This

    substance has been given to us hitherto mainly through the philosophy of

    Dr. Wollaston, whom many of us know, and it is obtained in great purity

    and beauty. It is a very remarkable metal in many points, besides its

    known special uses. It usually comes to us in grains. Here is a very fine

    specimen of native platinum in grains. Here is also a nugget or ingot, and

    here are some small pieces gathered out of certain alluvial soils in

    Brazil, Mexico, California, and the Uralian districts of Russia.

    It is strange that this metal is almost always found associated with some

    four or five other metals, most curious in their qualities and

    characteristics. They are called platiniferous metals; and they have not

    only the relation of being always found associated in this manner, but

    they have other relations of a curious nature, which I shall point out to

    you by a reference to one of the tables behind me. This substance is

    always native–it is always in the metallic state; and the metals with

    which it is found connected, and which are rarely found elsewhere, are

    palladium, rhodium, iridium, osmium, and ruthenium. We have the names in

    one of the tables arranged in two columns, representing, as you see, two

    groups–platinum, iridium, and osmium constituting one group; and

    ruthenium, rhodium, and palladium the other. Three of these have the

    chemical equivalent of 98-1/2, and the others a chemical equivalent of

    about half that number. Then the metals of one group have an extreme

    specific gravity–platinum being, in fact, the lightest of the three, or

    as light as the lightest. Osmium has a specific gravity of 21.4, and is

    the heaviest body in nature; platinum is 21.15, and iridium the same; the

    specific gravity of the other three being only about half that, namely,

    11.3, 12.1, and 11.8. Then there is this curious relation, that palladium

    and iridium are very much alike, so that you would scarcely know one from

    the other, though one has only half the weight of the other, and only half

    the equivalent power. So with iridium and rhodium, and osmium and

    ruthenium, which are so closely allied that they make pairs, being

    separated each from its own group. Then these metals are the most

    infusible that we possess. Osmium is the most difficult to fuse: indeed, I

    believe it never has been fused, while every other metal has. Ruthenium

    comes next, iridium next, rhodium next, platinum next (so that it ranks

    here as a pretty fusible metal, and yet we have been long accustomed to

    speak of the infusibility of platinum), and next comes palladium, which is

    the most fusible metal of the whole. It is a curious thing to see this

    fine association of physical properties coming out in metals which are

    grouped together somehow or other in nature, but, no doubt, by causes

    which are related to analogous properties in their situation on the

    surface of the earth, for it is in alluvial soils that these things are


    Now, with regard to this substance, let me tell you briefly how we get it.

    The process used to be this. The ore which I shewed you just now was

    taken, and digested in nitro-muriatic acid of a certain strength, and

    partly converted into a solution, with the leaving behind of certain

    bodies that I have upon the table.  The platinum being dissolved with care

    in acids, to the solution the muriate of ammonia was added, as I am about

    to add it here. A yellow precipitate was then thrown down, as you perceive

    is the case now; and this, carefully washed and cleansed, gave us that

    body [pointing to a specimen of the chloride of platinum and ammonium],

    the other elements, or nearly all, being ejected.  This substance being

    heated, gave us what we call platinum sponge, or platinum in the metallic

    state, so finely divided as to form a kind of heavy mass or sponge, which,

    at the time that Dr. Wollaston first sent it forth, was not fusible for

    the market or in the manufacturers’ workshops, inasmuch as the temperature

    required was so high, and there were no furnaces that could bring the mass

    into a globule, and cause the parts to adhere together. Most of our metals

    that we obtain from nature, and work in our shops, are brought at last

    into a mass by fusion.  I am not aware that there is in the arts or

    sciences any other than iron which is not so.  Soft iron we do not bring

    together by fusion, but by a process which is analogous to the one that

    was followed in the case of platinum, namely, welding; for these divided

    grains of spongy platinum having been well washed and sunk in water for

    the purpose of excluding air, and pressed together, and heated, and

    hammered, and pressed again, until they come into a pretty close, dense,

    compact mass, did so cohere, that when the mass was put into the furnace

    of charcoal, and raised to a high temperature, the particles, at first

    infinitely divided–for they were chemically divided–adhered the one to

    the other, each to all the rest, until they made that kind of substance

    which you see here, which will bear rolling and expansion of every kind.

    No other process than that has hitherto been adopted for the purpose of

    obtaining this substance from the particles by solution, precipitation,

    ignition, and welding. It certainly is a very fine thing to see that we

    may so fully depend upon the properties of the various substances we have

    to deal with; that we can, by carrying out our processes, obtain a

    material like this, allowing of division and extension under a rolling

    mill–a material of the finest possible kind, the parts being held

    together, not with interstices, not with porosity, but so continuous that

    no fluids can pass between them; and, as Dr. Wollaston beautifully shewed,

    a globule of platinum fused by the voltaic battery and the oxy-hydrogen

    blowpipe, when drawn into a wire, was not sounder or stronger than this

    wire made by the curious coalescence of the particles by the sticking

    power that they had at high temperatures. This is the process adopted by

    Messrs. Johnson and Matthey, to whose great kindness I am indebted for

    these ingots and for the valuable assistance I have received in the


    The treatment, however, that I have to bring before you is of another

    kind; and it is in the hope that we shall be able before long to have such

    a thing as the manufacture of platinum of this kind, that I am encouraged

    to come before you, and tell you how far Deville has gone in the matter,

    and to give you illustrations of the principles on which he proceeds. I

    think it is but fair that you should see an experiment shewing you the way

    in which we get the adhesion of platinum. Probably you all know of the

    welding of iron: you go into the smith’s shop, and you see him put the

    handle of a poker on to the stem, and by a little management and the

    application of heat he makes them one.  You have no doubt seen him put the

    iron into the fire and sprinkle a little sand upon it.  He does not know

    the philosophy he calls into play when he sprinkles a little sand over the

    oxide of iron, but he has a fine philosophy there, or practises it, when

    he gets his welding. I can shew you here this beautiful circumstance of

    the sticking together of the particles up to the fullest possible

    intensity of their combination. If you were to go into the workshops of

    Mr. Matthey, and see them hammering and welding away, you would see the

    value of the experiment I am about to shew you. I have here some

    platinum-wire.  This is a metal which resists the action of acids, resists

    oxidation by heat, and change of any sort; and which, therefore, I may

    heat in the atmosphere without any flux. I bend the wire so as to make the

    ends cross: these I make hot by means of the blowpipe, and then, by giving

    them a tap with a hammer, I shall make them into one piece. Now that the

    pieces are united, I shall have great difficulty in pulling them apart,

    though they are joined only at the point where the two cylindrical

    surfaces came together. And now I have succeeded in pulling the wire

    apart, the division is not at the point of welding, but where the force of

    the pincers has cut it, so that the junction we have effected is a

    complete one. This, then, is the principle of the manufacture and

    production of platinum in the old way.

    The treatment which Deville proposes to carry out, and which he has

    carried out to a rather large extent in reference to the Russian supply of

    platinum, is one altogether by heat, having little or no reference to the

    use of acids. That you may know what the problem is, look at this table,

    which gives you the composition of such a piece of platinum ore as I

    shewed you just now. Wherever it comes from, the composition is as

    complicated, though the proportions vary:–

    Platinum, . . . . . 76.4

    Iridium,. . . . . .  4.3

    Rhodium,. . . . . .  0.3

    Palladium,. . . . .  1.4

    Gold, . . . . . . .  0.4

    Copper, . . . . . .  4.1

    Iron, . . . . . . . 11.7

    Osmide of Iridium,.  0.5

    Sand, . . . . . . .  1.4



    This refers to the Uralian ore. In that state of combination, as shewn in

    the table, the iridium and osmium are found combined in crystals,

    sometimes to the amount of 0.5 per cent., and sometimes 3 or 4 per cent.

    Now, this Deville proposes to deal with in the dry way, in the place of

    dealing with it by any acid.

    I have here another kind of platinum; and I shew it to you for this

    reason. The Russian Government, having large stores of platinum in their

    dominions, have obtained it in a metallic state, and worked it into coin.

    The coin I have in my hand is a twelve silver rouble piece. The rouble is

    worth three shillings, and this coin is, therefore, of the value of

    thirty-six shillings. The smaller coin is worth half that sum; and the

    other, half of that. The metal, however, is unfit for coinage. When you

    have the two metals, gold and silver, used for coinage, you have a little

    confusion in the value of the two in the market; but when you have three

    precious metals (for you may call platinum a precious metal) worked into

    coin, they will be sure to run counter to one another. Indeed, the case

    did happen, that the price of platinum coin fixed by the Government was

    such, that it was worth while to purchase platinum in other countries, and

    make coin of it, and then take it into that country and circulate it. The

    result was, that the Russian Government stopped the issue. The composition

    of this coin is–platinum, 97.0; iridium, 1.2; rhodium, 0.5; palladium,

    0.25; a little copper, and a little iron. It is, in fact, bad platinum: it

    scales, and it has an unfitness for commercial use and in the laboratory,

    which the other well-purified platinum has not. It wants working over


    Now, Deville’s process depends upon three points,–upon intense heat,

    blowpipe action, and the volatility of certain metals. We know that there

    are plenty of metals that are volatile; but this, I think, is the first

    time that it has been proposed to use the volatility of certain

    metals–such as gold and palladium–for the purpose of driving them off

    and leaving something else behind. He counts largely upon the volatility

    of metals which we have not been in the habit of considering volatile, but

    which we have rather looked upon as fixed; and I must endeavour to

    illustrate these three points by a few experiments. Perhaps I can best

    show you what is required in the process of heating platinum by using that

    source of heat which we have here, and which seems to be almost

    illimitable–namely, the voltaic battery; for it is only in consequence of

    the heat that the voltaic battery affects the platinum. By applying the

    two extremities of the battery to this piece of platinum-wire, you will

    see what result we shall obtain. You perceive that we can take about this

    heating agent wherever we like, and deal with it as we please, limiting it

    in any way. I am obliged to deal carefully with it; but even that

    circumstance will have an interest for you in watching the experiment.

    Contact is now made. The electric current, when compressed into thin

    conducting-wires offering resistance, evolves heat to a large extent; and

    this is the power by which we work. You see the intense glow immediately

    imparted to the wire; and if I applied the heat continuously, the effect

    of the current would be to melt the wire. As soon as the contact is

    broken, the wire resumes its former appearance; and now that we make

    contact again, you perceive the glow as before. [The experiment was

    repeated several times in rapid succession.] You can see a line of light,

    though you can scarcely perceive the wire; and now that it has melted with

    the great heat, if you examine it, you will perceive that it is indeed a

    set of irregularities from end to end–a set of little spheres, which are

    strung upon an axis of platinum running through it. It is that wire which

    Mr. Grove described as being produced at the moment when fusion of the

    whole mass is commencing. In the same manner, if I take a tolerably thick

    piece of platinum, and subject it to the heat that can be produced by this

    battery, you will see the brilliancy of the effect produced. I shall put

    on a pair of spectacles for the experiment, as there is an injurious

    effect of the voltaic spark upon the eyes, if the action is continued; and

    it is neither policy nor bravery to subject any organ to unnecessary

    danger; and I want, at all events, to keep the full use of my eyes to the

    end of the lecture.

    You now see the action of the heat upon the piece of platinum–heat so

    great as to break in pieces the plate on which the drops of metal fall.

    You perceive, then, that we have sufficiently powerful sources of heat in

    nature to deal with platinum. I have here an apparatus by which the same

    thing can be shewn. Here is a piece of platinum, which is put into a

    crucible of carbon made at the end of one pole of the battery, and you

    will see the brilliant light that will be produced. There is our furnace,

    and the platinum is rapidly getting heated; and now you perceive that it

    is melted, and throwing off little particles. What a magnificent

    philosophical instrument this is. When you look at the result, which is

    lying upon the charcoal, you will see a beautifully fused piece of

    platinum. It is now a fiery globule, with a surface so bright, and smooth,

    and reflecting, that I cannot tell whether it is transparent, or opaque,

    or what. This, then, will give you an idea of what has to be done by any

    process that pretends to deal with thirty, or forty, or fifty pounds of

    platinum at once.

    Let me now tell you briefly what Deville proposes to do. First of all, he

    takes this ore, with its impurities, and mixes it (as he finds it

    essential and best) with its own weight of sulphuret of lead–lead

    combined with sulphur. Both the lead and the sulphur are wanted; for the

    iron that is there present, as you see by the table, is one of the most

    annoying substances in the treatment that you can imagine, because it is

    not volatile; and while the iron remains adhering to the platinum, the

    platinum will not flow readily. It cannot be sent away by a high

    temperature–sent into the atmosphere so as to leave the platinum behind.

    Well, then, a hundred parts of ore and a hundred parts of sulphuret of

    lead, with about fifty parts of metallic lead, being all mingled together

    in a crucible, the sulphur of the sulphuret takes the iron, the copper,

    and some of the other metals and impurities, and combines with them to

    form a slag; and as it goes on boiling and oxidising, it carries off the

    iron, and so a great cleansing takes place.

    Now, you ought to know that these metals, such as platinum, iridium, and

    palladium, have a strong affinity for such metals as lead and tin, and

    upon this a great deal depends. Very much depends upon the platinum

    throwing out its impurities of iron and so forth, by being taken up with

    the lead present in it. That you may have a notion of the great power that

    platinum has of combining with other metals, I will refer you to a little

    of the chemist’s experience–his bad experience. He knows very well that

    if he takes a piece of platinum-foil, and heats a piece of lead upon it,

    or if he takes a piece of platinum-foil, such as we have here, and heats

    things upon it that have lead in them, his platinum is destroyed. I have

    here a piece of platinum, and if I apply the heat of the spirit-lamp to

    it, in consequence of the presence of this little piece of lead which I

    will place on it, I shall make a hole in the metal. The heat of the lamp

    itself would do no harm to the platinum, nor would other chemical means;

    but because there is a little lead present, and there is an affinity

    between the two substances, the bodies fuse together at once. You see the

    hole I have made. It is large enough to put your finger in, though the

    platinum itself was, as you saw, almost infusible, except by the voltaic

    battery. For the purpose of shewing this fact in a more striking manner, I

    have taken pieces of platinum-foil, tin-foil, and lead-foil, and rolled

    them together; and if I apply the blowpipe to them, you will have, in

    fact, a repetition on a larger scale of the experiment you saw just now

    when the lead and platinum came together, and one spoiled the other. When

    the metals are laid one upon the other, and folded together and heat

    applied, you will not only see that the platinum runs to waste, but that

    at the time when the platinum and lead are combined there is ignition

    produced–there is a power of sustaining combustion. I have taken a large

    piece, that you may see the phenomenon on a large scale. You saw the

    ignition and the explosion which followed, of which we have here the

    results–the consequence of the chemical affinity between the platinum and

    the metals combined with it, which is the thing upon which Deville founds

    his first result.

    When he has melted these substances and stirred them well up, and so

    obtained a complete mixture, he throws in air upon the surface to burn off

    all the sulphur from the remaining sulphuret of lead; and at last he gets

    an ingot of lead with platinum–much lead, comparatively, and little

    platinum. He gets that in the crucible with a lot of scori?nd other

    things, which he treats afterwards. It is that platiniferous lead which we

    have to deal with in our future process. Now, let me tell you what he does

    with it. His first object is to get rid of the lead. He has thrown out all

    the iron, and a number of other things, and he has got this kind of

    compound indicated in the table. He may get it as high as 78 per cent. of

    platinum, and 22 of lead; or 5, or 10, or 15 of platinum, and 95, or 90,

    or 85 of lead (which he calls weak platinum), and he then places it in the

    kind of vessel that you see before you. Suppose we had the mixture here;

    we should have to make it hot, and then throw in air upon the surface. The

    combustible metal–that is, the lead–and the part that will oxidise, are

    thoroughly oxidised; the litharge would flow out in a fused state into a

    vessel placed to receive it, and the platinum remains behind.

    [Illustration: Fig. 36.]

    Here is the process which Deville adopts for the purpose of casting off

    the lead, after he has got out the platinum from the ore. (Having made use

    of your friend, you get rid of him as quickly as you can.) He gets his

    heat by applying the combination of oxygen and hydrogen, or of carburetted

    fuel, for the purpose of producing a fire. I have here a source of

    coal-gas; there I have a source of hydrogen; and here I have a source of

    oxygen. I have here also one of the blowpipes used by Deville in his

    process for working platinum in the way I have spoken of. There are two

    pipes, and one of them goes to the source of coal-gas, and the other to

    the supply of oxygen.

    [Illustration: Fig. 37.]

    By uniting these we obtain a flame of such a heat as to melt platinum. You

    will, perhaps, hardly imagine what the heat is, unless you have some proof

    of it; but you will soon see that I have actually the power of melting

    platinum. Here is a piece of platinum-foil running like wax under the

    flame which I am bringing to bear against it. The question, however, is

    whether we shall get heat enough to melt, not this small quantity, but

    large masses–many pounds of the metal. Having obtained heat like this,

    the next consideration is what vessel is he to employ which could retain

    the platinum when so heated, or bear the effects of the flame?  Such

    vessels are happily well supplied at Paris, and are formed of a substance

    which surrounds Paris; it is a kind of chalk (called, I believe, by

    geologists, _calcaire grossi?_), and it has the property of enduring an

    extreme degree of heat. I am now going to get the highest heat that we can

    obtain. First, I shew you the combustion of hydrogen by itself. I have not

    a large supply, because the coal-gas is sufficient for most of our

    purposes. If I put a piece of lime obtained from this chalk into the gas,

    you see we get a pretty hot flame, which would burn one’s fingers a good

    deal But now let me subject a piece of it to the joint action of oxygen

    and hydrogen. I do this for the purpose of shewing you the value of lime

    as a material for the furnaces and chambers that are to contain the

    substances to be operated on, and that are consequently to sustain the

    action of this extreme heat. Here we have the hydrogen and the oxygen,

    which will give the most intense heat that can be obtained by chemical

    action; and if I put a piece of lime into the flame, we get what is called

    the lime-light. Now, with all the beauty and intensity of action which you

    perceive, there is no sensible deterioration of the lime except by the

    mechanical force of the current of gases rushing from the jet against the

    lime, sweeping away such particles as are not strongly aggregated. “Vapour

    of lime” some call it; and it may be so, but there is no other change of

    the lime than that under the action of heat of this highly-exalted

    chemical condition, though almost any other substance would melt at once.

    Then, as to the way in which the heat is applied to the substance. It is

    all very well for me to take a piece of antimony, and fuse it in the flame

    of a blowpipe. But if I tried this piece in the ordinary lamp flame, I

    should do nothing; if I tried a smaller piece, I should do little or

    nothing; and if I tried a still smaller piece, I should do little or

    nothing; yet I have a condition which will represent what Deville carries

    to the highest possible extent, and which we all carry to the highest

    extent, in the use of the blowpipe. Suppose I take this piece of antimony:

    I shall not be able to melt it in that flame of the candle by merely

    holding it there; yet, by taking pains, we can even melt a piece of

    platinum there. This is a preparation which I made for the purpose of

    proving the fusibility of platinum in a common candle. There is a piece of

    wire, drawn by that ingenious process of Dr. Wollaston’s, not more than

    the three-thousandth part of an inch in diameter. He put the wire into the

    middle of a cylinder of silver, and drew both together until the whole

    compound was exceedingly thin; and then he dissolved away the silver by

    nitric acid. There was left in the centre a substance which I can scarcely

    see with an eye-glass, but which I know is there, and which I can make

    visible, as you see, by putting it into the candle, where the heat makes

    it glow like a spark. I have again and again tried this experiment

    up-stairs in my own room, and have easily fused this platinum-wire by a

    common candle. You see we have, therefore, heat enough in the candle, as

    in the voltaic battery, or in the highly-exalted combustion of the

    blowpipe, but we do not supply a continuous source of heat. In the very

    act of this becoming ignited, the heat radiates so fast that you cannot

    accumulate enough to cause the fusion of the wire, except under the most

    careful arrangement. Thus I cannot melt that piece of antimony by simply

    putting it into the candle; but if I put it upon charcoal, and drive the

    fiery current against it, there will be heat enough to melt it. The beauty

    of the blowpipe is, that it sends hot air (making hot air by the

    combustion of the flame) against the thing to be heated. I have only to

    hold the antimony in the course of that current, and particle by particle

    of the current impinges upon the antimony, and so we get it melted. You

    now see it red-hot, and I have no doubt it will continue to burn if I

    withdraw it from the flame and continue to force the air on it. Now, you

    see it burning without any heat but that of its own combustion, which I am

    keeping up by sending the air against it. It would go out in a moment if I

    took away the current of air from it; but there it is burning, and the

    more air I give it, by this or any other action, the better it is. So,

    then, we have here not merely a mighty source of heat, but a means of

    driving the heat forcibly against substances.

    Let me shew you another experiment with a piece of iron. It will serve two

    purposes–shewing you what the blowpipe does as a source of heat, and what

    it does by sending that heat where it is wanted. I have taken iron in

    contrast with silver or other metals, that you may see the difference of

    action, and so be more interested in the experiment. Here is our fuel, the

    coal-gas; and here our oxygen. Having thus my power of heat, I apply it to

    the iron, which, as you see, soon gets red-hot. It is now flowing about

    like a globule of melted mercury. But observe, I cannot raise any vapour:

    it is now covered with a coat of melted oxide, and unless I have a great

    power in my blowpipe, it is hardly possible to break through it. Now,

    then, you see these beautiful sparks: you have not only a beautiful kind

    of combustion, but you see the iron is being driven off, not producing

    smoke, but burning in a fixed condition. How different this is from the

    action of some other metals–that piece of antimony, for instance, which

    we saw just now throwing off abundance of fumes. We can, of course, burn

    away this iron by giving plenty of air to it; but with the bodies which

    Deville wants to expose to this intense heat he has not that means: the

    gas itself must have power enough to drive off the slag which forms on the

    surface of the metal, and power to impinge upon the platinum so as to get

    the full contact that he wants for the fusion to take place. We see here,

    then, the means to which he resorts–oxygen, and either coal-gas or

    water-gas[19], or pure hydrogen, for producing heat, and the blowpipe for

    the purpose of impelling the heated current upon the metals.

    I have two or three rough drawings here, representing the kind of furnaces

    which he employs. They are larger, however, than the actual furnaces he

    uses. Even the furnace in which he carries on that most serious operation

    of fusing fifty pounds of platinum at once is not much more than half the

    size of the drawing. It is made of a piece of lime below and a piece of

    lime above. You see how beautifully lime sustains heat without altering in

    shape; and you may have thought how beautifully it prevents the

    dissipation of the heat by its very bad conducting powers.

    [Illustration: Fig. 38]

    While the front part of the lime which you saw here was so highly ignited,

    I could at any moment touch the back of it without feeling any annoyance

    from the heat So, by having a chamber of lime of this sort, he is able to

    get a vessel to contain these metals with scarcely any loss of heat. He

    puts the blowpipes through these apertures, and sends down these gases

    upon the metals, which are gradually melted. He then puts in more metal

    through a hole at the top. The results of the combustion issue out of the

    aperture which you see represented. If there be strips of platinum, he

    pushes them through the mouth out of which the heated current is coming,

    and there they get red-hot and white-hot before they get into the bath of

    platinum. So he is able to fuse a large body of platinum in this manner.

    When the platinum is melted, he takes off the top and pours out from the

    bottom piece, like a crucible, and makes his cast. This is the furnace by

    which he fuses his forty pounds or fifty pounds of platinum at once. The

    metal is raised to a heat that no eye can bear. There is no light and

    shadow, no chiaro-oscuro there; all is the same intensity of glow. You

    look in, and you cannot see where the metal or the lime is; it is all as

    one. We have, therefore, a platform with a handle, which turns upon an

    axis, that coincides with the gutter that is formed for the pouring of the

    metal; and when all is known to be ready, by means of dark glasses, the

    workmen take off the top piece and lift up the handle, and the mould being

    then placed in a proper position, he knows that the issue of the metal

    will be exactly in the line of the axis. No injury has ever happened from

    the use of this plan. You know with what care it is necessary to carry

    such a vessel of mercury as we have here, for fear of turning it over on

    one side or the other; but if it be a vessel of melted platinum, the very

    greatest care must be used, because the substance is twice as heavy: yet

    no injury has been done to any of the workmen in this operation.

    I have said that Deville depends upon intense heat for carrying off

    vapour; and this brings me to the point of shewing how vapours are carried

    off. Here is a basin of mercury, which boils easily, as you know, and

    gives us the opportunity of observing the facts and principles which are

    to guide us. I have here two poles of the battery, and if I bring them

    into contact with the mercury, see what a development of vapour we have.

    The mercury is flying off rapidly; and I might, if I pleased, put all the

    company around me in a bath of mercury vapour. And so, if we take this

    piece of lead and treat it in the same way, it will also give off vapour.

    Observe the fumes that rise from it; and even if it was so far enclosed

    from the air that you could not form any litharge, you would still have

    those abundant fumes flying off. I may also take a piece of gold, and shew

    you the same thing. I have here a piece of gold which I put upon a clean

    surface of Paris limestone. Applying the heat of the blowpipe to it, you

    see how the heat drives off the vapour; and if you notice at the end of

    the Lecture, you will observe on the stone a purple patch of condensed

    gold. Thus you see a proof of the volatilisation of gold. It is the same

    with silver. You will not be startled if I sometimes use one agent and

    sometimes another to illustrate a particular point. The volatility of gold

    and silver is the same thing, whether it be effected by the voltaic

    battery or by the blowpipe. [A lump of silver was placed in a charcoal

    crucible between the poles of a voltaic battery.] Now, look at the fumes

    of silver, and observe the peculiar and beautiful green colour which they

    produce. We shall now shew you this same process of boiling the silver,

    cast on a screen from the electric lamp which you have before you; and

    while Dr. Tyndall is kindly getting the lamp ready for this purpose, let

    me tell you that Deville proposes to throw out in this way all these

    extraneous things that I have spoken of, except two–namely, iridium and

    rhodium. It so happens, as he says, that iridium and rhodium do make the

    metal more capable of resisting the attacks of acids than platinum itself.

    Alloys are compounded up to 25 per cent. of rhodium and iridium, by which

    the chemical inaction of the platinum is increased, and also its

    malleability and other physical properties. [The image of the voltaic

    discharge through vapour of silver was now thrown upon the screen.] What

    you have now on the screen is an inverted image of what you saw when we

    heated the silver before. The fine stream that you see around the silver

    is the discharge of the electric force that takes place, giving you that

    glorious green light which you see in the ray; and if Dr. Tyndall will

    open the top of the lamp, you will see the quantity of fumes that will

    come out of the aperture, shewing you at once the volatility of silver.

    I have now finished this imperfect account. It is but an apology for not

    having brought the process itself before you. I have done the best I could

    under the circumstances; and I know your kindness well, for if I were not

    aware that I might trust to it, I would not appear here so often as I have

    done. The gradual loss of memory and of my other faculties is making

    itself painfully evident to me, and requires, every time I appear before

    you, the continued remembrance of your kindness to enable me to get

    through my task. If I should happen to go on too long, or should fail in

    doing what you might desire, remember it is yourselves who are chargeable,

    by wishing me to remain. I have desired to retire, as I think every man

    ought to do before his faculties become impaired; but I must confess that

    the affection I have for this place, and for those who frequent this

    place, is such, that I hardly know when the proper time has arrived.


[Footnote 1: Page 16. The Royal George sunk at Spithead on The 29th of

August, 1782. Colonel Pasley commenced operations for the removal of the

wreck by the explosion of gunpowder, in August, 1839. The candle which

Professor Faraday exhibited must therefore have been exposed to the action

of salt water for upwards of fifty-seven years.]

[Footnote 2: Page 17. The fat or tallow consists of a chemical combination

of fatty acids with glycerine. The lime unites with the palmitic, oleic,

and stearic acids, and separates the glycerine. After washing, the

insoluble lime soap is decomposed with hot dilute sulphuric acid. The

melted fatty acids thus rise as an oil to the surface, when they are

decanted. They are again washed and cast into thin plates, which, when

cold, are placed between layers of cocoa-nut matting, and submitted to

intense hydraulic pressure. In this way the soft oleic acid is squeezed

out, whilst the hard palmitic and stearic acids remain. These are further

purified by pressure at a higher temperature, and washing in warm dilute

sulphuric acid, when they are ready to be made into candles. These acids

are harder and whiter than the fats from which they were obtained, whilst

at the same time they are cleaner and more combustible.]

[Footnote 3: Page 19. A little borax or phosphorus salt is sometimes

added, in order to make the ash fusible.]

[Footnote 4: Page 27. Capillary attraction or repulsion is the cause which

determines the ascent or descent of a fluid in a capillary tube. If a

piece of thermometer tubing, open at each end, be plunged into water, the

latter will instantly rise in the tube considerably above its external

level. If, on the other hand, the tube be plunged into mercury, a

repulsion instead of attraction will be exhibited, and the level of the

mercury will be lower in the tube than it is outside.]

[Footnote 5: Page 29. The late Duke of Sussex was, we believe, the first

to shew that a prawn might be washed upon this principle. If the tail,

after pulling off the fan part, be placed in a tumbler of water, and the

head be allowed to hang over the outside, the water will be sucked up the

tail by capillary attraction, and will continue to run out through the

head until the water in the glass has sunk so low that the tail ceases to

dip into it.]

[Footnote 6: Page 37. The alcohol had chloride of copper dissolved in it:

this produces a beautiful green flame.]

[Footnote 7: Page 54. Lycopodium is a yellowish powder found in the fruit

of the club moss (_Lycopodium clavatum_). It is used in fireworks.]

[Footnote 8: Page 58. Bunsen has calculated that the temperature of the

oxyhydrogen blowpipe is 8061? Centigrade. Hydrogen burning in air has a

temperature of 3259? C., and coal-gas in air, 2350? C.]

[Footnote 9: Page 60. The following is the action of the sulphuric acid in

inflaming the mixture of sulphuret of antimony and chlorate of potassa. A

portion of the latter is decomposed by the sulphuric acid into oxide of

chlorine, bisulphate of potassa, and perchlorate of potassa. The oxide of

chlorine inflames the sulphuret of antimony, which is a combustible body,

and the whole mass instantly bursts into flame.]

[Footnote 10: Page 63. The “air-burner,” which is of such value in the

laboratory, owes its advantage to this principle. It consists of a

cylindrical metal chimney, covered at the top with a piece of rather

coarse iron-wire gauze. This is supported over an argand burner, in such a

manner that the gas may mix in the chimney with an amount of air

sufficient to burn the carbon and hydrogen simultaneously, so that there

may be no separation of carbon in the flame with consequent deposition of

soot. The flame, being unable to pass through the wire gauze, burns in a

steady, nearly invisible manner above.]

[Footnote 11: Page 74. Water is in its densest state at a temperature of

39.1? Fahrenheit]

[Footnote 12: Page 74. A mixture of salt and pounded ice reduces the

temperature from 32? F. to zero–the ice at the same time becoming fluid.]

[Footnote 13: Page 82. Potassium, the metallic basis of potash, was

discovered by Sir Humphrey Davy in 1807, who succeeded in separating it

from potash by means of a powerful voltaic battery. Its great affinity for

oxygen causes it to decompose water with evolution of hydrogen, which

takes fire with the heat produced.]

[Footnote 14: Page 98. Professor Faraday has calculated that there is as

much electricity required to decompose one grain of water as there is in a

very powerful flash of lightning.]

[Footnote 15: Page 101. A solution of acetate of lead submitted to the

action of the voltaic current, yields lead at the negative pole, and brown

peroxide of lead at the positive pole. A solution of nitrate of silver,

under the same circumstances, yields silver at the negative pole, and

peroxide of silver at the positive pole.]

[Footnote 16: Page 129. The gas which is thus employed as a test for the

presence of oxygen, is the binoxide of nitrogen, or nitrous oxide. It is a

colourless gas, which, when brought in contact with oxygen, unites with

it, forming hyponitric acid, the red gas referred to.]

[Footnote 17: Page 152. _Marble_ is a compound of carbonic acid and lime.

The muriatic acid being the stronger of the two, takes the place of the

carbonic acid, which escapes as a gas, the residue forming muriate of lime

or chloride of calcium.]

[Footnote 18: Page 186. _Lead pyrophorus_ is made by heating dry tartrate

of lead in a glass tube (closed at one end, and drawn out to a fine point

at the other) until no more vapours are evolved. The open end of the tube

is then to be sealed before the blowpipe. When the tube is broken and the

contents shaken out into the air, they burn with a red flash.]

[Footnote 19: Page 216. _Water-gas_ is formed by passing vapour of water

over red-hot charcoal or coke. It is a mixture of hydrogen and carbonic

oxide; each of which is an inflammable gas.]

Poster’s note: “combustion that makes!” was corrected from a misprint

“combusion that makes!” in the original.

End of The Chemical History Of A Candle

by Michael Faraday


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