CHAPTER III. TESTIMONY OF OXYGEN. Religion and Chemistry | ||
3. CHAPTER III.
TESTIMONY OF OXYGEN.
WERE we to limit our regards to those physical qualities of the atmosphere which we studied in the first two chapters, we should overlook the most wonderful adaptations in its divine economy. These properties belong to the atmosphere, in great measure at least, in virtue of its aeriform condition, and, so far as we know, an atmosphere composed of other gases, and still having the same density, would soften the intensity of the light, and diffuse the genial influences of the sun's heat, as well as air. Not so, however, with the chemical qualities of the atmosphere, which we are next to consider. These belong to the atmosphere solely as air, and could not have been obtained with any other known materials.
When a chemist wishes to investigate the nature of a new substance, his first step is to analyze it. Let us, therefore, as a preliminary to our present inquiry, ascertain what is the composition of this aeriform matter we call air. The air has been analyzed hundreds of times in every latitude and in every climate; and the result has been uniformly that which is given in the following table:—
Oxygen | 20.61 |
Nitrogen | 77.95 |
Carbonic Dioxide | .04 |
Aqueous Vapor (average) | 1.40 |
Nitric Acid,} | |
Ammonia,} | traces. |
Carburetted Hydrogen,} | ________ |
100.00 |
Oxygen | 1,233,010 billions of tons. |
Nitrogen | 3,994,593 '' '' |
Carbonic Dioxide | 5,287 '' '' |
Aqueous Vapor | 54,460 '' '' |
Besides oxygen and nitrogen gases, which, as you will notice, are the chief constituents, there are always present in the atmosphere the vapor of water, carbonic dioxide, and ammonia gas; and if we add to these uniform constituents the various exhalations constantly arising from the earth, we shall have as accurate an idea of the composition of the air as chemistry can give. While, however, the proportions of oxygen and nitrogen are almost absolutely constant, those of the other ingredients are very fluctuating, and the total quantity exceedingly small, never amounting in all, exclusive of aqueous vapor, to more than one part in a thousand, unless in some confined locality, and under very unusual circumstances.
Moreover, we must carefully avoid the error of considering air as a distinct substance, like water or coal. On the contrary, it is merely a mechanical mixture of its constituent gases, and is in no sense a definite chemical compound. Indeed, we may regard the globe as surrounded by at least three separate atmospheres,—one of oxygen, one of nitrogen, and one of aqueous vapor,—all existing simultaneously in the same space, yet each entirely distinct from the other two, and only very slightly influenced by their presence. To each of these atmospheres the Author of nature has assigned separate and different functions. They are like so many servants in a household, each with a distinct set of duties, which are discharged with a fidelity and diligence unknown to any earthly service. Let us consider what those duties are, and see how skilfully each is adapted to the offices which it is designed to fill.
Were all the other constituents of the air removed, the earth would still be surrounded by an atmosphere of oxygen, having about one-fifth of the density, and exerting at the surface of the globe about one-fifth of the pressure, of the present atmosphere. In studying the chemical relations of air, let us begin with some of the more
It is easy to prepare oxygen in a pure state. It is then a perfectly colorless and transparent gas, and so persistently does it retain its aeriform condition that it cannot be reduced to the liquid state by pressure alone. A German chemist, Natterer, submitted this gas to a pressure of over forty-five thousand pounds, or twenty tons on a square inch, but he did not succeed in changing its condition. More recently, by the combined action of great pressure and the most intense cold which can be artificially produced, all the gases formerly called permanent have been liquefied, and oxygen among the number. But this remarkable result, while it shows conclusively that the so-called permanent gases differed from other forms of aeriform matter in degree only, and not in kind, also brings into prominence the extreme qualities of these constituents of our atmosphere. Most aeriform substances may be reduced to liquids by pressure under a very moderate reduction of temperature; [*] but oxygen
The importance of this fact will be seen at once on comparing the condition of the oxygen and nitrogen in the atmosphere with that of the aqueous vapor. A fall of temperature of only a few degrees will generally condense a portion of the vapor, and, small as is its relative amount, the resulting rain is at times poured down upon the earth in deluging floods; and if you consider what must have been the destructive results had the whole mass of the atmosphere been liable to a similar fluctuation, even under extreme conditions, you will discover in the permanency of oxygen a most obvious adaptation of its properties to the thermal condition of our globe.
The permanently aeriform state of oxygen will appear still more remarkable when we consider how largely it enters into the composition of the solid crust of the earth. Oxygen belongs to that class
Oxygen gas, like all other forms of aeriform matter, tends to expand, and can be prevented from obeying this natural tendency only by enclosing
As the air is now constituted, there is a constancy of pitch, however far sound travels. Any tone once generated remains the same tone until it dies away. Its degree of loudness alters in proportion to the distance of the listener, but the pitch is constant. Were it not, however, for this law of diffusion,— were the atmosphere not perfectly homogeneous, and the gases of which it consists even partially separated,—there would have been a very different result. The constancy of pitch could no longer have been depended upon. The sound as it travelled would vary its pitch with the ever-varying medium through which it passed, and would arrive at the ear with a tone entirely different from that with which it started. Nor would it require any great difference in the medium to produce a sensible result and to confuse all those delicate differences of pitch on which the whole art of music depends. Whenever, therefore, you may be next enjoying the grand Pastoral Symphony of Beethoven or the Requiem of Mozart, recall the careful adjustment of forces by which alone these magnificent creations of genius were rendered possible, and you cannot fail to recognize in this simple law of nature the same hand that first strung the lyre and made the soul of man responsive to its seven notes.
Returning again to the qualities of oxygen, let us
And here I must correct an erroneous, although very common impression, that there is something substantial in fire. This is one of those ideas, originating in an illusion of the senses, which we have inherited from a more ignorant age, and which our modern science cannot wholly dispel from the popular mind. Fire was formerly regarded as one of the elementary forms of matter, and all burning was supposed to consist in the escape of this principle of fire, previously pent up in the combustible substance. In support of this doctrine the old philosophers confidently pointed at flame as the visible manifestation of the escaping fire-element; and, childish as this doctrine may seem, it was the prevalent belief of the world for at least two thousand years.
The last phase which this doctrine assumed was the phlogiston theory of the last century. In the hands of Bergmann and Stahl, the vague ideas of the time received a more material form, and were embodied in a philosophical system. They termed the principle of fire phlogiston, and burning, or the escape of fire, dephlogistication, and their ingenious system did not a little to retard the progress of truth. The philosophers of that age either took no account of the increase of weight which results from burning, or attempted to explain the few instances in which the fact was forced upon their attention by the fanciful notion of Aristotle—that the essence of fire was specifically light. Hence, they reasoned,
Burning is merely chemical change, and all combustion with which we are familiar in common life is a chemical combination of the burning substance, whether it be coal, wood, oil, or gas, with the oxygen of the air. Combustion is simply a process of chemical combination, and the light and heat which are evolved in the process are only the concomitants of the chemical change. Why those mysterious influences of light and heat are radiated from the coal which is combining with oxygen in our grates, we may understand better hereafter; but this much we already know,—the sensations of light and heat are caused by waves of an ethereal medium breaking upon the extremities of the delicate nerves of our human organism; and such waves are set in motion during the chemical change which we call combustion. What the chemist mostly studies, however, is the change itself, and to this we will for the present confine our attention.
The chief products of ordinary combustion, that is,
Moreover, this smoke, though so long unnoticed by man, was not overlooked by the Author of nature. It is a part of his grand and beneficent design in the scheme of organic nature. No sooner do the products of that wood burning on the hearth escape into the free expanse of the outer air, than a new cycle of changes begins. The carbonic dioxide and the aqueous vapor, after roving at liberty for a time, are absorbed by the leaves of some wide-spreading tree, smiling in the sunshine, and in the tiny laboratory of their green cells are worked up by those wonderful agents, the sun-rays, into new wood, absorbing from the sun a fresh supply of power, which is destined, perhaps, to shed warmth and light around the fireside of a future generation.
But let us not anticipate our subject. In a future
In order to evoke the latent forces in the oxygen of the atmosphere, it is not necessary, however, to raise the temperature of any considerable portion either of the gas or of the combustible. There is a provision in nature by which chemical combination, once started at any portion of the combustible mass, is sustained until the whole is consumed. All chemical combination is attended by the evolution of heat, and in the combination of oxygen with most combustible substances the amount of heat thus generated is so great, that by the burning of one portion sufficient heat is evolved to raise the temperature of a second portion to the point of ignition, and thus the process is continued. Consider, for example, what takes place in the burning of a jet of gas. We start the combustion by bringing the flame of a lighted match over the orifice of the burner. By this the temperature of the gas and that of the air surrounding it are raised to a red heat, and chemical combination at once ensues. But the chemical union, as just stated, is attended with the evolution of great heat, which, before it is dissipated, raises to the point of ignition the temperature of the next portion of gas issuing from the burner. This, combining in its turn with oxygen, generates a fresh quantity of heat, and thus keeps up the combustion so long as the gas is supplied. What I have shown to be true of a gas
Thus it appears that burning is chemical combination with oxygen, that this union is attended with the evolution of heat, and that a high temperature is the condition under which oxygen manifests its latent power. But, you may say, these facts do not explain the difference between the two states of oxygen, they merely give the conditions under which these states are manifested; and this is true. Why it is that at one temperature oxygen is so completely passive, and at another temperature, a few hundred degrees higher, so highly active, we cannot fully explain; but the facts are undisputed.
The temperature at which oxygen assumes its active condition is called the point of ignition. Although fixed for each substance, it differs very greatly with the different kinds of combustible matter, being determined, apparently, by their relative affinities for the great fire-element. Thus phosphorus ignites at a temperature less than that of boiling water, sulphur at about 500°, wood only at a full red-heat, anthracite coal at a white-heat, while iron requires the highest heat of a blacksmith's forge. Beginning with a phosphorus match, which can be ignited by friction, and using the more combustible materials as kindlings, we can readily attain in our furnaces the highest temperature required, and thus the energies of this powerful agent are fully at the command of man. But notice at the same time
But even this precaution would have been insufficient to secure safety, were it not that the active energies of oxygen, even when aroused, have been most carefully tempered by extreme dilution. It would be easy to show by experiment that the slowness of combustion depends on the fact that in the atmosphere oxygen is mixed with a great mass of an inert gas, and the proportions have been so adjusted in the scheme of creation as generally to restrain the awakened energies of the fire-element within the narrow limits which man appoints; but when, through his misfortune or carelessness, it overrides these limits, and, from administering to man's wants, becomes the agent of his destruction, we are reminded in the awful conflagration by what a delicate tenure we hold our earthly possessions, and how small a change would be sufficient to involve all organized matter in a general conflagration. Remember now that fire is one of the most valuable servants of mankind; that it is the source of all artificial heat and light; that in the steam-engine it is the apparent origin of that power which animates the commerce and the industry of the civilized world; that under its influence iron becomes plastic,
If I have succeeded in making clear the relations of this twofold character of oxygen to man and his works, I think that you cannot fail to have been
If the crust of the globe is a fair sample of the whole mass, oxygen was the chief material employed by the Great Architect in constructing our earth. Moreover, world-building was a process of burning, like those we have been studying, and the foundations of the earth were undoubtedly laid in flames.
When we attempt to break up the various materials around us into simpler parts, we soon reach a class of substances which cannot be further decomposed. Simple inspection will show that granite rock, for example, is a mixture of three minerals, called feldspar, mica, and quartz. We know,
We call all substances which have never yet been decomposed, whatever may be their nature, chemical elements, and of such some seventy are now known. Setting apart oxygen as the supporter of combustion, the great mass of the remaining elements are combustible; that is, under certain conditions they combine rapidly with oxygen, evolving light and heat. Indeed, many of the combustible substances with which we are most familiar are elements. Charcoal is an element, phosphorus is an element, sulphur is an element, iron and all other metals are elements, and out of such combustible materials, together with oxygen, the world is made, but chiefly out of oxygen.
When we burn charcoal in air, or in pure oxygen gas, the burning is a process of world-making. The
I have at the bottom of this closed glass tube a small piece of a yellowish-white metal, looking very much like a flattened shot; and so it is, but the metal is not lead, although it resembles lead very closely. Like lead it is quite soft, and can be easily beaten into leaves thinner than writing paper; but it is very much lighter than lead, and tarnishes so rapidly in the air that we are obliged to keep it thus protected. We call the metal calcium, and although you may never have seen the substance before, it is one of the most abundant metals in nature, yet seldom seen, because of the extreme difficulty with which it is extracted from its ores. When heated to redness, calcium burns with a brilliant white light and a scintillating flame. In burning, it combines, of course, with oxygen, and the result is lime, common quick lime, such as is used for making mortar. This is a process which in the original world-making must have played a very important part, for lime rocks form a large portion of the earth's crust. None of these rocks, however, will slake like quick-lime, and we must go a step further in our world-building, and bring in the agency of water, before we can reach the actual condition of things.
We have now before us two products of burning, one a solid, called lime, made by uniting calcium with oxygen, the other a gas, called carbonic dioxide, made by uniting charcoal with oxygen. Both are soluble to a certain extent in water, and these clear solutions, called lime-water and soda-water respectively, are even more familiar to you than the substances themselves. Mix now the solutions together. The water becomes at once very turbid, and there soon settles from it a white powder. The lime and carbonic dioxide have united, and this is the result. If we collect and examine the white powder we shall find that it is chalk, and from the same material, spread in thick layers over the ocean-bed, and subsequently hardened by the mutual action of heat and water, have been formed limestone, marble, and the different varieties of lime rock, which are all ores of calcium.
But we may study with profit a second example of world-building. I have here a small quantity of another very abundant element, called silicon, but, like calcium, a comparative rarity, because it is with difficulty obtained pure. It resembles in many respects carbon, and has been observed in three different states, corresponding to charcoal, graphite, and diamond Like carbon, it also is combustible, combining with the oxygen of the air when heated to a high temperature, and forming a very hard white solid, called by chemists silica, which is the same thing as quartz, rock-crystal, agate, jasper, calcedony, opal, etc. All these familiar minerals are merely different conditions of this one material, and
Setting aside the silica for a moment, let us turn to another very widely distributed element, called aluminum. This brilliant white metal, comparing favorably even with silver in lustre, was, until very recently, as great a rarity as calcium or silicon; but within a few years a process has been discovered by which it can be extracted from its ore at a cost sufficiently low to render the metal available in the arts, and it has now come into quite general use for making mathematical instruments, for jewelry, and for similar purposes. It forms also, with copper, a valuable alloy, which does not readily tarnish, and resembles gold so closely that the two cannot be distinguished by their external appearance.
Aluminum, like most of the metals, is combustible, although it does not burn readily in the air, unless the temperature is very high and the metal finely subdivided; but it then burns very brilliantly, emitting a vivid light, and forming a compound called by chemists alumina, which is melted by the intense heat to a yellowish transparent glass, and is the same substance from which nature makes the sapphire and the ruby. Emery also, which, on account of its great hardness, is used so largely for
Taking next the element magnesium, which is also a brilliant white metal, allied to zinc, you notice that it takes fire even in the flame of a candle, and burns with dazzling brilliancy. The result is magnesia, so much used as a medicine. Unite magnesia to silica, and we have, according to the proportions, hornblende or augite, two minerals which abound in many varieties of rock. Add water to the composition, and we get also serpentine or soapstone, with several other allied mineral species.
I might multiply these illustrations indefinitely, but I will limit myself to only one other example. Here is a metallic element called potassium, so light and combustible that it swims and burns on water. Burning in water may seem, at first sight, very paradoxical; but in studying chemistry we must be ready to give up old prejudices. Water is almost pure oxygen, containing in the same volume more than one hundred times as much of the fire-element as air, and all combustibles would burn in water were it not that the oxygen is imprisoned in the liquid by an immensely strong force. Potassium, however, has such intense chemical affinities that it will break through all bars and bolts in order to unite with oxygen, and it therefore burns thus brilliantly even in the midst of water. [*] The final result is a
Such, then, are some of the steps in the process of world-building. I do not mean to imply that we can reproduce all these substances in our laboratories, although even this is true in almost every case. My object is only to show what must have been in general the process of nature, and to make evident the fact that oxygen has been the chief world-builder.
But why call oxygen the world-builder more than the other elements? This diagram answers the question, and it illustrates one of the most
Evidently, then, so far as our knowledge extends, oxygen, silicon, and carbon, together with a few metals, have been the chief building-materials employed by the Great Architect, and oxygen has been, as it were, the universal cement by which the other elements have been joined together to form that grand and diversified whole we call our earth.
One more remark in regard to this subject, and I will close this chapter. It is probable that there was a time, anterior to the earliest geological records, when the elements were in a free state; when the oxygen now solidified was a gas, and when, at the appointed time, the union of the elements began. Then our earth was a bright, burning star, radiating heat and light into space. Indeed, if we accept the nebular hypothesis of Laplace, the earth was formerly a part of the sun, was thrown off by the centrifugal force from his
For every aeriform substance there is a fixed temperature above which the gas cannot be reduced to a liquid by any pressure, however great; but below which this change can be produced if the mechanical force is sufficient. This fixed temperature is called "the critical point,'' and the pressure required to condense a gas becomes less and less as the temperature is reduced below this point, which differs very greatly with different substances. The critical point of many of the known gases is above the ordinary temperature of the air and all such gases may be reduced to liquids simply by mechanical pressure. The critical point of carbonic dioxide gas is about 88°, and as this temperature is within the limits of the variations in our climate, carbonic dioxide furnishes the most convenient illustration of the principle we are discussing. For example, in some specimens of granite rock we find cavities which are filled with liquidcarbonic dioxide if the temperature is below 87°—as can readily be seen by examining with a microscope the thin sections prepared for this purpose —but when the temperature rises above 87° the liquid at once disappears, to condense again, however, as soon as the temperature falls. The critical points of oxygen and nitrogen are not exactly known, but must be more than 150° below the zero of Fahrenheit, and hence chemists did not succeed in condensing these gases to liquids until they submitted them to extreme cold as well as to great pressure.
CHAPTER III. TESTIMONY OF OXYGEN. Religion and Chemistry | ||