RESEARCH II.
INTO THE COMBINATIONS OF NITROUS OXIDE,AND ITS DECOMPOSITION BYCOMBUSTIBLE BODIES.
EXPERIMENTS and OBSERVATIONS on the COMBINATIONS of NITROUS OXIDE.
I.Combination of Water with Nitrous Oxide.
a.The discoverer of nitrous oxide first observed its solubility in water; and it has since been noticed by different experimentalists.
Dr. Priestley found that water dissolved about one half of its bulk of nitrous oxide, and that at the temperature of ebullition, this substance was incapable of remaining in combination with it.[153]
b.I introduced to 9 cubic inches of pure water, i. e. water distilled under mercury, 7 cubic inches of nitrous oxide, which had been obtained over mercury, from the decomposition of nitrate of ammoniac, and in consequence was perfectly pure. After they had remained together for 11 hours, temperature being 46°, during which time they were frequently agitated, the gas remaining was 2,3; consequently 4,7 cubic inches had been absorbed. And then, 100 cubic inches, = 25300 grains of water, will absorb 54 cubic inches, = 27 grains, of nitrous oxide.
c.The taste of water impregnated with nitrous oxide, is distinctly sweetish; it is softer than common water, and, in my opinion, much more agreeable to the palate. It produces no alteration in vegetable blues, and effects no change of color in metallic solutions.
d.Thinking that water impregnated with nitrous oxide might probably produce some effects when taken into the stomach, by givingout its gas, I drank, in June, 1799, about 3 ounces of it, but without perceiving any effects.
A few days ago, considering this quantity as inadequate, I took at two draughts nearly a pint, fully saturated; and at this time Mr. Joseph Priestley drank the same quantity.
We neither of us perceived any remarkable effects.
Since that time I have drank near three pints of it in the course of a day. In this instance it appeared to act as a diuretic, and I imagined that it expedited digestion. As a matter of taste, I should always prefer it to common water.
e.Two cubic inches of pure water, that had been made to absorb about 1,1 cubic inches of nitrous oxide; when kept for some time in ebullition, and then rapidly cooled, produced nearly 1 of gas. Sulphur burnt in this gas with a vivid rose-colored flame.
In another experiment, in which the gas was expelled by heat from impregnated water, and absorbed again after much agitation on cooling;the residuum was hardly perceptible, and most likely depended upon some gas which had adhered to the mercury, and was liberated during the ebullition. Hence it appears that nitrous oxide is expelled unaltered from its aqueous solution by heat.
f.I have before mentioned,Division III, that nitrous oxide, during its combination with spring water, expels the common air dissolved in it. This common air generally amounts to one sixteenth, the volume of the water being unity. A correction on account of this circumstance must be made for the apparent deficiency of diminution, and for the common air mingled in consequence, with nitrous oxide during its absorption by common water.
g.Water impregnated with nitrous gas absorbed nitrous oxide; but the residual gas was much greater than that of common water, and gave red fumes with atmospheric air. Nitrous gas agitated for a long while over water highly impregnated with nitrous oxide, was not in the slightest degree diminished, in one experiment indeed it was ratherincreased; doubtless from the liberation of some nitrous oxide from the water by the agitation.
h.Nitrous oxide kept in contact with aqueous solution of sulphurated hydrogene and often agitated, was not in the slightest degree diminished.
Sulphurated hydrogene, introduced into a solution of nitrous oxide, was rapidly absorbed, and as the process advanced, the nitrous oxide was given out.
i.Water impregnated with carbonic acid, possessed no action upon nitrous oxide, and did not in the slightest degree absorb it. When carbonic acid was introduced to an aqueous solution of nitrous oxide; the aëriform acid was absorbed, and the nitrous oxide liberated.
k.From these observations it appears that nitrous oxide has less affinity for water, than even the weaker acids, sulphurated hydrogene and carbonic acid; as indeed one might have conjectured a priori from its degree of solubility: likewise that it has a stronger attraction for water than the gases not possessed of acid or alkalineproperties; it expelling from water nitrous gas, oxygene, and common air; probably hydrocarbonate, hydrogene, and nitrogene.
II.Combinations of Nitrous Oxide withFluid Inflammable Bodies.
a.Vitriolic ether absorbs nitrous oxide in much larger quantities than water.
A cubic inch of ether, at temperature 52°, combined with a cubic inch and seven tenths of nitrous oxide.
Ether thus impregnated was not at all altered in its appearance; its smell was precisely the same, but the taste appeared less pungent, and more agreeable. Nitrous oxide is liberated unaltered from ether at a very low temperature, that is, at about the boiling point of this fluid.
For expelling nitrous oxide from impregnated ether, and for ascertaining in general the quantity of gases combined with fluids, I have lately made use of a very simple method, which it may not be amiss to describe.
The impregnated fluid is introduced into a small thin tube, graduated to,05 cubic inches, through mercury. The quantity of fluid should never equal more than a fifth or sixth of the capacity of the tube.
The lower part of the tube is adapted to an orifice in the shelf of the mercurial apparatus, so as to make an angle of about 40° with the surface of the mercury.
The flame of a small spirit lamp is then applied to that part of the tube containing the fluid; and after the expulsion of the gas from it, the heat is raised so as to drive out the fluid through the orifice of the tube. Thus the liberated gas is preserved in a state proper for accurate examination.
Impregnated ether, during its combination with water, gives out the greater part of its nitrous oxide. During the liberation of nitrous oxide from ether, by its combination with water, a very curious phænomenon takes place.
If the water employed is colored, so that it may be seen in a stratumdistinct from the impregnated ether, at the point of contact a number of small spherules of fluid will be perceived, apparently repulsive both to water and ether; these spherules become gradually covered with minute globules of gas, and as this gas is liberated from their surfaces, they gradually disappear.
b.Alcohol dissolves considerable quantities of nitrous oxide.
2 cubic inches of alcohol, at 52°, combined with 2,4 cubic inches of nitrous oxide. The alcohol thus impregnated had a taste rather sweeter than before, but in other physical properties was not perceptibly altered.
Nitrous oxide is incapable of remaining in combination with this fluid at the temperature of ebullition; it is liberated from it unaltered by heat.
Impregnated alcohol, during its combination with water, gives out the greater part of its combined nitrous oxide: on mingling the two fluids together, at the point of contact the alcohol becomes covered with an infinite number of small globules of gas, which continue to be generatedduring the whole of the combination, and in passing through the fluid render it almost opaque.
c.The essential oils absorb nitrous oxide to a greater extent than either alcohol or ether.
,5 cubic inches of oil of carui combined with 1,2 cubic inches of nitrous oxide at 51°. The color of the oil thus impregnated was rather paler than before.
Nitrous oxide is expelled unaltered from impregnated oil of carui, by heat.
1 of oil of turpentine absorbed nearly 2 of nitrous oxide, at 57°. Its properties were not sensibly altered from this combination, and the gas was expelled from it undecompounded, by heat.
d.As well as the essential oils, the fixed oils dissolve nitrous oxide at low temperatures, whilst at high temperatures they do not remain in combination.
1 of olive oil absorbed, at 61°, 1,2 of nitrous oxide, but without undergoing any apparent physical change.
III.Action of Fluid Acids on Nitrous Oxide.
a.Nitrous oxide exposed to concentrated sulphuric acid, undergoes no change, and suffers no diminution, that may not be accounted for from the abstraction of a portion of its water by the acid.
b.Nitrous oxide is scarcely at all soluble in nitrous acid, and exposed to that substance, undergoes no alteration.
c.Muriatic acid, of specific gravity 1,14 absorbs about a third of its bulk of nitrous oxide. It suffers no apparent change in its properties from being thus impregnated, and the gas is again given out from it on the application of heat.
d.Acetic acid absorbs nearly one third of its bulk of nitrous oxide.
e.Aqua regia, that is, the nitro-muriatic acid, absorbs a very minute portion of nitrous oxide.
f.Nitrous oxide was exposed to a new compound acid, consisting of oxygenated muriatic acid, and sulphuric acid, which I discovered inJuly, 1799, and of which an account will be shortly published; but it was neither absorbed or altered.
I have before mentioned that the aqueous solutions of sulphurated hydrogene and carbonic acid, neither dissolve or alter nitrous oxide.
IV.Action of Saline Solutions, and other Substances,on Nitrous Oxide.
a.Nitrous oxide exposed to concentrated solution of green sulphate of iron, at 58°, underwent no perceptible diminution; not even after it had been suffered to remain in contact with it for half an hour.
b.It underwent diminution of nearly,2 when agitated in contact with a solution of red sulphate of iron, the volume of the solution being unity.
c.Solution of green sulphate of iron, fully impregnated with nitrous gas, did not in the slightest degree absorb nitrous oxide, and appeared to have no action upon it.
d.Solution of green muriate of iron, whether impregnated with nitrous gas, or unimpregnated, has no affinity for, or action upon, nitrous oxide.
e.Solution of red muriate of iron in alcohol, absorbed nearly one fifth of its bulk, of nitrous oxide.
f.Solution of prussiate of potash absorbed nearly one third of its volume, of nitrous oxide, which was again expelled from it by heat.
g.Solution of nitrate of copper appeared to have no affinity for nitrous oxide.
h.Concentrated solution of nitrate of ammoniac, at 58°, absorbed one eighth of its bulk of nitrous oxide.
i.Solutions of alkaline sulphures absorb nitrous oxide in quantities proportionable to the water they contain; it is expelled from them unaltered by heat. None of the hydro-sulphures dissolve more than half their bulk of nitrous oxide.
k.Concentrated solutions of the sulphites possess little or noaction on nitrous oxide; diluted solutions absorb it in small quantities.
l.Concentrated solution of muriate of tin absorbs about one eighth of nitrous oxide; more dilute solutions absorb larger quantities.
From these observations we learn, that neutro-saline solutions in general, have very feeble attractions for nitrous oxide; and as solutions of green muriate, and sulphate of iron, whether free from nitrous gas, or impregnated with it, possess no action upon nitrous oxide, nitrous gas may be separated from this substance by those solutions with greater facility than nitrous oxide can be separated from nitrous gas, by water or alcohol.
Charcoal absorbs nitrous oxide as well as all other gases; and it is disengaged from it by heat.
I have as yet found no other solid body, not possessed of alkaline properties, capable of absorbing nitrous oxide in any state of existence.
The bodies possessing the strongest affinity for oxygene, the dry sulphites, muriate of tin, the common sulphures, white prussiate ofpotash, and green oxide of iron, do not in the slightest degree act on nitrous oxide at common temperatures.
V.Action of different Gases on Nitrous Oxide.
a.12 measures of muriatic acid gas were mingled with 7 measures of nitrous oxide at 56°. After remaining together for a minute, they filled a space equal to 19½ measures. When water was introduced to them, the muriatic acid was absorbed much more slowly than if it had been unmingled.
In another experiment, when the gases were saturated with water, 9 measures of each of them, when mingled and suffered to remain in contact for a quarter of an hour, filled a space nearly equal to 19; and after the muriatic acid had been absorbed by potash, the nitrous oxide remained unaltered in its properties.
From the expansion, it appears most probable that aëriform muriatic acid, and nitrous oxide, have a certain affinity for each other, andthat they combine when mingled together; for in the last experiment, the increase of volume cannot be accounted for by supposing that nitrous oxide undergoes less change of volume than muriatic acid, by aëriform combination with water, and that the expansion depended upon the solution of some of its combined water by the muriatic acid. That muriatic acid and nitrous oxide have a slight affinity for each other, likewise appears from the absorption of nitrous oxide by aqueous solution of muriatic acid.
Thinking that nitrous oxide might attract muriatic acid from its solution in water, I exposed a minute quantity of fluid muriatic acid to nitrous oxide; but no alteration of volume took place in the gas.
b.6 measures of nitrous oxide were mingled with 11 measures of sulphureous acid, saturated with water; after remaining at rest for six minutes, they filled a space nearly equal to 18 measures. Exposed to water, the sulphureous acid was absorbed, but not nearly so rapidly aswhen in a free state. Sulphur burnt with a vivid flame in the residual nitrous oxide. 7 measures of sulphureous acid were now mingled with 8 of nitrous oxide. They filled a space nearly equal to 15¾, and no farther expansion took place afterwards.
From these experiments it appears probable that sulphureous acid, and nitrous oxide, have some affinity for each other.
c.11 measures of carbonic acid were mingled with 8 of nitrous oxide; they filled a space nearly equal to 19 measures. On exposing the mixture to caustic potash, the carbonic acid was absorbed, and the nitrous oxide remained pure. Hence it appears that carbonic acid and nitrous oxide do not combine with each other.
d.Oxygenated muriatic acid, and nitrous oxide, were mingled in a water apparatus: there was a slight appearance of condensation; but this was most probably owing to absorption by the water; on agitation, the oxygenated muriatic acid was absorbed, and the greater part of the nitrous oxide remained unaltered.
e.Sulphurated hydrogene and nitrous oxide, mingled together, neither expanded or contracted; exposed to solution of potash, the acid[154]only was absorbed.
f.10 measures of nitrous gas were admitted to 12 of nitrous oxide at 59°. They filled a space equal to 22, and after remaining together for an hour, had undergone no change. Solution of muriate of iron absorbed the nitrous gas without affecting the nitrous oxide.
g.Nitrous oxide was successively mingled with oxygene, atmospheric air, hydrocarbonate, phosphorated hydrogene, hydrogene, and nitrogene, at 57°; it appeared to possess no action on any of them, and was separated by water, the gases remaining unaltered.
h.As nitrous oxide was soluble in ether, alcohol, and the other inflammable fluids, it was reasonable to suppose that its affinity forthose bodies would enable them to unite with it in the aëriform state. At the suggestion of Dr. Beddoes I made the following experiment:
To 12 measures of nitrous oxide, at 54°, I introduced a single drop of ether; the gas immediately began to expand, and in four minutes filled a space equal to sixteen measures and a quarter. When an inflamed taper was plunged into the gas thus holding ether in solution, a light blue flame slowly passed through it.
A considerable diminution of temperature is most probably produced, from the great expansion of nitrous oxide during its combination with ether.
A drop of alcohol was admitted to 14 measures of nitrous oxide. In five minutes, the gas filled a space equal to fifteen and a third; but no farther diminution took place afterwards.
A minute quantity of oil of turpentine was introduced to 14 measures of nitrous oxide; it filled, in 4 minutes, a space rather less than 14; and no farther change took place afterwards. Most likely this contraction arose from the precipitation of the water dissolved in thegas by the stronger affinity of the oil for nitrous oxide. To ascertain with certainty if any oil had been dissolved by the gas, I introduced into it a small quantity of ammoniac. It immediately became slightly clouded, most probably from the formation of soap, by the combination of the dissolved oil with the ammoniac.
From these experiments we learn, that when nitrous oxide is mingled with either carbonic acid, oxygene, common air, hydrocarbonate, sulphurated hydrogene, hydrogene, or nitrogene, they may be separated from each other without making any allowance for contraction or expansion; but if a mixture of either muriatic acid, or sulphureous acid gas, with nitrous oxide, is experimented upon; in the absorption of the acid by alkalies, the apparent volume of gas condensed will be less than the real one, by a quantity equal to the sum of expansion from combination. Consequently a correction must be made on account of this circumstance.
Though alcohol, ether, essential oils, and the fluid inflammablebodies in general, dissolve nitrous oxide with much greater rapidity than water, yet as we are not perfectly acquainted with their action on unabsorbable gases, it is better to employ water for separating nitrous oxide from these substances; particularly as that fluid is more or less combined with all gases, and as we are acquainted with the extent of its action upon them.
By pursuing the subject of the solution of essential oils in gases, we may probably discover a mode of obtaining them in a state of absolute dryness. For if other gases as well as nitrous oxide, have a stronger affinity for oils than for water, water most probably will be precipitated from them during their solution of oils; and after their saturation with oil, it is likely that they are capable of being deprived of that substance by ammoniac.
VI.Action of aëriform Nitrous Oxide in the Alkalies.History of the discovery of the combinationsof Nitrous Oxide with the Alkalies.
a.When nitrous oxide in a free state is exposed to the solid caustic alkalies and alkaline earths, at common temperatures, it is neither absorbed nor acted upon; when it is placed in contact with solutions of them in water, a small quantity is dissolved; but this combination appears to depend on the water of the solution, for the gas can be expelled unaltered, at the temperature of ebullition.
b.Caustic potash was exposed to nitrous oxide for 13 hours: the diminution was not to one fiftieth, and this slight condensation most probably depended upon its combination with the water of the gas.
Concentrated solution of potash absorbed a fourth of its bulk of nitrous oxide. When the impregnated solution was heated, globules of gas were given out from it rapidly; but the quantity collected was too small to examine.
Soda, whether solid or in solution, exhibited exactly the same phænomena with nitrous oxide. The solution of soda absorbed near a quarter of its bulk of gas.
c.11 measures of ammoniacal gas were mingled with 8 measures of nitrous oxide over dry mercury, both of the gases being saturated with water. No change of appearance was produced by the mixture, and they filled, after two minutes, a space equal to 19. On the introduction of a little water, the ammoniac was absorbed, and the nitrous oxide remained unaltered, for it was dissolved by water as rapidly as if it had never been mingled with ammoniac.[155]
7 measures of nitrous oxide, exposed to 6 measures of solution of ammoniac in water, was in an hour diminished to 4½ nearly. When the solution was heated over mercury, permanent gas was produced, which was unabsorbable by a minute quantity of water, and soluble in a large quantity; consequently it was nitrous oxide.
d.Nitrous oxide was exposed to dry caustic strontian; it underwent a diminution of nearly one fortieth, which most likely was owing to the combination of the strontian with its water.
11 measures of nitrous oxide were agitated in contact with 8 of strontian lime water: nearly 4 measures were absorbed. The impregnated solution exposed to heat, rapidly gave out its gas; 3 measures were soon collected, which mingled with a small quantity of hydrogene, and inflamed by the taper, gave a smart detonation.
e.Nitrous oxide exposed to lime and argil, both wet and dry, was not in the slightest degree acted upon.
From these experiments it is evident that nitrous oxide in the aëriform state cannot be combined either with the alkalies, or the alkaline earths. That a combination may be effected between nitrous oxide and these substances, it must be presented to them, in thenascent state.
The salts composed of the alkalies and nitrous oxide, are notanalogous to any other compound substances, being possessed of very singular properties. Before these properties are detailed, it may not be amiss to give an account of the accidental way in which I discovered the mode of combination.
In December, 1799, designing to make a very delicate experiment, with a view to ascertain if any water was decomposed during the conversion of nitrous gas into nitrous oxide, by sulphite of potash, I exposed 200 grains of crystalised sulphite of potash, containing great superabundance of alkali, to 14 cubic inches of nitrous gas, containing one eighteenth nitrogene. The alkali was employed to preserve any ammoniac that might be formed, in the free state, as it would otherwise combine with sulphureous acid.[156]
The volume of gas diminished with great rapidity; in two hours and tenminutes it was reduced to 6⁴/₅, which I considered as the limit of diminution. Accidentally, however, suffering it to remain for three hours longer, I was much surprised by finding that not quite 2 cubic inches remained, which consisted of nitrous oxide, mingled with the nitrogene that existed before the experiment.
In accounting theoretically for this phænomenon, different suppositions necessarily presented themselves.
1st, It was possible, that though sulphite of potash, and potash, separately possessed no action on free nitrous oxide, yet in combination they might exert such affinities upon it as either to absorb it, or make it enter into new combinations.
2dly. It was more probable that the caustic potash, though incapable of condensing aëriform nitrous oxide, was yet possessed of a strong affinity for it when in thenascent state, and that the nitrous oxide condensed in the experiment had been combined in this state with the free alkali.
To ascertain if the compound of potash and sulphite of potash with sulphate, was capable of acting upon nitrous oxide, I suffered a quantity of this substance to remain in contact with the gas for near a day: no change whatever took place.
To determine whether the diminution of nitrous oxide depended upon its absorption in the nascent state, by the peculiar compound of potash and sulphite of potash, or if it was simply owing to the alkali.
I mingled a solution of sulphite of potash with caustic soda; the salt, after being evaporated at a low temperature, was exposed to nitrous gas. The nitrous oxide formed was absorbed, but in rather less quantities than when alkaline sulphite of potash was employed.
Hence it was evident that the alkali was the agent that had condensed the nitrous oxide in those experiments, for soda is incapable of combining either with sulphate, or sulphite of potash.
To ascertain whether any change in the constitution of the nitrousoxide had been produced by the condensation, I introduced a small quantity of sulphite of potash, with excess of alkali, that had absorbed nitrous oxide, into a long and thin cylindrical tube filled with mercury; and inclining it at an angle of 35° with the plane of the mercury, applied the heat of a spirit lamp to that part of the tube containing the salts; when the glass became very hot, gas was given out with rapidity; in less than a minute the tube was full. This gas was transfered into another tube, and examined; it proved to be nitrous oxide in its highest state of purity;[157]for a portion of it absorbed by common water, left no more than a residuum of ¹/₁₅, and sulphur burnt in it with a vivid rose-colored flame.
Being now satisfied that the alkalies were capable of combining with nitrous oxide; to investigate with precision the nature of these new compounds, I proceeded in the following manner.
VII.Combination of Nitrous Oxide with Potash.
a.Into a solution of sulphite of potash, which had been made by passing sulphureous acid gas from a mercurial airholder into caustic potash dissolved in water, I introduced 17 grains of dry potash. The whole evaporated at a low temperature, gave 143 grains of salt. This salt was notwhollycomposed of sulphite of potash and potash; it contained as well, a minute quantity of carbonate, and sulphate of potash, formed during the evaporation.[158]
120 grains of it finely pulverised, and retaining the water of crystalisation, were exposed to 15 cubic inches of nitrous gas, over mercury. The nitrous gas diminished with great rapidity, and in threehours a cubic inch and nine tenths only remained, which consisted of nearly one third nitrous oxide, and two thirds nitrogene that had pre-existed in the nitrous gas. The increase of weight of the salt could not be determined, as some of it was lost by adhering to the vessel in which the combination was effected, and to the mercury. It presented no distinct series of crystalisations, even when examined by the magnifier; rendered green vegetable blues, and its taste was very different from that of the remaining quantity of salt that had been exposed to the atmosphere. A portion of it strongly heated over mercury, gave out gas with great rapidity, which had all the properties of the purest nitrous oxide.
When water was poured upon some of it, no gas was given out, and the whole was equably and gradually dissolved. Alcohol, as well as ether, appeared incapable of dissolving any part of it.
When muriatic acid was introduced into it, confined by mercury, a rapid effervescence took place. Part of the gas disengaged wassulphureous acid, and carbonic acid; the remainder was nitrous oxide.
b.I made a number of experiments upon salts procured in the manner I have just described, with a view to obtain the compound of nitrous oxide and potash, free from admixture of other salts.
When the mixed salt was boiled in alcohol or ether, no part of it appeared to be dissolved. Finding that little or no gas was given out during the ebullition of concentrated solutions of the mixed salts, I attempted to separate the sulphate, sulphite, and carbonate of potash, from the combination of nitrous oxide and potash, by successive evaporations and crystalisations. But though in this way it was nearly freed from sulphate of potash, yet the extreme and nearly equal solubility of the other salts, prevented me from completely separating them from each other.
By exposing, however, very finely pulverised sulphite of potash, mingled with alkali, for a great length of time to nitrous gas, it wasalmost wholly converted into sulphate; and after the separation of this solution, evaporation, and crystalisation, at a low temperature, I obtained the new combination, mingled with very little carbonate of potash, and still less of sulphite.
The minute quantity of sulphite chiefly appeared in very small crystals; distinct from the mass of salt, which possessed no regular crystalisation, and was almost wholly composed of the new compound, intimated mingled with a little carbonate. The new compound, as nearly as I could estimate from the quantity of nitrous oxide absorbed, consisted of about 3 alkali, to 1 of nitrous oxide, by weight.
It exhibited the following properties:
1. Its taste was caustic, and possessed of a pungency different from either potash or carbonate of potash.2. It rendered vegetable blues green, which might possibly depend upon the carbonate of potash mixed with it.3. Pulverised charcoal mingled with a few grains of it, and inflamed,burnt with flight scintillations. Projected into zinc in a state of fusion, a slight inflammation was produced.4. When either sulphuric, muriatic, or nitric acid was introduced to it under mercury, it gave out nitrous oxide, mingled with a little carbonic acid.5. Thrown into a solution of sulphurated hydrogene, gas was disengaged from it, but in quantities too minute to be examined.6. When carbonic acid was thrown into a solution of it in water, gas was disengaged; on examination it proved to be nitrous oxide.7. A concentrated solution of it kept in ebullition in a cylinder, confined by mercury, gave out a few globules of gas, which were too minute to be examined, and probably consisted of common air previously contained in the water.
1. Its taste was caustic, and possessed of a pungency different from either potash or carbonate of potash.
2. It rendered vegetable blues green, which might possibly depend upon the carbonate of potash mixed with it.
3. Pulverised charcoal mingled with a few grains of it, and inflamed,burnt with flight scintillations. Projected into zinc in a state of fusion, a slight inflammation was produced.
4. When either sulphuric, muriatic, or nitric acid was introduced to it under mercury, it gave out nitrous oxide, mingled with a little carbonic acid.
5. Thrown into a solution of sulphurated hydrogene, gas was disengaged from it, but in quantities too minute to be examined.
6. When carbonic acid was thrown into a solution of it in water, gas was disengaged; on examination it proved to be nitrous oxide.
7. A concentrated solution of it kept in ebullition in a cylinder, confined by mercury, gave out a few globules of gas, which were too minute to be examined, and probably consisted of common air previously contained in the water.
c.In the experiments made to ascertain these properties all the salt was expended, otherwise I should have endeavoured to ascertain what quantity of gas would have been liberated by heat from a givenweight; and likewise what would have been the effects of admixture of it with oil. When some of the mixed salt was mingled with oil of turpentine, part of it was dissolved, and the fluid became white; but no gas was given out. On this coarse experiment, however, I cannot place much dependance. If the combination of nitrous oxide and potash is capable of combining with oil without decomposition, barytes and strontian[159]will probably separate the oil from it, and thus it may possibly be obtained in a state of purity.
In a rough experiment made on the conversion of nitrous gas into nitrous oxide, by concentrated solution of sulphite of potash with excess of alkali, very little of the nitrous oxide was absorbed. Hence it is probable that water lessens the affinity of potash for nascent nitrous oxide.
VIII.Combination of Nitrous Oxide with Soda.
The union of nitrous oxide with soda is effected in the same manner as with potash. The alkali, mingled by solution and evaporation, with either sulphite of soda, or of potash, is exposed to nitrous gas; the nitrous oxide is condensed by it at the moment of generation, and the combination effected.
As far as I have been able to observe, nitrous oxide is not absorbed to so great an extent by soda, as potash.
I have not yet been able to obtain the combination of nitrous oxide with soda in its pure state. To the attainment of this end, difficulties identical with those noticed in the last section present themselves. It is extremely difficult to procure the soda perfectly free from carbonic acid, and though by using sulphite of potash the sulphate formed is easily separated, yet still evaporation andcrystalisation will not disengage the sulphite and carbonate from the new compound.
The compound of soda and nitrous oxide, mingled with a little sulphite and carbonate of soda, was rapidly soluble, both in warm and cold water, without effervescence. Its solution, heated to ebullition, gave out no gas. The taste of the solid salt was caustic, and more acrid than that of the mixture of carbonate and sulphite of soda. When cast upon zinc in fusion, it burnt with a white flame. When heated to 400° or 500°, it gave out nitrous oxide with rapidity. Nitrous oxide was expelled from it by the sulphuric, muriatic, and carbonic acids,I believe, by sulphurated hydrogene.[160]
IX.Combination of Nitrous Oxide with Ammoniac.
I attempted to effect this combination by converting nitrous gas into nitrous oxide, by sulphite of ammoniac, wetted with strong solution of caustic ammoniac; but without success; for the whole of the nitrous oxide produced remained in a free state.
When I exposed sulphite of potash, mingled by solution and evaporation with highly alkaline carbonate of ammoniac,[161]to nitrous gas, the diminution was nearly one fourth more than if pure sulphite of potash had been employed. Hence it appears most likely that ammoniac is capable of combination with nitrous oxide in the nascent state.
In the experiments on the conversion of nitrous gas into nitrous oxide, by nascent hydrogene, and by sulphurated hydrogene,Res. I. Divis. V.probably the water formed at the same time with the ammoniac and nitrous oxide, prevented them from entering into combination;possiblythe peculiar compound was formed, but in quantities so minute as not to be distinguished from simple ammoniac;[162]for even the existence of ammoniac in these processes, is but barely perceptible.
If it should be proved by future experiments, that in the decomposition of nitrous gas by nascent hydrogene, a peculiar compound of nitrous oxide, water and ammoniac, is formed, it will afford proofs in favor of the doctrine of predisposing affinity;[163]for then this decomposition might be supposed to depend upon the disposition of oxygene, hydrogene and nitrogene to assume the states of combination in which they might form a triple compound, of water, nitrous oxide, and ammoniac.
Nitrous oxide might probably be made to combine with ammoniac by exposing a mixture of nitrous gas and aëriform ammoniac, to the sulphites.
It is probable that nitrous oxide may be combined with ammoniac, by means of double affinity. Perhaps sulphate of ammoniac and the combination of potash with nitrous oxide mingled together in solution, would be converted into sulphate of potash and the compound of nitrous oxide, and ammoniac.
X.Probability of forming Compounds of Nitrous Oxideand the Alkaline Earths.
I attempted to combine nitrous oxide with lime and strontian, by exposing sulphites of lime and strontian with excess of earth, to nitrous gas; but this process did not succeed: the diminution took place so slowly as to destroy all hopes of gaining any results in a definite time. Sulphite of potash is decomposable by barytes, strontian, and lime;[164]consequently it was impossible to employ this substance to effect the combination.
As the dry sulphures, when well made, convert nitrous gas into nitrous oxide, it is probable that the union of the earths with nascent nitrous oxide may be effected by exposing nitrous gas to their sulphures, containing an excess of earth.
Perhaps the combination of nitrous oxide with strontian may be effected by introducing the combination of potash and nitrous oxide into strontian lime water.
It is probable that nitrous oxide may be combined with clay and magnesia, by exposing these bodies, mingled with sulphite of potash or soda, to nitrous gas.
XI.Additional Observations on the combinationsof Nitrous Oxide with the Alkalies.
A desire to complete physiological investigations relating to nitrous oxide, has hitherto prevented me from pursuing to a greater extent, the experiments on the combination of this substance with the alkalies, &c. As soon as an opportunity occurs, I purpose to resume the subject.
The observations detailed in the foregoing sections are sufficient to show that nitrous oxide is capable of entering into intimate union with the fixed alkalies: and as the compounds formed by this union areinsoluble in alcohol, decomposable by the acids, and heat, and possessed of peculiar properties, they ought to be considered as a new class of saline substances.
If it is thought proper, on a farther investigation of their properties, to signify them by specific names, they may, according to the usually adopted fashion of nomenclature, be callednitroxis: thus thenitroxi of potashwould signify the salt formed by the combination of nitrous oxide with potash.
Future experiments must determine the different affinities of nitrous oxide for the alkalies, and alkaline earths.
With regard to the uses of these new compounds it is difficult to form a guess. When they are obtained pure, and fully saturated with nitrous oxide, on account of the low temperature at which their gas is liberated, they will probably constitute detonating compounds. From their facility of decomposition by the weaker acids, they may possibly be used medicinally, if ever the evolution of nitrous oxide in the stomach should be found beneficial in diseases.
XII.The properties of Nitrous Oxide resemble those of Acids.
If we were inclined to generalise, and to place nitrous oxide among a known class of bodies, its properties would certainly induce us to consider it as more analogous to the acids than to any other substances; for it is capable of uniting with water and the alkalies, and is insoluble in most of the acids. It differs, however, from the stronger acids, in not possessing the sour taste,[165]and the power of reddening vegetable blues: and from both the stronger and weaker acids, in not being combinable when in a perfectly freestate, at common temperatures, with the alkalies. If it should be proved by future experiments, that condensation by cold gave it the capability of immediately forming neutro-saline compounds with the alkalies; it ought to be considered as the weakest of the acids. Till those experiments are made, its extraordinary chemical and physiological properties are sufficient to induce us to consider it as a bodysui generis.
It is a singular fact that nitrous gas, which contains in its composition a quantity of oxygene so much greater than nitrous oxide, should nevertheless possess no acid properties. It is uncombinable with alkalies, very little soluble in water, and absorbable by the acids.
On the DECOMPOSITION of NITROUS OXIDE by COMBUSTIBLE BODIES. Its ANALYSIS. OBSERVATIONS on the different combinations of OXYGENE and NITROGENE.
I.Preliminaries.
Fromthe phænomena mentioned inRes. I. Divis. III.[166]it appears that the combustible bodies burn in nitrous oxide at certain temperatures. The experiments in this Division were instituted for the purpose of investigating the precise nature of these combustions, with a view of ascertaining exactly the composition of nitrous oxide.
It will be seen hereafter that very high temperatures are required forthe decomposition of nitrous oxide, by most of the combustible bodies, and that in this process heat and light are produced to a very great extent. These agents alone are possessed of a considerable power of action on nitrous oxide; of which it is necessary to give an account, that we may be able to understand the phænomena in the following sections.
II.Conversion of Nitrous Oxide into Nitrous Acid,and a Gas analogous to Atmospheric Air, by Ignition.
a.Dr. Priestley asserts, that nitrous oxide exposed for a certain time to the action of the electric spark, is rendered immiscible with water, and capable of diminution with nitrous gas, without suffering any alteration of volume; and likewise that the same changes are effected in it by exposure to ignited incombustible bodies.[167]
The Dutch chemists state, that the electric spark passed through nitrous oxide, occasions a small diminution of its volume, and that the gas remaining is analogous to common air.[168]They conclude that this change depends on the separation of its constituent parts, oxygene and nitrogene, from each other.
None of these chemists have suspected the production of nitrous acid in this process.
b.Nitrous oxide undergoes no change whatever from the simple action of light. I exposed some of it, confined by mercury, for many days to this agent, often passing through it concentrated rays by means of a small lens. When examined it appeared, as well as I could estimate, of the same degree of purity as at the beginning of the experiment.
c.A temperature below that of ignition effects no alteration in the constitution of nitrous oxide. I passed nitrous oxide from a retortcontaining decomposing nitrate of ammoniac, through a green glass tube, strongly heated in an air-furnace, but not suffered to undergo ignition. The gas, received in a water apparatus exhibited the same properties as the purest nitrous oxide; some of it absorbed by water, left a residuum of not quite one thirteenth.
d.The action of the electric spark for a long while continued, converts nitrous oxide into a gas analogous to atmospheric air, and nitrous acid.
I passed about 150 strong shocks from a small Leyden phial, through 7 ten grain measures of pure nitrous oxide. After this it filled a space rather less than six measures: the mercury was rendered white on the top, as if it had been acted on by nitric acid. Six measures of nitrous gas mingled with the residual gas of the experiment, over mercury covered by a little water, gave red fumes, and rapid diminution. In five minutes the volume of the gases nearly equalled ten. Thermometer in this experiment was 58°.
Electric sparks were passed for an hour and half through 7 ten grain measures of nitrous oxide over mercury covered with a little red cabbage juice, previously saturated with nitrous oxide, and rendered green by an alkali. After the process the gas filled a space equal to rather more than six measures and half, and the juice was become of a pale red. The gas was introduced into a small tube filled with pure water, and agitated; no absorption was perceptible: 7 measures of nitrous gas added to it gave red fumes, and after six minutes a diminution to 9¼ nearly. 6½ measures of common air from the garden, with 7 of nitrous gas, gave exactly 9.
In this experiment it was evident that nitrous oxide was converted into a gas analogous to atmospheric air, at the same time that an acid was formed. There could be little doubt but that this was the nitrous acid. To ascertain it, however, with greater certainty, the electric spark was passed through 6 measures of nitrous oxide, over a littlesolution of green sulphate of iron, confined by mercury. As the process went on, the color of the solution became rather darker. When the diminution was complete, a little prussiate of iron was added to the solution. A precipitate of pale blue prussiate of potash was produced.
c.Nitrous oxide was passed from decomposing nitrate of ammoniac, through a porcelain tube well glazed inside and outside, strongly ignited in an air-furnace, and communicating with the water apparatus. The gas collected was rendered opaque by dense red vapor. It appeared wholly unabsorbable by water. After the precipitation of its vapor, a candle burnt in it with nearly the same brilliancy as in atmospheric air. 20 measures of it that had been agitated in water immediately after its production, mingled with 40 measures of nitrous gas, diminished to about 47.5; whereas 20 measures that had remained unagitated for some time after their generation, introduced to the same quantity of nitrous gas, gave nearly 49. 20 measures of atmospheric air, with 40 of the same nitrous gas, were condensed to 46.
The water with which the gas had been in contact, was strongly acid. A little of it poured into a solution of green sulphate of iron, and then mingled with prussian alkali, produced a green precipitate. Hence the acid it contained was evidently nitrous.
That no source of error could have existed in this experiment from fissure in the tube, I proved, by sending water through it whilst ignited, after the process, from the same retort in which the nitrate of ammoniac had been decomposed; a few globules of air only were produced, not equal to one tenth of the volume of the water boiled, and which were doubtless previously contained in it.
I have repeated this experiment two or three times, with similar results; whenever the air was agitated in water immediately after its production, it gavealmostthe same diminution with nitrous gas as common air; when, on the contrary, it has been suffered to remain for some time in contact with the phlogisticated nitrous acid suspendedin it, the condensation has been less with nitrous gas by five or six hundred parts. Hence I am inclined to believe, that if it were possible to condense all the nitrous acid formed, immediately after its generation, so as to prevent it from absorbing oxygene from the permanent gas, this gas would be found identical with the air of the atmosphere.
The changes effected by fire on nitrous oxide are not analogous to those produced by it in other bodies; for the power of this agent seems generallyuniform, either in wholly separating the constituent principles of bodies from each other, or in making them enter into more intimate union.[169]
It is a singular phænomenon, that whilst it condenses one part of the oxygene and nitrogene of nitrous oxide, in the form of nitrous acid; itshould cause the remainder to expand, in the state of atmospheric air. Does not this fact afford an inference in favor of thechemicalcomposition of atmospheric air?
III.Decomposition of Nitrous Oxide by Hydrogene,at the temperature of Ignition.
In the following experiments on the decomposition of nitrous oxide by hydrogene, the gases were carefully generated in the mercurial apparatus, and their purity ascertained by the tests mentioned inResearch I. They were measured in small tubes graduated to grains, and then transferred into the detonating tube, which was eight tenths of an inch in diameter, and graduated to ten grain measures.
The space occupied by the gases being noted after the inflammation by the electric shock, green muriate of iron, and prussiate of potash, were successively introduced, to ascertain if any nitrous acid had been formed. The absorption, if any took place, was marked, and the gasestransferred into a narrow grain measure tube, and their bulk and composition accurately ascertained.
b.The hydrogene employed was procured from water by means of zinc and sulphuric acid. 50 grain measures of it fired by the electric spark, with 30 grain measures of oxygene containing one eleventh nitrogene, gave a residuum of about 4. Nitrous gas mingled with those 4, indicated the presence of rather less than 1 of unconsumed oxygene. In another experiment 23 of it, with 20 of the same oxygene left rather more than 6 residuum.
The nitrous oxide was apparently pure, for it left a remainder of about ,05 only, when absorbed by common water.
c.30 of hydrogene were fired with 40 of nitrous oxide; the concussion was very great, and the light given out bright red; no perceptible quantity of nitrous acid was formed; the residual gas filled a space equal to 52. No part of it was absorbable by water, it gave no diminution with nitrous gas, when it was mingled with a littleoxygene, and again acted on by the electric spark, an inflammation and slight diminution was produced.
d.33 of hydrogene were fired with 35 of nitrous oxide: nitrous acid was produced in very minute quantity; the gas that remained was not absorbable by water, and filled a space equal to 37 grains. Nitrous gas mingled with these, underwent a very slight diminution.
e.46 hydrogene were fired with 46 nitrous oxide. The quantity of nitrous acid formed was just sufficient to tinge the white prussiate of potash. The gases filled a space equal to 49, gave no perceptible diminution with nitrous gas, and did not inflame with oxygene.
f.40 hydrogene were fired with 39 nitrous oxide; no perceptible quantity of nitrous acid was formed. The residual gas filled a space equal to 41; was unabsorbable by water, underwent no diminution when mingled with nitrous gas; or when acted on by the electric spark in contact with oxygene.
g.20 hydrogene were fired with 64 nitrous oxide; afterdetonation the expansion of the gases was greater in this experiment than any of the preceding ones; dense white fumes were observed in the cylinder, and a slow contraction of volume took place. After a little green muriate of iron had been admitted, the gases filled a space equal to 73: prussiate of potash mingled with the muriate, gave a deeper blue than in any of the preceding experiments. The residual gas was unabsorbable by water: 65 of it, mingled with 65 of nitrous gas, diminished to 93; whilst 65 of common air, with 65 of nitrous gas, gave 84.
h.8 of hydrogene were fired with 54 of nitrous oxide; the same phænomena as were observed in the last experiment took place; nitrous acid was formed; after the absorption of which the residual gas filled a space equal to 55. 50 of this, with an equal quantity of nitrous gas, diminished to 76. In these processes the temperatures were from 56° to 61°.
These experiments are selected as the most accurate of nearly fifty,made on the inflammation of different quantities of nitrous oxide and hydrogene.
As Mr. Keir found muriatic acid in the fluid, produced by the inflammation of oxygene and hydrogene in closed vessels, in Dr. Priestley’s experiments, I preserved the residual gas of about 3 cubic inches of nitrous oxide, that had been detonated at different times with less than a cubic inch and half of hydrogene; but solution of nitrate of silver was not clouded when agitated in this gas, nor when introduced into the detonating tube in which the inflammation had been made.
From these experiments we learn that nitrous oxide is decomposable at the heat of ignition, by hydrogene, in a variety of proportions.
When the quantity of hydrogene very little exceeds that of the nitrous oxide, both of the gates disappear, water is produced, no nitrous acid is formed, and the volume of nitrogene evolved is rather greater than that of the nitrous oxide decomposed.
When the quantity of hydrogene is less than that of the nitrous oxide, water, nitrous acid, oxygene and nitrogene, are generated in different proportions; one part of the nitrous oxide is most probably wholly decomposed by the hydrogene, and the other part converted into nitrous acid and atmospheric air, in consequence of the ignition.
From experimentsc,d, ande, the composition of nitrous oxide may be deduced. In experimentd, 39 of nitrous oxide were decomposed by 40 of hydrogene, and converted into 41 of nitrogene.
Now frombit appears that 40 of hydrogene require for their condensation about 20.8 of oxygene in volume; so that founding the estimation upon the quantity of hydrogene consumed, 100 parts of nitrous oxide would consist nearly of 63.1 of nitrogene, and 36.9 of oxygene. But 41 of nitrogene weigh 12.4,Res. I. Div. I. Consequently, deducing the composition of nitrous oxide from the quantity of nitrogene evolved, 100 parts of it would consist of 63.5 nitrogene, and 36.5 oxygene.
These estimations are very little different from those which may be deduced from the other experiments, and the coincidence is in favor of their accuracy.
From the following experiment it appears that the temperature required for the decomposition of nitrous oxide by hydrogene must be higher than that which is necessary to produce the inflammation of hydrogene with oxygene. I introduced into small tubes filled with equal parts of nitrous oxide and hydrogene, standing on a surface of mercury, iron wires ignited to different degrees, from the dull red to the vivid white heat. The gases were always inflamed by the white and vivid red heats; but never by the dull red heat, though the last uniformly inflamed mixtures of oxygene and hydrogene, and atmospheric air and hydrogene.
Dr. Priestley[170]first detonated together nitrous oxide and hydrogene; his experiment wasrepeated by the Dutch chemists, who found that when a small quantity of hydrogene was employed, the nitrous oxide was partially converted into a gas analogous to common air. Their estimation of its composition, which is not far removed from the truth, was founded on this phænomenon.[171]
IV.Decomposition of Nitrous Oxide by Phosphorus.
a.Phosphorus introduced into pure nitrous oxide at common temperatures, is not at all luminous. It is capable of being fused, and even sublimed in it, without undergoing acidification, and without effecting any alteration in its composition.
About 2 grains of phosphorus were fused, and gradually sublimed, in 2 cubic inches of pure nitrous oxide, over mercury, by the heat of aburning lens. No alteration was produced in the volume of gas, and a portion of it absorbed by water, left a residuum of one twelfth only.
Phosphorus was sublimed in pure nitrous oxide over mercury, in a dark room, by an iron heatednearlyto ignition; but no luminous appearance was perceptible, nor was any gas decomposed.
b.Phosphorus decomposes nitrous oxide at the temperature of ignition, with greater or less rapidity, according to the degree of heat. We have already seen, that when phosphorus in active inflammation is introduced into nitrous oxide, it burns with intensely vivid light.
Phosphorus was sublimed by a heated wire in a jar filled with nitrous oxide, standing over warm mercury. In this state of sublimation an iron heated dull red was introduced to it by being rapidly passed through the mercury; a light blue flame surrounded the wire, and disappeared as soon as it ceased to be red.
To phosphorus sublimed as before, in nitrous oxide, over warm mercury,a thick wire ignited to whiteness was introduced; a terrible detonation took place, and the jar was shattered in pieces.
By employing thick conical jars,[172]containing only a small quantity of nitrous oxide, I effected the detonation several times with safety; but on account of the great expansion of the elastic products, the jar was generally either raised from the mercury, or portions of gas were thrown out of it. Hence I was unable to ascertain the exact changes produced by this mode of decomposition.
c.As my first attempts to ascertain the constitution of nitrous oxide were made on its decomposition by phosphorus, I employed manydifferent modes of partially igniting this substance in it over mercury, so as to produce a combustion without explosion.
The first method adopted was inflammation by means of oxygenated muriate of potash. A small particle of oxygenated muriate of potash was inserted into the phosphorus to be burnt. On the application of a wire, moderately hot, to the point of insertion, the salt was decomposed by the phosphorus, and sufficient fire generated and partially applied by the slight explosion, to produce the combustion of the phosphorus, without the previous sublimation of any part of it.
The second way employed was the ignition of a part of the phosphorus, by means of the combustion of a small portion of tinder of cotton,[173]or paper, in contact with it, by the burning glass.
The third, and most successful mode, was by introducing into thegraduated jar containing the nitrous oxide, the phosphorus in a small tube containing oxygene, so balanced as to swim on the surface of the mercury, without communicating with the nitrous oxide. The phosphorus was fired in the oxygene with an ignited iron wire, by which at the moment of combustion, the tube containing it was raised into the nitrous oxide, and thus the inflammation continued.
d.In different experiments, made with accuracy, I found that the whole of a quantity of nitrous oxide was never decomposable by ignited phosphorus; the combustion always stopped when the nitrous oxide remaining was to the nitrogene evolved as about 1 to 5; likewise that the volume of nitrogene produced was rather less than that of the nitrous oxide decomposed, and that this deficiency arose from the formation of nitrous acid by the intense ignition produced during the process.
Of one experiment I shall give a detail.
Temperature being 48°, two cubic inches of pure nitrous oxide, whichhad been generated over mercury, were introduced into a jar of the capacity of 9 cubic inches, graduated to,1 cubic inches, and much enlarged at the base. A grain of phosphorus was inserted into a small vessel about one third of an inch long, and half an inch in diameter, containing about 15 grain measures of very pure oxygene; this vessel, which swam on the surface of the mercury, was carefully introduced into the jar containing the nitrous oxide. The phosphorus was fired by means of a heated wire, and before the oxygene was wholly consumed, the vessel containing it elevated into the nitrous oxide. The combustion was extremely vivid and rapid. After the atmospheric temperature was restored, the gas was rendered opaque by dense white vapor. When this had been precipitated, and the small vessel removed from the jar, the gas filled a space nearly equal to 1.9 cubic inches. On introducing to it a little solution of green muriate of iron, and prussiate of potash, green prussiate of iron was produced: hence, evidently, nitrous acid had been formed.
On the admission of pure water, an absorption of rather more than,3 took place.
The 16 measures remaining underwent no perceptible diminution with nitrous gas; the taper plunged into them was instantly extinguished.
To ascertain if the phosphoric acid produced in the experiments made under mercury did not in some measure prevent the decomposition of the whole of the nitrous oxide by the phosphorus, I introduced into a mixture of 5 nitrogene and 1 nitrous oxide, ignited phosphorus: but it was immediately extinguished.[174]
The Dutch Chemists found that phosphorus might be fused in nitrous oxide without being luminous. They assert that phosphorus in a state of inflammation, introduced into this gas, was immediately extinguished; though when taken out into the atmosphere, it again burnt of its own accord.[175]It is difficult to account for their mistake.
V.Decomposition of Nitrous Oxide byPhosphorated Hydrogene.
a.It has been mentioned inRes. II. Div. I. that phosphorated hydrogene and nitrous oxide posses no action on each other, at atmospheric temperatures.
Phosphorated hydrogene mingled with nitrous oxide, is capable of being inflamed by the electric spark, or by ignition.
b. E.1. 10 grain measures of phosphorated hydrogene, carefully produced by means of phosphorus and solution of caustic alkali, were mingled with 52 measures of nitrous oxide. The electric spark passed through them, produced a vivid inflammation. The elastic products were clouded with dense white vapor, and after some minutes filled a space nearly equal to 60. On the introduction of water, no absorption took place. When 43 of nitrous gas were admitted, the whole diminished to 70.
E.2. 25 of nitrous oxide were fired with 10 of phosphorated hydrogene, by the electric spark. After detonation[176]they filled a space exactly equal to 25. On the admission of solution of green sulphate of iron, and prussiate of potash, no blue or green precipitate was produced. On the introduction of water, no diminution was perceived. 25 of nitrous gas mingled with them, gave exactly 50.
E.3. 10 of nitrous oxide, mingled with 20 of phosphorated hydrogene, could not be inflamed.
25 of nitrous oxide, with 20 phosphorated hydrogene, inflamed. The gas after detonation, was rendered opaque by dense white vapor, and filled a space nearly equal to 45. No absorption took place when water was introduced. On admitting a little oxygene no white fumes, or diminution, was perceived. The electric spark passed through the mixture, produced an explosion, with great diminution.
c.FromE.1 it appears, that when a small quantity ofphosphorated hydrogene is inflamed with nitrous oxide, both the phosphorus and hydrogene are consumed; whilst the superabundant nitrous oxide, is converted into nitrous acid and atmospheric air, by the ignition; or a certain quantity is partially decomposed into atmospheric air by the combination of a portion of its oxygene with the combustible gas.
FromE.2 we learn, that when the phosphorated hydrogene and nitrous oxide are to each other as 25 to 10 nearly, they both disappear, whilst nitrogene is evolved, and water and phosphoric acid produced. Reasoning concerning the composition of nitrous oxide from this experiment, we should conclude that it was composed of about 38 oxygene, and 62 nitrogene.
The result ofE.3 is interesting; we are taught from it that the affinity of phosphorus for the oxygene of nitrous oxide is stronger than that of hydrogene, at the temperature of ignition; so that when phosphorated hydrogene is mingled with a quantity of nitrous oxide, not containing sufficient oxygene to burn both its constituent parts, the phosphorus only is consumed, whilst the hydrogene is liberated.
In repeating the experiments with phosphorated hydrogene that had remained for some hours in the mercurial apparatus, I did not gain exactly the same results; for a larger quantity of it was required to decompose the nitrous oxide, than in the former experiments; doubtless from its having deposited a portion of its phosphorus. They confirm, however, the above mentioned conclusions.
In the course of experimenting, I passed the electric spark, for a quarter of an hour, through about 60 measures of phosphorated hydrogene. It underwent no alteration of volume. Phosphorus was apparently precipitated from it, and it had wholly lost its power of inflaming, in contact with common air.