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Contraction of 1000 measures of liquid when 28.56 56.02

cooled from the boiling point to a tempera

ture 50° below it Quantity of vapour at 100° (in litres) produced 1.700 0.661

by 1 gramme of liquid Measures of vapour at 100° produced by 1 1633:1 488.3

measure of liquid at the boiling point

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B F8

33:42 2.3190 2.3124 Ds 2.3694 To 2-3709 JD N

0-9706 0-9426 L 0.967 HD 0-9691 BA

0-972 DB

0.9729 To 0.9757 BD 0-985 K NO ......! 22 1:5252 1.3629 Bt 1.5204 Co 1.5269 To

1.614 Da N0...... 15 1.0399 1.0388 Be 1.041 To 1.094 HD

1.1887 K NO.

23 1.69.16 1.72 Mt
NH3
8.5 0.5893 0-5901 HD 0.5931 To 0-5967 BA

0.80 K0.6022 AP
NH3, C 02 13 0.9013 08992 Ro | 0-90 Bi
NH3.28 H 12.74 0.8840 0.884 Bi
NH', CIH 13:38 0.9255 0.890

Bi
Si?

14.8 1.0261 Si C1

85.6 5.9347 5.939 Ds Si F'

522 3.6190 35735 JD Ti?..

24.5 1.6986 Ti C1

95.3 6.6072 6.836 Ds 3.600 Ds 4.17 Da Cr C19, 2Cr 79.5 5.5117 5.5 Ds 5.9 W As

150-4 10 4272 10.6 Mt As 08

1984 137551 13 85 Mt As H3

39-1 27108 2.695 Ds As 13 226.6 15-7102 16:1

Mt As C13

90.7 6.2882 6.3006 Ds Sb?

258 17.8871 Sb C13

1176 8:1532 78 Μο Te?

384 26.6227 Te H

65 4.5064 4.49 Bi N HỒ, Te H 2016 1.4213 1.32 Bi Bi?.

106.4 7.3767 Bil C13? 158.5 10.9888 11-35 Jq Sn?

59 4.0905 Sn C1

129.8 8.9990 9.1997 Ds Hg 101.4 7.0301 6.976

Ds 7.03 Hgs

78.27 5.4262 5:51 Mt Hg I 227.4 15.7656 15.9 Hg? Br.

110-6 9.7478 10.11 Mt Hg Br 179.8 12:4656 12:16 Mt HgCl..

119.1 82572 8.35 Mt
136.8 9.4813 9.8 Mt

7.1602 13-5460 17.8692

3:5216 3-5023 Ds
20-4091

8.1690 8:1852 Ds
23.2371
10.5918
34.5855
5.8543
1.8464
9.5831
14.2755

5.3139
11.6906 11.9511 Ds
9.1328 9.0625 Ds
7.0492
20:4811
12.6634
16.1941
10.7269
12-3211

Mt

Mt

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Remarks on the preceding Table.
AP. denotes Allen & Pepys; Be. Bérard; Bf. Buff; Bi. Bineau; Br.
Brisson; Bt. Berthollet; Bz. Berzelius; BA. Biot & Arago; BD. Berze-
lius & Dulong; BG. Biot & Gay-Lussac; Ca. Cavendish; Cb. Couerbe;
Co. Colin; Cr. Cruikshanks; CD. Clement & Desormes; Da. Dalton; Dm.
Deiman; Ds. Dumas; Dz. Despretz; DB. Dumas & Boussingault; FS.
Fourcroy, Vauquelin, & Seguin; G. Gay-Lussac; GT. Gay-Lussac &
Thénard; H. Henry; HD. Humphry Davy; JD. John Davy; Jq. Jaque-
lain; K. Kirwan; L. Lavoisier; Ma. Marchand; Mt. Mitscherlich; Rg.
Regnault; Ro. Rose; S. Saussure; Te. Thénard; Tf. Tromsdorff; To.
Thomson; Tr. Tralles; W. Walter.

The calculation of the specific gravity of gases rests upon the follow-
ing suppositions: (1.) That the atomic weights of the elementary bodies
are those given on page 50, and consequently, that if one measure of oxy-

gen gas weigh 16, one measure of nitrogen gas will weigh 14, and one measure of carbonic acid gas 22.—(2.) That the air is a mixture of 21 measures of oxygen, 78.95 of nitrogen, and 0.05 of carbonic acid gas. If x denote the sp. gr. of oxygen, y of nitrogen, and z that of carbonic acid gas (that of air = 1) then 0.21 x + 0.7895 y + 0.0005 z = 1; moreover, 7 x = 8 y; and 11 x = 8 z. From this we find that the specific gravity of oxygen is 1.10926, that of nitrogen 0.9706, and that of carbonic acid gas 1.5252. From one of these three magnitudes, taken as a starting point, the specific gravities of the remaining substances have been calculated according to their atomic weights,—and from the same data it has likewise been determined whether they undergo 0, 1, 3, 6, 9, 12, 18, or 24-fold expansion in the gaseous state. The specific gravities of those substances which in the table bave a note of interrogation put after them, have never been determined by direct experiment; in the hypothetical calculation of them it has been assumed, according to analogy, that the vapours of selenium and tellurium are 6-atomic, vapour of antimony 2-atomic, and the vapours of carbon, boron, fluorine, hydrofluoric acid, silicium, titanium, bismuth, and tin, are 1-atomic gases. The differences between the results of calculatiou and experiment are easily explained in the case of vapours, because the exact determination of their specific gravity is subject to great difficulties. The differences between the results of calculation and observation in the case of the permanent gases perhaps arise from the adoption of incorrect hypotheses in the calculation, e.g. the atomic weight of nitrogen may have been assumed too low. Since, however, the results of the most distinguished observers frequently differ more from one another than from the calculated specific gravity, a new and exact revisiou of the specific gravities seems to be required, to enable us to decide positively respecting the correctness or incorrectness of the assumed hypotheses.

One litre (or 1 cubic decimetre) of water at + 4° (its point of greatest density) weighs 1000 grammes. 1 litre of atmospheric air under the 45th parallel of latitude, at 0° C. and 0.76 met. atmospheric pressure, weighs, according to Biot & Arago, 1.2991 gramme (according to Dumas & Boussingault 1.2995). This gives for the weight at 4°,-since at this temperature (p. 224) the air is expanded zią of its bulk at 0o (278 : 274 = 1.2991 :X), 1.28 gramme.

To find the weight of a litre of any other gas at 0° and 0.76 met. bar. multiply the specific gravity of the gas by 1.2991 (the sp.

1). In this manner we may obtain with tolerable accuracy the relation by weight of water to the gas, since 1 litre of water weighs 1000 grammes; only it must be remembered that the weight of the gas is taken at 0°, and that of the water at + 4°. If we would find the relation between the specific gravities of the gas and water at the same temperature, viz. + 4°, we must assume that of water = 1000, and multiply the sp. gr. of the gas (that of air = 1) by 1.28.

According to the preceding, the specific gravity of air at 0°, and under a pressure of 0.76 metre, is to that of water at + 4° as 1.2991 : 1000; hence (since 1.2991 : 1000 = 1:769-7) water is 770 times as heavy as air. If, then, the sp. gr. of air = l, that of water = 770; and if the specific gravity (that of water = 1) of any liquid or solid body be multiplied by 770, the product will be its specific gravity, taking that of air = 1. On the contrary, to reduce the sp. gr. of a gas (air = 1) to what it will be, taking water 1, we divide the former by 770. To find the expansion which a body undergoes in assuming the gaseous form, multiply its sp. gr. (water = 1) by 770 (the product will be its sp. gr. air = 1),

gr. of air

and divide this product by the sp. gr. (air = 1) which it has in the gaseous state; e. g., in the case of water: 1.000 (sp. gr. of water) x 770 = 770; and 770:0:6239 (sp. gr. of vapour of water) = 1234-1;—for sulphur 4995774 = 231•4; that is to say, 1 volume of water at do yields 1234:1 volumes of vapour of water at oand 0.76 met. pressure; and 1 volume of sulphur yields 231'4 volumes of sulphur vapour.

[Poggendorff's tables on the specific gravity of gases. (Pogg. 17, 259; 21, 629; 41, 449; 49, 416.)-Buff's method of determining the specific gravity of gases. (Pogg. 22, 242.) Dumas' Directions for determining the sp. gr. of gases. (Ann. Chim. Phys. 33, 341; also Pogg. 25, 236; also Ann. Pharm. 3, 59.) Mitscherlich's. (Pogg. 29, 193.)]

C. Quantity of Heat in Gases. The quantity of combined heat in gases varies according to the nature of the ponderable body, and likewise according to the pressure to which the gas is subjected.

a. According to the Nature of the Ponderable Body. The quantity of combined heat in the more permanent gases can only be approximately determined from the development of heat which takes place in the chemical combination of their ponderable elements with other substances to form non-gaseons compounds;—this development of heat is, however, partly due to the act of chemical combination. The quantity of heat set free in the absorption of acid gases and ammonia by water being but small, it would seem that these gases possess less heat of fluidity than vapour of water and some other vapours.

The quantity of heat in vapours is found by conducting a known weight of the vapour (produced by boiling the non-gaseous element in a retort) through a worm-tube, or into a receiver surrounded with a known quantity of water-or, in the case of vapour of water, directly into the water and observing the increase of temperature produced in the water by the condensation of the vapour. This increase of temperature (expressed in degrees) multiplied by the volume of water in the receiver (the weight of the condensed vapour being assumed = 1) is equal to the heat of fluidity set free by the condensation of the gas,' + the decrease of temperature which the condensed matter undergoes from its boiling point to the temperature exhibited by the water at the end of the experiment.—Persoz (Chim. molec. 250) heats the liquid to its boiling point, and then drops it with a pipette upon mercury, the temperature of which is about 50° above the boiling point of the liquid, till the mercury is nearly cooled down to that point,--and determines the quantity of heat which has become latent, by observing the temperature of the mercury before and after the experiment, the quantity of the mercury, and that of the liquid evaporated.

Table of the Latent Heat of Vapours. Column A: Name of the substance.—B: Its specific gravity in the liquid or solid state.—C: Number of degrees centigrade above 0° which the vaporized body would exhibit at its boiling point, if none of the heat were rendered latent.--D: Deducting from this the heat required to raise the substance from 0° to its boiling point, the remainder is the quantity of latent

heat in the vapour at the boiling point.-E: Number of degrees by which the temperature of water at 0° would be raised by the quantity of heat which the same weight of vaporized matter at its boiling point would give up, if it were to lose its gaseous condition and be cooled down to 0°.-F: The same after deducting the quantity of heat required to heat the substance from 0° to its boiling point, -and found by multiplying the specific heat by the number of degrees at which the boiling point is fixed. This column F serves, therefore, for comparing the quantities of latent heat in different vaporized substances. If the numbers in columns E and F be divided by the specific heats of the respective substances, the quotients will give the numbers in columns C and D:-- these numbers might be obtained directly by experiment if the vapours of the several substances were passed, not through water, but through the bodies from which they are respectively formed, e. g. vapour of alcohol through cold alcohol, &c. -G: name of the observer.

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The quantities of heat required for vaporization appear to be to one another nearly in the inverse ratio of the densities of the vapours produced, and therefore also, in some measure, of the atomic weights of the corresponding substances: for on multiplying the latent heat of a vapour by its specific gravity, we obtain a set of numbers nearly equal to one another. If the latent heat belonging to the substance in its liquid state, which, however, is known only in the case of water, were added to the other portion of latent heat, a more exact coincidence would perhaps be obtained.—This law, however, does not yet agree with the results of experiment sufficiently well to entitle it to be considered as established. (Comp. Th. Saussure, N. Gehl. 4, 97; also Gilb. 29, 126; Ure, Ph. Trans. 1818, p. 385; also Schw. 28, 360; Despretz, Ann. Chem. Phys. 24, 323.)

5. I subjoin the following table of the latent heats of vapours recently determined by the experiments of Favre and Silbermann

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