514 
PROFESSOR J. J. THOMSON ON SOME APPLICATIONS OF 
\k6- 
[i. />o 2 Po'Q® s «»5 8 _ ll _ 
or 
o 2 dw 
— _ P TeH 
Q 5 ■ 
where C x is a constant. 
From the equation 
o 
II 
we get, in a similar way, 
4*2 2 / dw \ 
f2 = Qc sE -»(d 
'dw\ 
Ml 
e constant 
(71) 
(72) 
Equations (71) and (72), along with the three equations (68), are sufficient to 
determine the live quantities y, £, e, a>. 
If we multiply equations (71) and (72) together, we get 
2 C (dw 
C, C 3 e* m ^ 
) + S) 
so that, as long as the temperature remains constant, is constant; or, in words, 
the ratio of the quantities of water and carbonic acid formed by the explosion always 
bears a constant ratio to the ratio of the quantity of hydrogen left free to the 
quantity of free carbonic acid. 
Since equations (71) and (72) involve Q, the amount of combination which goes on 
when a given quantity of the gases are exploded will depend upon the volume in 
which they are confined. The equations show that the amount of combination null 
increase as the volume diminishes. In a paper on the “ Chemical Combination of 
Gases ” '* I arrived at similar results (except with regard to the effect of temperature, 
which I did not investigate) by a purely kinematical method. 
Method applicable to Solutions of any Strength. 
§ 1 9. When the solutions are too concentrated to permit us to assume that the energy 
possessed by the molecules of the salt is the same as the energy possessed by the same 
number of molecules in the gaseous state, we must use the more general expression 
given on p. 487 for the positional part of L, viz., 
P’ dp 
6 f y- dv — 10, 
J V n Oe 
* ‘ Phil. Mag.,’ vol. 19, 1884. 
