1012 
table V, in which the value 34690 cal. has been chosen for Yn Ero 
so that in my opinion the most probable expression for the disso- 
ciation constant is as follows: 
972 
7589 
1 Bik 
log K = — 5 + > log T + log (1 T ) + 1.887 . (13) 
TABLE ME 
= ia oe l 
f(Cels) | „Tor K (found). log K (calc.) difference 
| 
800 | 1073 | 0.111—4 | 0.104—4 | — 0.007 
| 
900 |. 4173 | -0,692-A4 | .0.708=4 | 40-00 
1000 1273 | 0.199—3 | 0.206—3 | + 0.007 
1100 | 1373 | 0.639-3 | 0.634-3 | — 0.005 
1200 1413 | 0.009—2 
| | 
0.003 —2 | — 0.006 
The diserepancies between the found and the calculated values 
are smaller than the errors of observation. 
8. Before proceeding with the calculation of chemical equilibria 
by the aid of the expressions for the gas entropy mentioned in § 2 
and Prof. vaN per Waats Jr.’s expression mentioned in § 4, I will 
discuss the results at which Stern has arrived in his paper, which 
I mentioned in the “Postscript” of my latest communication. 
The expressions for the gas entropy used by Srern, deviate in a 
very essential point from those mentioned in $ 2. The entropy of 
a gas is determined by Srern with respect to the solid state at 
T—O as zero condition. The expression for monatomic gases 
agrees with equation 1 of my first paper, when there the value 
3 5 
7 ln 2 + R-+S solid at T=0 
js substituted for C,. In the same way the value of a di-atomic 
Roy 2 
gas is indicated by equation 2, if En R + Ssotid at T=0-') is taken for 
C,. It is clear that in contrast with the application of the entropy 
values of § 2, therefore according to Stern the algebraic sum of the 
entropies of the solid substances at 7’=0 occurs in the expressions 
1) Besides Stern takes the vibration in the diatomic molecule into account, 
which in equation 2 necessitates the addition of an expression with v. Also the 
variability of the specific heats is therefore taken into account with this expression, 
