1018 
and ATKINSON ') we find further that the determinations at the lowest 
temperatures, where the degree of dissociation is very small, are 
useless for the calculation. If the term with v is omitted from 
equation 6, it can be brought into the following form for the bromine 
dissociation : 
3 
. + — log T — 88802, % (14) 
in which w represents the degree of dissociation at atmospheric 
pressure. Application of this expression to the experimental deter- 
minations yields the following table : 
TABLE VI. 
| 2nd member ATCy 
t x of (14) (TC)—9 | (AT Jo 
900 0.0148 |  —30.039 35236 
—40.75 
950 | 0.0253 a ab lead tee ge 
| —39.85 
1000 | 0.0398 — 30.845 39266 
| — 40.75 
1050 | 0.0630 | —31.220 | 41304 
| mean — 40.45 
The thus found value of — 40.45 yields 4.10—!° em. for the radius 
of inertia. If the experimental determinations do not contain great 
errors, a very small radius of inertia follows from this calculation. 
And this radius would be found still smaller, if the term with » was 
taken into account. I think, however, that no great importance is 
to be attached to this value, because the values of the fifth column 
differ too much from each other, and the determinations are less 
numerous and less accurate than for the iodine dissociation. The 
accuracy is here again smaller, because the equilibrium lies strongly 
on one side in these determinations. 
13. The equilibrium 2ABZ A, + B 
When Prof. van Der Waats Jr.’s considerations are applied in a 
perfectly analogous way to the equilibrium 2 AB A, Bb,, we 
find for the dissociation constant: 
SnET—0 
2 
ih 
Se a he = en 
NA. NB: > myg.mp, M,M ee 4) 4 
eee R1 a ee en (15) 
2 3 U2 : 
NAB map Ma al je 
le KT) \l—e KT 
1) PERMAN and Arkinson, Z. phys. Chem. 38. 215. 577 (1900) Cf. also: Arzoo. 
Handbuch 4. 2. 233 (1913), 
