SOLUBILITY ASD ESTROPY OF SOLYTIOSS OF GASESIS S'SRIOVS SOLVESTS
Feb., 1961
+ C1+ Br+ C1
+ + +
AtC12IAtBr2I= IC12Br-
331
prise after the striking photochemical reactions reported p r e ~ i o u s l yand , ~ we see once again that the influeiice of light on tracer-level reactions cannot IBrCl be safely disregarded. n-hich have equilibrium constants of 2 X and 6 X lop3,respectirely, the last at 1.1 X Acknowledgment.-I wish to express my grati25 15,16 tude to Professor I. Perlman for his direction of this The photosensitivity of the astatine distribution research and to Professor Robert E.Connick for a in the prrsenre of IBr should come as no great sur- great, deal of helpful discussion. AtIC1-
ItIBr-
=
=
(18) (22) (23)
SOLUBILITY ASD ENTROPY OF SOLUTION OF He, S?,A, O?, CH4, C2He,CO, AND SF, I N VARIOUS SOLVENTS; REGULARITY OF GAS SOLUBILITIES BY T.KOBATAKE AND J. H. HILDEBRAXD Department o j Chemistrg, University o j California, B e r k d e y , Caltfornia Recezved August 28, 1960
The apparatus and proCareful measurements of gas solubility in selected solvents have been made in the range 5-30'. (-edureare described in some detail. The gas, solvent, mole fraction x 104 a t 1 atmosphere and 2 5 O , and the entropy of solution, cal. mole-'dg.-', respectively, are: N2/CS2 2.215, - 1.77; CHa/CS212.69, - 1.77, C02/CS232.80, -4.83; S F d CR, 9.245. -0.30: CO,/C,F,R 208.8. -7.53: CHI/C,F,C82.62. -3.40: He/C7F7F. 8.90. 5.30: SFR/C,F,, 224.3 -8.00: Kz/ (C4F-s)3N-34.901-0.54; x/(C4F9)3N 50.03,'- 1.71.; ~02j1C4F9);N52.0,' - 1.90;' C 0 2 / ( C a F g ) & 200, - 7.30; C2H&/(CaFs)8 332.7, -8.80; Oz/i-CsHls 28.14, - 1.32; C2Hs/i-CsHls293.8, - 10.15; SF6/i-C8Hls153.5, -7.45. These and many other figures are plotted as (a) entropy of solution us. -R In 5 2 : (b) log x2us. solubility parameters of solvents; (e) log xz us. force constants of gases. They show extensive regularities with high predictive value and theoretical significance.
The work here reported is a continuation of systematic studies of gas solubility in the light of regular solution theory extending over many years and recently greatly intensified. 1-5 Careful determinations by Reeves4 of the solubility of argon in
five non-polar solvents over a range of temperature yielded important information about the different temperature coefficients of gas solubility. Jolley and Hildebrands published values for partial molal volumes and gave quantitative relations between
G
4
2
0
3 I
-2
I8
-4
-6
-8
- 10 - 12 8
10
12
-R In 2 2 . Fig. 1.
14
lG
18
Y. KOBATAKE AND J . H. HILDEBRAND
332 I
I
I
I
200
250
- 1.0
- 1.5
-2.10
H“
g -2.
