secondary cells with lithium anodes and immobilized fused_salt
secondary cells with lithium anodes and immobilized fused_salt
secondary cells with lithium anodes and immobilized fused_salt
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dasel-ved vdxe of 7 9 are assunecl equd to + E-7, where AHo is<br />
the heat of reaction for Cg; C1F3 + 2r" (&Yo = 57 KCal/mole)<br />
IS t'ce nczivstion energy for the reverse of reection (7). Semenov's<br />
ai.<br />
gives 9-7 = 2.5 :(Cal/xole <strong>and</strong> 36 = 11.0 KCal/n;ole. The raciical-rGdic&<br />
xactlons (-5) =&(a)' are assmeri to have zero activetion energies. Therefore<br />
Z = i(57.0 + 2.5 + 11.0-0)- 35 KCal/aole. This value is somewhat lower thm the<br />
GbserveL value of h.3 KCal/nole <strong>and</strong> suggests thzt the long chain mechanism (C)<br />
+obaiLy is zot inportant in the decomposition of CWs.<br />
-..<br />
c _<br />
u.7;'ortmztely the data do not allow e choice to be nade between the molecular<br />
illmination mechanis-3 (A) za8 the non chain mechanism (B). Thermochemical data<br />
give Keq = 10 -~.a5~;+<br />
for the reverse of reaction (4). Therefore,<br />
U = + 105-8 e-(-22,&0/i~) liter/mole sec.<br />
r.ot unreasonable for a bkolecular reaction.<br />
reaction (A) camot be eliminated.<br />
The A factor 105-8 liter/nole sec is<br />
fience, the nolecular elimination<br />
If the non chain radical mech&nisn (B) is correct, then the measured activation<br />
energy, h0.3 XCal/mole, is equal to the bond dissociation energy for the first C1-F<br />
bond in C1? Tnis value seems reasonable since the average bond enerfg in ClF5 is<br />
j6 i~al/~Oie5'5. Further support for the non chain radical mechanism is given<br />
by the generalization of Benson <strong>and</strong> DeNore6 that the A factor f uninoleculy<br />
reactions involving the splitting off of atms are in the range of 10' to 1015sec- .<br />
It now remains to discuss the recent photochemical investigation by Krieger et<br />
2<br />
a l e<br />
They studieC tne kinetics of the photochemical formation of ClF5 from<br />
clF3 ana T2 (365 su, 16-70') an8 obtained the complex rate expression:<br />
,<br />
5eir sonewhat unllsual nechanisn involves the formation of an activated ClF5 molecule<br />
which can (1) be collisionally ceactivzted to CW5, (2) react directly <strong>with</strong> C1F3 to<br />
,Corn 2 CF4 raLicals, or (3) +it into CU4 + F. In order to explain their observed<br />
results (quantum yield aependent on inert gas pressure <strong>and</strong> on ClF3 pressure), all<br />
*- "r-ee 1 of these processes nust occur to an appreciable extent in each of their experlzents.<br />
PI,. L..cse pLotochezica1 results indicate that the CP5 activatec? nolecule decomposes<br />
r.oze rapi~f thazz classical theory would predict. Also, the thermal decomposition<br />
of CL75 stould be press'ure ciependent <strong>and</strong> accelerated by the presence of the product<br />
CLT2.<br />
,7- -..e tkezzial &:.d -,hotoche-;lical resfits can be shown to be compatible in two ways.<br />
-._.".A i.. caz bc calculated from the photochemical rate constaqts that the accele.-3*-.-<br />
- effect 0:' Cll3 woiia not be sufficient to appreciably affect the first-order<br />
plot shoi.3 In Fig. 1. Therclal experiments would have to be run <strong>with</strong> added CLF3 <strong>and</strong><br />
at various total pressures to determine if the decomposition is dependent on the<br />
. . I<br />
- .- .<br />
7. :;. :;. Sc~anov, "Sozle Iro3iess in Chemical Kinetics ana Reactivity," Volune I,<br />
princeton University ?res, Princeton, New Jersey, 1958, P 29.<br />
"li Y.