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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102.<br />
volume <strong>and</strong> then by pumping to a few microns pressure; this treatment would also<br />
remove F20. The sample was then warmed cautiously to decompose the F2@4 to<br />
F2@2; the O2 released was measured gasometrically. This oreration was carried<br />
out most successfully by removing the liquid nitrogen bath until a small increase<br />
in pressure was observed, replacing the liquid nitrogen, <strong>and</strong> repeating<br />
the process until the F202 could be melted (113°K) <strong>with</strong>out further oxygen<br />
evolution. The oxygen thus evolved i.as mass spectrometrically free of F2<br />
(hsiever, this was not a very sensitive test because the mass spectrometer<br />
inlet system vas somewhat reactive <strong>with</strong> small uantities of fluorine). The<br />
blood-red liquid F202 was then frozen at 77°K ?orange solid) <strong>and</strong> the residual<br />
O2 was pumped away. Subsequent remelting at 113°K resulted in no further re-<br />
' lease of OP. The sample was then warmed slowly to room temperature to decompose<br />
the F202 <strong>and</strong> measure the F2 + 02.<br />
This procedure was occasionally unsuccessful in cases <strong>with</strong> the initial<br />
mole ratio F2/02 of 1.0 or 3.0, because a minor explosion ("pop") would be heard<br />
dwing the decomposition of F2O4, accompanied by a sudden rise in pressure.<br />
The gasmetric data indicated that in these cases some of the F202 was decom-<br />
posed during the sudden decomposition of F204. Because of this, the apparent<br />
yields of F& <strong>and</strong> F202 reported in Table 1 are taken only from experiments in<br />
vhich there vas no audible evidence of explosion. Nevertheless, the reported<br />
yields of F204 may be slightly too high in some cases because of sane decomposi-<br />
tion of F202 during the decomposition of F204.<br />
The data reported in Table 1 show several unusual features. First,<br />
in the mixtures Containing only F2 <strong>and</strong> 02, the number of millimoles of oxygen<br />
converted to F202 ard F204 remain nearly constant despite a large variation in<br />
the initial ratio of F2 to 02, even when the major part of the oxygen was<br />
consumed. The G-value for products also remained constant at a value that is<br />
several-fol higher than the values that are usually found for non-chain<br />
conditions involves a short chain process that is initiated <strong>with</strong> approximately<br />
equal efficiency whether the initial absorption of energy is done by oxygen or<br />
by fluorine.<br />
These observations suggest that the formation of F202 under these<br />
,<br />
Another observation is that the ratio of F20 to F202 in the products<br />
displays no obvious trend vith the initial ratio of F2f02. The possible chain<br />
L F. 1 F2 1 F2 1 F2<br />
F2 F202 + F. F204 + F. F2@o + Fa<br />
'muld not lead to these results in a hcmogeneous system, but the kinetics are<br />
probably conplicated by the fact that the products precipitate as solids.<br />
The experiments in which the reactants were diluted <strong>with</strong> argon show<br />
that the presence of argon ha6 a small positive effect on the total conversion<br />
of oxygen, whereas dilution <strong>with</strong> citrogen does not appear to effect the yield.<br />
Some energy transfer from argon seems icdicated.<br />
a) G for ion pair formation is'expected to be about 4; for radicals it often<br />
ranges fran 6-10.