ORNL-1771 - Oak Ridge National Laboratory
ORNL-1771 - Oak Ridge National Laboratory
ORNL-1771 - Oak Ridge National Laboratory
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4NP QUARTERLY PROGRESS REPORT<br />
on d<br />
3FeC12 = 2FeCI, + Fe , Fo = 0.35 V.<br />
The NiCI, solutions, as far as is known, undergo<br />
the same electrochemical reactions regardless of<br />
concentration. Thus the changes in decomposition<br />
potential with concentration may be assigned to<br />
differences in NiC!, activity alone. With the aid<br />
of the Nernst equation, the NiCI, activity at 33.3<br />
mole % NiCI, may be coniputed to be 100 times that<br />
in the 3.3 mole 76 solution and 300 times that in<br />
the 1 mole % solution.<br />
Solubility of Xenon in Molten Salts<br />
R. F. Newton, Researcli Director's Department<br />
D, G. Hill, Consultant<br />
The use of molten salts as reactor fuels offers<br />
the possibility of removing the gaseous fission-<br />
product poisons, of which zmon is the rnost im-<br />
portant, If, for example, the xenon concentration of<br />
the SO-Mw CFRE can be held at 10% of its equi-<br />
librium value (1.1 x mole of xenon per milli-<br />
I iter of fuel), important perturbations in reactivity<br />
can be avoided, In on aircraft reactor, however,<br />
it will be nccessary to effect this removal nd xenon<br />
with on absolute minimum of ouxiIiary equiprrient.<br />
The available literature appears to contain no<br />
measureinents of she solubility of gases in molten<br />
salts. Accordingly, it has seemed desirable to<br />
evaluate the solubility of xenon in molten fluorides<br />
over the temperature range of interest. Preliminary<br />
tests indicate that the following experimental tech-<br />
nique is satisfactory.<br />
The apparatus, which is constructed of nickc!<br />
where it will be in contact with the fluoridc melt<br />
and of glass elsewhere, consists of two sections<br />
that can be isolated by freezing a plt~g of fluoride<br />
in the U-tube connecting them, In one section of<br />
the apparatus the melt is allowed to saturate with<br />
xenon under predetermined conditions of ternpera-<br />
ture and pressure. Melting of the fluoride plug<br />
permits the saturated salt to flow into the other<br />
section, whi!e the 1J-tube seal prevents entrance of<br />
gaseous xenon into this section; refreezing of the<br />
plug isolates the sections again. 117 the second<br />
section, xenon is stripped from the salt by repeated<br />
circulation of the hydrogen contained in the a p p<br />
ratus through the salt and past a liquid-nitrogen-<br />
cooled trap. After the stripping process is com-<br />
plete, the hydrogen is removed, $he xenon is allowed<br />
to come to room temperature, arid he amount col-<br />
70<br />
lected is ascertained by measurements in a modi-<br />
fied Mcl_eod gage.<br />
Preliminary experiments at 600'6 and essentially<br />
1 atm of xenon indicate that the solubility in the<br />
NaF-KF-LiF eutectic is not greater than loM7<br />
mole of xenon per milliliter of salt. The method and<br />
technique proved to be feasible, but minor experimental<br />
difficulties necesFitatsd modification of<br />
the nickel apparatus. More accurate data under<br />
these and other conditions will be available in the<br />
near fWtIJre.<br />
Meanwhile, in order to gain familiarity with the<br />
technique, the solubility of xenon in the KNO,-<br />
NaNQ, eutectic (36 mole '36 NaNQ,) has been<br />
measured in an apparatus constructed entirely of<br />
glass. The solubility of xenon in this melt is<br />
about 8.5 x mole/itil at 280°C and low7<br />
mole/ml at 360°C. This liquid apparently shows<br />
the positive temperature coefficient of solubility<br />
expected for gases in molten salts.<br />
%-Ray DiFfr~~fi~n Studies in Salt Systems<br />
P. A. Agron M. A. Bredig<br />
Chemistry Division<br />
Cesium Halides. It has been suggested21t22 that<br />
the increase in volume on melting of simple binary<br />
salts is indicative ofstructural changes in the melt,<br />
that is, of a decrease to a lower ionic coordination.<br />
Volume increases up to 30% have been indicated for<br />
the alkali halides. The x-ruy data23 on the thermal<br />
expansion of solid CsBr and Csl gave volume<br />
changes of approximately 26%, but an extrapolation<br />
of about 50°C to their melting points WQS required<br />
for the computation of these changes. It WQS there-<br />
fore of interest to uscertain whether a solid-phase<br />
transition analogous to the one known to exist in<br />
CsCl occurs in the unexplored temperature interval.<br />
This would replace the assumed structural change<br />
in the melting process by one in the solid state.<br />
High-purity CsBr and Csl were intimately mixed<br />
with fine nickel powder to provide airs internal<br />
stairdurd whose thermal expansion is know BCCU-<br />
rate~y.,~ ~attice parameters as a function of tem-<br />
perature were obtained on the hi yh-temperature<br />
21J. W. Johnson, M. A. Bredig, and W. J. Smith, Gem.<br />
Dzv. @LOT. ?Tog. Rep. Der. 31, 1952, <strong>ORNL</strong>-1482, p 32.<br />
,P, A. Agron and M. A. Bredig, Ch~rn. Semzann. Prog.<br />
Rep. June 20, 1954, ORML-1755 (in press).<br />
24Ls Jo;dan and W. H. Swunger, J. Research Nnt. Bur.<br />
xtandn7ds 5, 123 i ( 1930)-