ORNL-1771 - Oak Ridge National Laboratory
ORNL-1771 - Oak Ridge National Laboratory
ORNL-1771 - Oak Ridge National Laboratory
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Stability of Chrorni lam Compounds in<br />
Molten IF! uor ides<br />
J. D. Redinan C. F. Weaver<br />
Mater i al s Chem i s try Divi s ion<br />
It was shown in previous experiments that CrF,<br />
or some complex compound of divalent chromium<br />
was fhe corrosion product in the ZrFdobase fluoride<br />
melts of interest. However, when NaF-KF-LiF<br />
mixtures, with and without UF,, were tested in<br />
equipment prepared from al ley s containing chromium,<br />
the reaction products found were complex com-<br />
pounds of CrF,. Since films that were apparently<br />
NaK,CrF, or similar materials have been observed<br />
in some experiments, attempts have been made to<br />
observe the stability and soluLility of CrF, and<br />
CrF, in typical salt mixtures of the two types.<br />
In the temperature range 600 to 8RQ°C, CrF, is<br />
not stable in NaZrF, solution in contact with<br />
equipment of nickel. Examination of filtered speci-<br />
mens shows that the reaction<br />
2CrF, + Ni ,A NiF, + XrF,<br />
proceeds to essential completion, The solubility<br />
of 6rF2 in the NaZrF, solvent seems to exceed<br />
6000 parts of Cr per million parts of salt at 600%;<br />
solubility at 800°C seems ta be at least 15,000 ppm<br />
and may be consideratly higher.<br />
In the NaF-KF-LiF system it appears that CPF,<br />
is not stable. Whether the disproportionution re-<br />
action<br />
3CrF,-dCr0 i 2CrF,<br />
or some other mechanism is involved 15 not evident<br />
from the data available. It appears from preliminary<br />
evidence, however, that the solubility of Cr3' is<br />
several thousand parts per million at 600OC.<br />
Reduction of NiF, by H, in NaF-ZrF, Systems<br />
C. M. Blood H. A. Friedman<br />
G. M. Watson<br />
Materials Chemistry Division<br />
The use of hydrogen as a reducing agent in the<br />
removal of oxidizing impurities from fluoride melts<br />
has been routine for almost two years. One of the<br />
principal impurities removed is the Ni +' introduced<br />
as a result of treating the melts with hydrogen<br />
fluoride in nickel containers at 80OoC, Since<br />
hydrogen was first employed in this fashion, kinetic<br />
studies have been under way in order to supply data<br />
on which improved fluoride production procedures<br />
PERIOD ENDING SEPTEMBER 70, I954<br />
could be based. The Ni" was found to reduce so<br />
rapidly that the controlling step was the rate of<br />
removal of hydrogen fluoride from the melt; hence<br />
the chemistry of the process presents no problem of<br />
consequence from an engineering standpoint. With<br />
the completion of measurements at 800'C during the<br />
past quarter, these studies have been di scontinued.<br />
The experimentol method used for the measure-<br />
ments at 800°C was the same as that used in<br />
previously described experiments at 600 and<br />
?Oo°C.'8 Figure 5.5 shows a comparison of the<br />
effect of temperature on the rates of reduction for<br />
four concentrations. The slopes of the curves show<br />
that the apparent activation energy for the rate de-<br />
termining step is about 7800 cal, This energy of<br />
activation is in accord with the hypothesis that<br />
the reaction is heterogeneous and is catalyzed by<br />
nickei surfaces.<br />
18G. M. Wutsan, C. M. Blood, F. F. Rlankenship, ANP<br />
Quar, Prog, Reg). MUT. 10, 1954, QRNL-7692, p 62.<br />
____ ................. ...... ~-<br />
J .... .I ......... '<br />
fl~<br />
............. -<br />
~~ ..............<br />
A.-<br />
Fig. 5.5. Effect of Temperature and Concentra-<br />
tion on the Rate of Reduction of Nif, by H, in<br />
Molten NaF-ZrF1 (53-47 mole %).<br />
63