ORNL-4191 - the Molten Salt Energy Technologies Web Site
ORNL-4191 - the Molten Salt Energy Technologies Web Site ORNL-4191 - the Molten Salt Energy Technologies Web Site
centration (97% removed). The distribution of prot- actiriiurn was as follows: 72 2% in the steel wool plus untransferred salt, 4.3% in the unfiltered salt transferred away from the steel wool, 8.7% in the steel liner and dip leg, and 12.0% in saiiiples, for a total of 97.8% recovered. The data obtained in Lhis experiment confirmed the resulis of previously icprted7 experiments that indicate the Rrillo process may warrant further examination. Thorium Reduction Followed by Fiitratior! We reported earlier6 that a large fraction of the reduced protactinium that would not pass through a sintered copper filter was found in samples. of unfiltered salt. This suggested the possibility of collecting the reduced protactinium on a rrietal filter from which it could presumably be removed by dissolving it in a molten salt after passing I-IF through the filter. We performed several experiments to test the efficiency of protactinium recovery by filtration. The initial treatment of molten LiF-ThF4 (73-27 mole %) mixed with enough 231Pa to give a concentration of 20 to 60 ppm was performed in unlined nickel pots. The molten salt was treated first with mixed hydrogen and HF, followed by a brief hydrogen treatment before it was transferred through a nickel filter into a graphite-lined pot equipped with a graphite dip leg. Here the reduction of protactinium was carried out in the usual fashion, either by exposure to a solid thorium rod or to thorium turnings suspended in a nickel basket, taking sainples of filtered and unfiltered salt after each thorium treatment of the melt. The reduced melt was then transferred back into the nickel pot through the transfer filter. In four experiments the amount of protactinium found in the transfer filter varied from 10 to 30% of the total amount present. This represented 40 to 95% of the amouiit of protactinium suspended in the reduced salt (average, 69%). The amount of protactinium in the graphite liner and dip leg varied frorn 20 to 57% of the total (average, 33%). The data show that a filtiation method will not catch prntactinium on the filter, but nevertheless the removal of protactinium from a melt does appear feosible. One experiment was attempted with a niobium liner and dip leg. The reduction of protactinium with thorium proceeded normally (12% of the Pa remained in the filtered salt after 2 hr of thorium treatment), but transfer of the reduced salt through the filter could not be effected because of a clogged 154 filter. A considcrable amount of grayish. material was found in the bottom of the pot after it cooled to room temperature. A sample of this material was reported to contain only 0.35 mg of Nb per g, but it is quite possible that this aruount of iinpuiity in the molten salt wodd have been sufficient to clog the filter. The effect of iron on the behavior of protactinium in thorium reduction experiments has noi been defined imambiguously as yet, but we continue to find reasonably good correlation between the distribution of iron and protactinium in these experiiiients. Counting of 233Pa and 59Fe in both solid samples and solutions of samples provided a check on the accuracy of 23 'Pa alpha pulse-height analyses and colorimetric iron determinations. Concl us ion - 1 horium metal is an effective agent for reducing protactinium in molten fluoride breeder blanket mixtures, but further study will be required to determine the best method of separating the reduced protactinium from the salt mix. R FUEL REPROCESSING BY REDUCTIVE EXTWACTaCaN INTO MOLTEN B!SMUTH I). M. Moulton vir. R. Grimes F. F. Blankenship J. H. Shaffer An electromotive series for the extraction of fission products frorn 21,jF.BeF2 into liquid bis- miiih has been constructed in the way described for the MSBR blanket materials in the preceding ieport in this series. Briefly, standard half-cell reduc- tion potentials are calculated for each metal, using as the standard states the ideal solutions it1 salt and bismuth extiapolated from infinite dilution to unit mole fraction. 'The exception is lithium, for which the standard state in sa1.t is 2LiF.BeF2. (This standard state is also used for beryllium, but it is not assigned a standard state in bismuth be- cause of its very low solubility.) This choice of standard states is the normal practice when deal- ing with dilute solutions. These standard poten- 3~ i tials are called 'P d to distinguish thein from yo, 9.VSH Program Serniann Pro&. Rept. Feb. 28, 1367, ORNIA~~~, p. is(?.
the standard potential for reduction to pure metal. Thus, is the potential corresponding to the extraction process and does not require the simultaneous use of metal activity coefficients that are far from 1 at infinite dilution. It. should perhaps be noted that the electromotive series is thermodynamically equivalent to other means of expressing the free energy of the extraction process, such as equilibrium constants or decontaminaiion factors. It is used because it permits ranking the metals in an order which djrectly indicates their relative ease of extraction regardless of their ionic valence and because it has proven useful in the experiments where a beryllium reference electrode is used to monitor the reduction process. From data previously reported the series has been constructed as shown in Table 12.2. The numbers in parentheses after the rare earths are the potentials calculated by using the experimental C' fractional valences. For beryllium, (.- o, the potential for reduction to the pure metal, is shown. All of these except ~e'+ are calculated relative to the Lit value. Although better measurements may change these values somewhat, they indicate the relative ease of extraction. 'The numbers in parentheses are probably a better approximation to the true values despite the peculiar valences. All elements up through europium can be extracted completely k- fore metallic beryllium begins to form; this forma-tion of He" represents the ultimate limit of the process. An order of magnitude change in the ratio [(mole fraction in metal)/(moIa fraction in saltjl corresponds to 0.057 v for divalent and 0.058 v ior trivalent species. Table 12.2. -?; at 600°C (volts vs H2-HF : 0.00) t Li BaZ+ EU 2 '- Nd3+ + SmZ ce3+ La3i 1.92 1,81 CF o) 1.79 1.62 (1 61) 1.58 (1,511 1.58 (1.49) 1.57 (1.45) 1.52 (1.47) ~ 155 We have begun a reinvestigation of fission product extraction. In this study we will measure fission product distribution as a ftirlction both of lithium concentration nnd of temperature with (hopefully) improved accuracy. Preliminary results of the first of this series, using cerium, are shown in Fig. 12.5. A failure ended the experiment before good concentration data could be gotten, but those wc: did get: indicate a valence close to 3, not 2.3 as before. The apparent minimum of ?; (Ce) at 700°C is not explained arid is rather hard to believe. For lithium, f''; was calculated from the measured lithium concentration and the potential between the bismuth pool and beryllium metal electrode, for which the temperature coefficient is known. The "MSR Program Semianri. Progr. Kept. Feh 28. 1966, ORNL-3936, p. 141. 11 C;. F, Haes, Jr~, Keactor Chern. Div. Atin. F'rogr. Rept. Dec. 31, 196.5, ORNL-391.3, p, 20. 2.4 2.0 1.9 i .a - > - . 4.7 Q 4.6 4.5 .n, ORNL. DWG 67-14825 __ . . ._ 7.- +.3 400 500 600 700 800 900 T ("GI Fig. 12.5. b:i for Lithium and Cerium.
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<strong>the</strong> standard potential for reduction to pure metal.<br />
Thus, is <strong>the</strong> potential corresponding to <strong>the</strong> extraction<br />
process and does not require <strong>the</strong> simultaneous<br />
use of metal activity coefficients that are<br />
far from 1 at infinite dilution.<br />
It. should perhaps be noted that <strong>the</strong> electromotive<br />
series is <strong>the</strong>rmodynamically equivalent to o<strong>the</strong>r<br />
means of expressing <strong>the</strong> free energy of <strong>the</strong> extraction<br />
process, such as equilibrium constants or decontaminaiion<br />
factors. It is used because it permits<br />
ranking <strong>the</strong> metals in an order which djrectly<br />
indicates <strong>the</strong>ir relative ease of extraction regardless<br />
of <strong>the</strong>ir ionic valence and because it has<br />
proven useful in <strong>the</strong> experiments where a beryllium<br />
reference electrode is used to monitor <strong>the</strong> reduction<br />
process.<br />
From data previously reported <strong>the</strong> series has<br />
been constructed as shown in Table 12.2. The<br />
numbers in paren<strong>the</strong>ses after <strong>the</strong> rare earths are<br />
<strong>the</strong> potentials calculated by using <strong>the</strong> experimental<br />
C'<br />
fractional valences. For beryllium, (.- o, <strong>the</strong> potential<br />
for reduction to <strong>the</strong> pure metal, is shown. All<br />
of <strong>the</strong>se except ~e'+ are calculated relative to <strong>the</strong><br />
Lit value.<br />
Although better measurements may change <strong>the</strong>se<br />
values somewhat, <strong>the</strong>y indicate <strong>the</strong> relative ease<br />
of extraction. 'The numbers in paren<strong>the</strong>ses are<br />
probably a better approximation to <strong>the</strong> true values<br />
despite <strong>the</strong> peculiar valences. All elements up<br />
through europium can be extracted completely k-<br />
fore metallic beryllium begins to form; this forma-tion<br />
of He" represents <strong>the</strong> ultimate limit of <strong>the</strong><br />
process. An order of magnitude change in <strong>the</strong> ratio<br />
[(mole fraction in metal)/(moIa fraction in saltjl<br />
corresponds to 0.057 v for divalent and 0.058 v ior<br />
trivalent species.<br />
Table 12.2. -?; at 600°C (volts vs H2-HF : 0.00)<br />
t<br />
Li<br />
BaZ+<br />
EU 2 '-<br />
Nd3+<br />
+ SmZ<br />
ce3+<br />
La3i<br />
1.92<br />
1,81 CF o)<br />
1.79<br />
1.62 (1 61)<br />
1.58 (1,511<br />
1.58 (1.49)<br />
1.57 (1.45)<br />
1.52 (1.47)<br />
~<br />
155<br />
We have begun a reinvestigation of fission<br />
product extraction. In this study we will measure<br />
fission product distribution as a ftirlction both of<br />
lithium concentration nnd of temperature with<br />
(hopefully) improved accuracy. Preliminary results<br />
of <strong>the</strong> first of this series, using cerium, are shown<br />
in Fig. 12.5. A failure ended <strong>the</strong> experiment before<br />
good concentration data could be gotten, but those<br />
wc: did get: indicate a valence close to 3, not 2.3 as<br />
before. The apparent minimum of ?; (Ce) at 700°C<br />
is not explained arid is ra<strong>the</strong>r hard to believe. For<br />
lithium, f''; was calculated from <strong>the</strong> measured<br />
lithium concentration and <strong>the</strong> potential between <strong>the</strong><br />
bismuth pool and beryllium metal electrode, for<br />
which <strong>the</strong> temperature coefficient is known. The<br />
"MSR Program Semianri. Progr. Kept. Feh 28. 1966,<br />
<strong>ORNL</strong>-3936, p. 141.<br />
11<br />
C;. F, Haes, Jr~, Keactor Chern. Div. Atin. F'rogr.<br />
Rept. Dec. 31, 196.5, <strong>ORNL</strong>-391.3, p, 20.<br />
2.4<br />
2.0<br />
1.9<br />
i .a<br />
-<br />
><br />
-<br />
. 4.7<br />
Q<br />
4.6<br />
4.5<br />
.n,<br />
<strong>ORNL</strong>. DWG 67-14825<br />
__ . . ._<br />
7.-<br />
+.3<br />
400 500 600 700 800 900<br />
T ("GI<br />
Fig. 12.5. b:i for Lithium and Cerium.