This report was prepared n an aocou.it of work sponsored by rh* United States Government. Ne-ri'*.-he United States nor the Energy Research and Dcvdopmtn-Admmistration. nor any of ffi*-r employees, nor any o* their contractors, subcontractors, or their employees, makes any warranty, express or implied,-x assumes any legal liability or responsibi'ity for the accuracy, completeness or usefulness of any information, apparatus, product or process disclosed, or represents that its use would not infringe pr-vatdy owned rights. OR NL 4866 UC 76-Molon S*lt Reactor Ttchnology Co-"*.

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NOTICE This document contains information of a preliminary nature. It is subject to revision or correction and therefore does not represent a final report.

Vol. 63 systems, with respect to the causes of this selectivity and to the nature and spacing of the supported modifying agent, should help to develop a better understanding of the actual forces involved. Solubilities of He, Ne and A were measured a t pressures from 1 to 2 atmospheres in a mixture of LiF, NaF and K F (46.5-11.542.0 mole %) a t 600, 700 and 800'. The solubilities increase linearly with gas pressure, decrease with increasing atomic weight (radius) of the solute and increase with increasing temperature. Henry's law constants in moles of solute/ (cm.3 of solution)(atmosphere) at 600' are 11.3 =k 0.7 X 10-8, 4.36 f 0.20 x 10-8 and 0.90 =k 0.04 X 10-8 and the enthalpies of solution are 8.0, 8.9 and 12.4 kcal./mole for He, Ne and A, res ectively. A model which equates the free energy of solution of the gas to the free energy of formation of holes the size orthe gas molecules in a continuous fluid having the same surface tension as the solvent yields solubility values which are in good agreement with those observed.