Solubility of helium and argon in liquid sodium

Veleckis, E.; Dhar, S.K.; Cafasso, F.A.; Feder, H.M.

doi:10.1021/j100687a021

Cited by 24 publications

(9 citation statements)

References 6 publications

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“…For gases which are ideal over the measured range, both units are independent of pressure. Their thermodynamic significance has been discussed elsewhere (10,11).…”

Section: Resultsmentioning

confidence: 99%

Solubility of xenon in liquid sodium

Veleckis¹,

Cafasso²,

Feder³

1976

J. Chem. Eng. Data

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The solubility of xenon In liquid sodium was measured as a function of pressure (2-8 atm) and temperature (350-600°C). Henry's law was obeyed with the value of the Henry's law constant, KH = %,/P, ranging from 1.38 X atm-' at 600°C, where be and Pare the atom fraction and the partial pressure of xenon, respectively. The temperature dependence of solubility may be represented by loglo = (0.663 f 0.01) -(4500 f 73) T1, where X Is the Oslwald coefficient (the volume of xenon dissolved per unit volume of sodium at the temperature of the experiment). The heat of solution of xenon In sodium was 20.6 f 0.7 kcal/mol, where the standard state of xenon is defined as that of 1 mol of an ideal gas, confined to a volume equal to the molar volume of sodium.atm-I at 350°C to 1.59 X The solubility of noble gases in liquid sodium is of considerable interest because of the use of sodium as a coolant in nuclear fission reactors. Helium and argon are frequently used as sodium blanketing gases, and krypton and xenon are fission product gases which may be released to sodium from the fuel-pins. The solubilities of helium and argon in liquid sodium have been reported (9, 70), and that of krypton has been determined ( 7 ) . Measurement of the solubility of xenon was undertaken to provide data necessary for the evaluation of the consequences of fuel-pin cladding failure. ExperimentalReference 70 describes the details of the method used for the determination of the trace solubilities of gases in liquid metals and shows a schematic diagram of the solubility apparatus. In the present application, the procedure was as follows. Approximately 2500 cm3 of liquid sodium contained in a large vessel (saturator) was saturated with natural xenon at a preselected temperature and pressure by circulating the gas through the liquid via a coiled, perforated tube placed near the bottom of the saturator. A measured amount (-1500 cm3) of the saturated sodium was then transferred to another vessel (stripper) via a heated, valved Y4-in. sodium-transfer line which interconnected the bottom plates of the vessels. The volume of sodium transferred was calculated from the known geometry of the stripper and the liquid levels of sodium before and after transfer. The levels were measured with a Mine Safety Appliances Corp. liquid level probe operating on the capacitance principle.In the stripper the dissolved gas was separated from sodium by sparging with helium, which was introduced through an immersed 1 0-cm stainless-steel dispersion disc (Micrometallic Corp., 5-pm mean pore size). The resulting xenon-helium mixture was then slowly exhausted through a 6-mm X 8-cm column of activated silica gel cooled to -196OC, on which the xenon was adsorbed while most of the helium passed through unadsorbed. The gel was then heated at 3OO0C and the desorbed gas, now enriched in xenon, was analyzed for xenon with a Beckman GC-5 gas chromatograph used in conjunction with an electron capture detector.' To whom correspondence should be addressed.In this procedure the following precau...

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“…For gases which are ideal over the measured range, both units are independent of pressure. Their thermodynamic significance has been discussed elsewhere (10,11).…”

Section: Resultsmentioning

confidence: 99%

Solubility of xenon in liquid sodium

Veleckis¹,

Cafasso²,

Feder³

1976

J. Chem. Eng. Data

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“…The helium solubility in liquid sodium is known (Veleckis et al 1971) so it might be supposed that this is the best available test for the pseudopotential. Unfortunately, the very low electron density in sodium (r, = 4) means that E , is no longer substantially larger than other contributions to the heat of solution.…”

Section: J Sterensonmentioning

confidence: 99%

Factorization theory for single-valued analytic functions on compact Riemann surfaces with boundary

Khavinson¹

1989

Russ. Math. Surv.

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In the low-pressure limit. a helium atom embedded in the electron gas appropriate to metallic hydrogen is only weakly perturbed from its free space structure, and its interaction with the electron gas can be represented by an energy-dependent pseudopotential. A calculation is made for the Gibbs energ) of mixing for H-He. using an Austin pseudopotential and a fluid state model based on hard-sphere structure factors. A large orthogonalisation hole is predicted. which ma) crudely represent the gradual transition from a helium atom to a screened x-particle as the electron densitj increases. The helium solubilit? is predominantly determined by the structure-independent interaction of the electron gas with the repulsive pseudopotential. and is probably leust at the lowest pressures. In the hydrogen-helium planets (Jupiter. Saturn) the helium concentration may be at or close to saturation at the molecular-metallic hydrogen transition. 0305-4608,'79/050791 + 11 $01.00

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“…It contributes to a better understanding of the interaction of neutral He with the itinerant electronic states in dense degenerated plasma existing in the metal. Experimental solubility values of He in liquid metals Na, (16) Li, (17) and K (17) at low gas pressures are small and they increase with temperature, showing large positive enthalpies of dissolution. The endothermic dissolution process of a He atom in a fluid metal has been interpreted as resulting from the strong repulsive interaction existing between He and the conduction electrons in the metals, based on a quantum-mechanical calculation for the systems He-Al and He-Mg, (18) and molecular dynamics techniques for the system He-Ni.…”

Section: Introductionmentioning

confidence: 99%