Chemical potential interaction parameters in charge-unsymmetric mixtures of molten salts

Braunstein, J.; Romberger, K. A.; Ezell, Ryan G.

doi:10.1021/j100719a015

Cited by 5 publications

(3 citation statements)

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Section: --4rt Ln< 1-2nmentioning

confidence: 99%

“…Whether or not any such cells would display voltages as high as those encountered with aluminum remains to be seen. There is at least one possibility already in the literature; beryllium concentration cells utilizing molten BeF2-LiF electrolytes have been reported to yield potentials greater than 0.22V(23).Curve matching was done by overlaying curves plotted by a Hewlett-Packard 9100B programmable calculator and plotter. All other data reduction was done with the aid of a Wang 720B programmable calculator.…”

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Chloroaluminate Equilibria in AlCl[sub 3]-NaCl Melts

Fannin

King

Seegmiller

1972

J. Electrochem. Soc.

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Equilibrium constants were calculated for reactions governing the species present at 175°C in molten mixtures of aluminum chloride and sodium chloride. The equilibria postulated pertain to formation of the complex ions AlCl4− , Al2Cl7− , and Al3Cl10− from Cl− , AlCl3 , and Al2Cl6 . The constants were derived from potentials exhibited by concentration cells of the type normalAl/AlCl3false(Nfalse) , normalNaCl//AlCl3false(N′false) , normalNaCl/normalAl , and from vapor pressures over pure AlCl3 and molten AlCl3‐normalNaCl mixtures. Measurements were made throughout the concentration range N=0.498–0.71 . The possibilities of using these concentration cells as high energy density batteries are considered.

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Section: --4rt Ln< 1-2nmentioning

confidence: 99%

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confidence: 99%

Chloroaluminate Equilibria in AlCl[sub 3]-NaCl Melts

Fannin

King

Seegmiller

1972

J. Electrochem. Soc.

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“…( Atff(AMgF3) (9) Using the data given in Table V and neglecting the slight temperature dependence of the various enthalpy terms, we obtain Aíí1(NaMgF3(s)) = -2.9 kcal mol'1 and AHr (KMgF3(s)) = -5.4 kcal mol"1. These enthalpies apply near 1300 K (NaMgF3) and near 1130 K (KMgF3).…”

Section: Discussionmentioning

confidence: 99%

Thermochemistry of the liquid mixtures of the alkaline earth fluorides with alkali fluorides

Hong¹,

Kleppa²

1978

J. Phys. Chem.

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The liquid mixtures of MgF2, SrF2, and BaF2 with LiF, NaF, and KF have been studied by solid-liquid mixing calorimetry at 1081 °C, The experiments cover concentrations up to 50-60 mol % alkaline earth fluoride, and allow a reliable determination of the liquid-liquid enthalpies of mixing and of the interaction parameters = AHM/NlN2 at this temperature. The results are compared with data previously reported for the corresponding mixtures of CaF2 and BeF2, and with enthalpy data for other alkaline earth halide-alkali halide mixtures. The new results show noticeable deviations from the linear dependence of on the size parameter 12 = (dx -d2)/d1d2predicted by conformal solution theory. The deviations are particularly significant for LiF-SrF2 and LiF-BaF2, and in these two systems may be related to specific structural factors. For the mixtures of MgF2, CaF2, SrF2, and BaF2 we demonstrate an empirical linear relation between and the relative ionic potential of the two cations, = |(Zi/fi) -(Z2/r2)|. (Z, is the charge of the ion with radius r¡.) Similar relations are found to exist for other alkaline earth halide-alkali halide mixtures and even for the binary alkali fluorides.

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EMF Measurements in Molten Salts*

Braunstein

1968

Experimental Thermodynamics Volume II

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Chemical potential interaction parameters in charge-unsymmetric mixtures of molten salts

Cited by 5 publications

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Chloroaluminate Equilibria in AlCl[sub 3]-NaCl Melts

Chloroaluminate Equilibria in AlCl[sub 3]-NaCl Melts

Thermochemistry of the liquid mixtures of the alkaline earth fluorides with alkali fluorides

EMF Measurements in Molten Salts*

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