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Liquid Metal Batteries: Past, Present, and Future

“…Experimental measurements of enthalpies of reaction, electromotive force, vapor pressure, and chemical equilibrium have been made to determine the thermodynamic activities of most binary alloys as a function of mole fraction and temperature [ a A = f ( x A , T )] and are readily available in the literature. ,,− These data can be used to calculate the theoretical cell discharge profile of an electrode couple; however, a detailed comparison of the multitude of possible liquid metal battery electrode couples is impractical due to the wide variety of phase behavior exhibited in binary alloy systems. To address this issue, an imprecise, but effective method for estimating cell voltages for binary alloy electrode couples is constructed here.…”

Thermodynamic Properties of Solid Binary Antimonides

“…The only direct Δ H ° measurement is that of Morozova et al for K 3 Sb (−298.7 kJ/mol at 298 K), using acid-solution calorimetry. Gibbs-energy measurements have been performed by the same groups that studied the Na–Sb system, including vapor-pressure measurements by Voronin and co-workers (459–679 K), , polarographic studies by Morachevskii and co-workers (Sb cathode, 513 and 600 K), , and EMF measurements by Borodkina (K electrode, 490 K; quoted by Morachevskii and Bochagina) . Table compares Δ G ° 513 for potassium antimonides from the three investigations.…”

“…A more accurate experimental determination of ΔH°would also be desirable. Four stable compounds are currently thought to exist in the Ca−Sb system (Figure 4): 139 CaSb 2 , Ca 11 Sb 10 , Ca 5 Sb 3 , and Ca 2 Sb. This is controversial, since previous phase diagrams showed a much different system, with compounds CaSb, CaSb 3 , and Ca 3 Sb 2 .…”

Thermodynamic modeling of the Ca–In and Ca–Sb systems supported with first-principles calculations

“…It can be seen that the calculated enthalpies of formation using the presently obtained parameters can well reproduce the experimental data [18] at 805°C. The very negative enthalpies of formation indicate that the short-range ordering, which has already been demonstrated by [20,24,40,41], exists in the melts. However, there is a deviation between the results of first-principles calculations and the experimental data.…”