Erratum: Molten Salts Data: Diffusion Coefficients in Single and Multi-Component Salt Systems [J. Phys. Chem. Ref. Data <b>1</b>
                  <b>1</b>, 505 (1982)]

Janz, George J.; Bansal, Narottam P.

doi:10.1063/1.555704

Cited by 90 publications

(177 citation statements)

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“…So D decreases and AU increases with in creasing ionicity of the diffusing species. These re sults agree well with numerous data on the influence of oxidation state of central atoms on diffusion coef ficients and activation energies for diffusion of com plexes [25]. The decrease in D is related to the in creased strength of the complexes, and this in turn leads to a decrease in the contribution to the diffu sion coefficient from the "hopping" mechanism as discussed in [26].…”

Section: Electrochemistry Of the Redox Process Eu(iii) + E~ O Eu(ii)supporting

confidence: 79%

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Electrochemical and Thermodynamic Properties of EuCl₃ and EuCl₂ in an Equimolar NaCl-KCl Melt

Kuznetsov

Rycerz

Gaune‐Escard

2001

Zeitschrift Für Naturforschung A

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Section: Electrochemistry Of the Redox Process Eu(iii) + E~ O Eu(ii)supporting

confidence: 79%

“…The changes in the partial Gibbs energies for the formation of europium chlorides from the elements in NaCl-KCl were calculated using (23) and (25). For the formation of europium chlorides in molten NaClKCl, the following changes were obtained:…”

Section: Comparison Between the Present Results And Calorimetric Datamentioning

confidence: 99%

Electrochemical and Thermodynamic Properties of EuCl₃ and EuCl₂ in an Equimolar NaCl-KCl Melt

Kuznetsov

Rycerz

Gaune‐Escard

2001

Zeitschrift Für Naturforschung A

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“…The result is facile charge transfer at the electrodeelectrolyte interface 12 and rapid mass transport to and from the electrode-electrolyte interface. 13,14 These features combined with low ohmic losses enabled by the high electrical conductivity of the molten salt electrolytes (up to 3 S cm −1 ) enable the battery to be driven at high charge/discharge rates with small overvoltage. In order to evaluate the kinetics of the alloying and dealloying processes, the potential of the WE, E, was measured at current densities of 50, 100, 200, 300, and 500 mA cm −2 at 650…”

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confidence: 99%

Calcium-Antimony Alloys as Electrodes for Liquid Metal Batteries

Ouchi

Kim

Ning

et al. 2014

J. Electrochem. Soc.

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The performance of a calcium-antimony (Ca-Sb) alloy serving as the positive electrode in a Ca Sb liquid metal battery was investigated in an electrochemical cell, Ca(in Bi) | LiCl-NaCl-CaCl 2 | Ca(in Sb). The equilibrium potential of the Ca-Sb electrode was found to lie on the interval, 1.2-0.95 V versus Ca, in good agreement with electromotive force (emf) measurements in the literature. During both alloying and dealloying of Ca at the Sb electrode, the charge transfer and mass transport at the interface are facile enough that the electrode potential varies linearly from 0.95 to 0.75 V vs Ca(s) as current density varies from 50 to 500 mA cm −2 . The discharge capacity of the Ca Sb cells increases as the operating temperature increases due to the higher solubility and diffusivity of Ca in Sb. The cell was successfully cycled with high coulombic efficiency (∼100%) and small fade rate (<0.01% cycle −1 ). These data combined with the favorable costs of these metals and salts make the Ca Sb liquid metal battery attractive for grid-scale energy storage. The liquid metal battery (LMB) has been shown to be an attractive potential solution to the problem of grid-level storage.1,2 The LMB comprises two liquid metal electrodes separated by a molten salt electrolyte that self-segregate into three liquid layers according to density and immiscibility. In the search for even lower-cost chemistries based on this formula, the Ca-Sb system became the focus of attention because Ca, thanks to its ubiquitous abundance, 3 offers high performance at a low price point. Previous measurements in this laboratory of the thermodynamics of liquid Ca-Sb alloys 4 revealed this system to be high-voltage (0.94-1.04 V) and low-cost (69 $ kWh −1 ). However, Ca is highly soluble in its salts 5 conferring such a high level of electronic conductivity that a battery fitted with a liquid Ca electrode would exhibit an unacceptably high self-discharge current. In this study we show how to suppress the Ca metal solubility in the molten salt electrolyte so as to make practical a Ca-Sb LMB.The literature indicates that the solubility of calcium metal is significantly reduced by alloying calcium with other metals to decrease its activity (a Ca ).5 Following this, one can envisage a Ca-Sb liquid metal battery as:where A is the negative electrode host and the electrolyte can be a solution of molten halide salts with calcium cation as the itinerant. The alloying of calcium with a more noble A metal such as magnesium desirably decreases the melting temperature of the negative electrode, reduces the reactivity of pure calcium metal, and decreases the solubility of calcium in the molten salt electrolyte while undesirably decreasing the cell voltage, 6 albeit an acceptably small amount. For the cell with Mg as the negative electrode host and Sb as the positive electrode, the half-cell reactions are negative : Ca(in Mg) = Ca 2+ + 2epositive : Ca 2+ + 2e − = Ca(in Sb) [3] and the resulting overall cell reaction is cell : Ca(in Mg) = Ca(in Sb).[4]On discharge, calcium...

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“…The inner surface of the furnace tube was coated by a very thin gold film in order to reflect the infrared light and thus achieve a uniform temperature distribution. The U-shaped conductivity cell made of transparent fused silica was calibrated before each run with pure NaCl melt [13]. Two conductivity cells were used with cell constants of about 141 and 231 cm-1.…”

Section: Methodsmentioning

confidence: 99%

Electrical Conductivity of Molten LaCl₃-NaCl, LaCl₃-KCl, and LaCl₃-CaCl₂

Fukushima

Iwadate

Andou

et al. 1991

Zeitschrift Für Naturforschung A

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The electrical conductivities (x's) of molten LaCl3-NaCl, LaCl3-KCl, and LaCl3-CaCl2 were measured at 893-1168 K, by a conventional ac technique and fitted by quadratic functions of temperature. They increase with increasing temperature and decrease with increasing mole fraction of LaCl3. The equivalent conductivities (A's) follow a linear relationship of In A vs. 1/T The A's of LaCl3-NaCl and LaCl3-KCl decrease drastically with increasing LaCl3 concentration. A of molten LaCl3 is smaller than that of molten CaCl2, in which the octahedral complex anion CaClg" is known to exist. It seems reasonable to assume that complex ions or cluster species such as LaCl^-and La2Cli!~ exist in molten LaCl3 and its mixture melts. Similar results, reported in a previous paper, were obtained for PrCl3-NaCl, PrCl3-KCl, and PrCl3-CaCl2.

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Erratum: Molten Salts Data: Diffusion Coefficients in Single and Multi-Component Salt Systems [J. Phys. Chem. Ref. Data 1 1, 505 (1982)]

Cited by 90 publications

References 0 publications

Electrochemical and Thermodynamic Properties of EuCl₃ and EuCl₂ in an Equimolar NaCl-KCl Melt

Electrochemical and Thermodynamic Properties of EuCl₃ and EuCl₂ in an Equimolar NaCl-KCl Melt

Calcium-Antimony Alloys as Electrodes for Liquid Metal Batteries

Electrical Conductivity of Molten LaCl₃-NaCl, LaCl₃-KCl, and LaCl₃-CaCl₂

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Erratum: Molten Salts Data: Diffusion Coefficients in Single and Multi-Component Salt Systems [J. Phys. Chem. Ref. Data 1 1, 505 (1982)]

Cited by 90 publications

References 0 publications

Electrochemical and Thermodynamic Properties of EuCl3 and EuCl2 in an Equimolar NaCl-KCl Melt

Electrochemical and Thermodynamic Properties of EuCl3 and EuCl2 in an Equimolar NaCl-KCl Melt

Calcium-Antimony Alloys as Electrodes for Liquid Metal Batteries

Electrical Conductivity of Molten LaCl3-NaCl, LaCl3-KCl, and LaCl3-CaCl2

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Electrochemical and Thermodynamic Properties of EuCl₃ and EuCl₂ in an Equimolar NaCl-KCl Melt

Electrochemical and Thermodynamic Properties of EuCl₃ and EuCl₂ in an Equimolar NaCl-KCl Melt

Electrical Conductivity of Molten LaCl₃-NaCl, LaCl₃-KCl, and LaCl₃-CaCl₂