Concentration cells with quartz membranes in molten salts: PbCl2NaCl, PbBr2NaBr, PbI2NaI systems

Sternberg, S.; Herdlicka, C.

doi:10.1016/0013-4686(68)85019-4

Cited by 2 publications

(1 citation statement)

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“…The background currents were determined by similar measurements in the absence of AgNO~. Extrapolations based on other studies yield a value of 2.7 x 10 -~ cm2/s for the diffusion coefficient of the Ag + ion in LiNO~ at 350~ (16,29). Cyclic voltammograms are shown in Fig.…”

Section: Results and Discussion O ~ -08mentioning

confidence: 90%

Reactions Involving Silver Ions and Silver Metal in Molten Nitrates

Miles¹,

McManis²,

Fletcher³

1984

J. Electrochem. Soc.

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Regarding quarternary systems, the introduction of the composition parameters y, t, and S serves in the planning of experiments and in reducing the large number of compositions to be studied in order to characterize a quarternary system adequately.Also, the use of these composition parameters makes it possible to plot thermodynamic data along well-defined composition paths and to identify the effects of competing interactions on a charge asymmetric cation. For example, the complexing effects of CsC1 or KC1 on MnCI~ become evident as the quarternary solutions become richer in CsC1, or in KC1, respectively.The successful application of Eq.[15], [16], and [17] to such nonideal charge asymmetric fused-salt solutions indicates that in quarternary, and possibly even in higher order systems, reactions within the binary solutions account for most of the internal reactivity which is responsible for deviations from ideality. Thus, the formation of a higher order system represents mixing of such prereacted binary systems and the properties of the multicomponent system should be predictable.However, it should be noted that Eq.[15], [16], and [17] are only applicable to the "acid," or higher valence, component of a charge asymmetric fused-salt mixture. ABSTRACTThe electrochemical reduction of molten LiNO3 on platinum or nickel electrodes produces insoluble LifO that passivates the cathode at high current densities. The presence of small amounts of silver ions prevents this passivation by undergoing reduction to silver metal in the form of dendritic deposits that increase the effective area of the electrode. The deposited silver is unstable in molten LiNO3 and reacts with the melt to regenerate silver ions. Corrosion studies of silver coupons gave a weight loss rate of 280 ~g h-lcm -2 in molten LiNO3 at 350~ but of only 5 ~g h-lcm -2 in KNO~ at 375~ The presence of water in the LiNO3 melt increases the corrosion rate of silver. Additions of Li20, LiNO2, LiC1, or AgNO3 to molten LiNO3 significantly decreases the corrosion rate. The addition of oxide ions to a AgNO~ containing melt produces a dark precipitate of Ag20 in NaNO~ or KNO3, but not in LiNO3. The decomposition reaction of Ag20 into its elements is kinetically slow in molten nitrates with a rate similar to that observed in air.) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 169.230.243.252 ABSTRACTThe photoelectrochemical properties of n-SiC were studied in aqueous electrolytes. The onset potential of the anodic photocurrent in steady state was found to be about 1V more anodic than that of the photocurrent measured by the lock-in method (-2V vs. SCE). This discrepancy was ascribed to the presence of transient photocurrent observed in the potential range between -1.9 and +0.6V vs. SCE. Possible mechanisms of the transient photoresponse were exam-

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Section: Results and Discussion O ~ -08mentioning

confidence: 90%