Cathodic Potential Limit Research Articles

Photoluminescence and Photocurrent Studies of Interfacial Defects at the InP / 1m KCl Electrolyte Junction

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A Voltammetric Investigation of AC Corrosion Phenomena at an Aluminum Electrode in Hydrochloric Acid

Abstract The electrochemical behavior of Al in HCl has been studied by cyclic voltammetry, square-wave chronoamperometry, and square-wave chronopotentiometry. High speed cyclic voltammetry was studied thoroughly, and the effects of temperature, HCl concentration, potential sweep rate, and cathodic potential limit were examined. Relevant parameters that can be determined from the cyclic voltammetric i-V curve include the breakdown and protection potentials for Al, the onset potential for hydrogen evolution, and the magnitude of the anodic and cathodic currents. The degree of passivity, which is reflected in the anodic breakdown potential and the magnitude of the anodic current, decreased with increasing solution temperature and HCl concentration, and increased with higher sweep rates. The nature of the Al passivation that occurs during the cathodic half-cycle depends on the cathodic potential limit. These processes and their relationship to the voltammetric curves are discussed in detail.

Half-wave potentials of electroactive substances in hexamethylphosphoric triamide

Abstract

Voltammetric studies in phosphorous oxychloride solutions containing lithium tetrachloroborate

The solvent reduction/oxidation in 0.1, 0.5 and 1 molar LiBCl 4−POCl 3 solutions was studied at pyrolytic graphite electrodes using the technique of cyclic voltammetry. The solvent reduction was found to occur at ∼ 2.25 V versus the lithium reference and resulted in the passivation of the pyrolytic graphite electrodes. The passivating film mainly consisted of polymeric phosphorous monoxide and lithium chloride. The cathodic potential limit in these solutions was, however, caused by the deposition of lithium metal. The anodic potential limit was caused by the formation of chlorine at ∼ 4.5 V versus the lithium reference due to the oxidation of the solvent. The chlorine formed in the anodic process was retained in the solution and could be reduced at less positive potentials (∼ 3 V versus the lithium reference).