The Electrochemical Behavior of Aluminum

Petrocelli, J. V.

doi:10.1149/1.2777957

Cited by 23 publications

(21 citation statements)

References 6 publications

(6 reference statements)

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“…Reduction of cobalt(III) by aluminium is favoured by thermodynamics, but aluminium is more prone to side reactions such as reduction of water and protons, both causing formation of hydrogen gas. 8,10,61,70,71 This was evidenced by formation of plenty of gas bubbles and a pressure build-up in the leaching vials, but the gas could not be identified. Joulié et al reported that a 750% excess of aluminium metal is required to reduce cobalt (III) efficiently during leaching of LIB cathode materials by sulphuric acid.…”

Section: Effect Of Current Collector Metals On Leachingmentioning

confidence: 99%

Solvometallurgical recovery of cobalt from lithium-ion battery cathode materials using deep-eutectic solvents

2020

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Section: Effect Of Current Collector Metals On Leachingmentioning

confidence: 99%

Solvometallurgical recovery of cobalt from lithium-ion battery cathode materials using deep-eutectic solvents

2020

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“…On exposure of a stainless steel surface to chloride solutions there probably is preferential adsorption (especially at grain boundaries) of chloride ions, which tends to exclude adsorption of film healing oxygen, as in the case of platinum surfaces (30). At certain imperfections in the protective film, occurring p~imarily at grain boundaries, cations from the metal can diffuse through the fihn more readily than at other points (45,46). This diffusion process may also be accelerated if chloride ions become imbedded in the lattice of the protective fihn; these chloride ions would then prevent the formation of protective oxides (47).…”

Section: Summary and Disc~yssionmentioning

confidence: 99%

Pitting Corrosion of 18Cr-8Ni Stainless Steel

Streicher

1956

J. Electrochem. Soc.

187

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I. Factors controlling pitting corrosion and laboratory methods used for its study are reviewed. An electrolytically accelerated test was developed for investigation of pit initiation. A controlled direct current was passed through a cell whose anode was the stainless steel specimen and whose electrolyte was the pitting solution. The number of pits formed depended on the current density, the steel specimen (composition and surface treatment), and the solution (composition and temperature).II. The accelerated electrolytic pitting method described in Part I was used to determine the influence of alloying elements added to 18Cr-8Ni stainless steel on pit initiation in sodium chloride and bromide solutions. Reduction in carbon content, increase in nitrogen content of these steels, and alloying additions of molybdenum and silicon increased resistance to pit initiation. Grain boundaries, rather than nonmetallic inclusions, were primary sites of pit initiation during simple immersion or in the electrolytically accelerated ~est. I. Development of an Accelerated Pit Initiation MethodPITTING CORROSION OF STAINLESS STEEL

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“…In order for this superposition approach to function it is necessary that the rate and kinetics of each partial reaction be independent of the other partial reaction(s) at a given potential. This independence of partial processes has been shown for several combinations of reductant (metals or hydrogen) and oxidant (5)(6)(7)(8)(9), and consequently would appear to be quite general. However, independence of the partial processes is not a necessary criteria for charge and mass balance across the electrode-solution interface, as suggested in some previous work (10,12).…”

mentioning

confidence: 73%

“…Each time ii occurs, the resultant Cdad + ion is removed by step [2] or [3]. Therefore illF = i#F + R~ [8] from which Eq. [6] becomes…”

Section: Model To Explain Resltsmentioning

confidence: 99%

Effects of Oxygen on the Mechanism of Cadmium Dissolution in Sulfate Solutions

Andersen

Ghandehari

Feng

et al. 1977

J. Electrochem. Soc.

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The dissolution rate of cadmium was measured in various nitrogen-and oxygen-saturated acidic sulfate solutions under potentiostatic conditions. At a given potential, the aissolution rate was found to be greater in O2-than in N2-saturated solutions. A dissolution mechanism is proposed which explains this phenomena as well as results from tests in which potential, solution agitation, and solution composition were varied. According to this mechanism Cd + ions are formed as intermediates and are then oxidized to the product Cd +2 ions by a chemical path involving O2 as well as by the conventional electrochemical path.Uniform corrosion of a metal in solution is most frequently explained in terms of the electrochemical polarization curves for the independent processes, i.e., metal oxidation and H + or 02 reduction [e.g., see Ref.(1-4)]. The polarization curves for the part reactions are added to yield that for the over-all system. This type of treatment is useful in explaining corrosion, passivation, and protection phenomena. It also has been recommended as a means for accelerated corrosion testing [e.g., Ref. (2,5)]. In the latter application the Tafel curves for one or both half-reactions (assuming one predominant cathodic and one predominant anodic reaction) are obtained by suppressing the opposite reaction. The Tafel curve is then extrapolated to the measured corrosion (mixed) potential or the two Tafel curves are extrapolated to the point of overlap to yield the corrosion current. The above superposition procedures are a means of replacing lengthy weight-loss or assay-dependent tests with one rapid electrochemical test. In order for this superposition approach to function it is necessary that the rate and kinetics of each partial reaction be independent of the other partial reaction(s) at a given potential. This independence of partial processes has been shown for several combinations of reductant (metals or hydrogen) and oxidant (5-9), and consequently would appear to be quite general. However, independence of the partial processes is not a necessary criteria for charge and mass balance across the electrode-solution interface, as suggested in some previous work (10, 12). Also an experimental attempt to obtain the corrosion rate of copper in oxygenated acid sulfate solutions by extrapolating the anodic copper polarization curve gave a corrosion rate which was erroneously low (11). ~ In the latter work (11) studies were made to determine why the partial processes were not independent when coupled, and a mechanism was proposed to explain the results.The present study was made to investigate other systems for which the partial processes are not independent, as part of an evaluation of the superposition means of accelerated corrosion testing. Cadmium in acidic sulfate solutions was the metal chosen for study because previous work (13) suggests it dissolves as Cd +2 ions via a Cd +1 intermediate; such an intermediate offers a vehicle for interactions between the part reactions. Both H + ions and O2 were studied as oxid...

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The Electrochemical Behavior of Aluminum

Cited by 23 publications

References 6 publications

Solvometallurgical recovery of cobalt from lithium-ion battery cathode materials using deep-eutectic solvents

Solvometallurgical recovery of cobalt from lithium-ion battery cathode materials using deep-eutectic solvents

Pitting Corrosion of 18Cr-8Ni Stainless Steel

Effects of Oxygen on the Mechanism of Cadmium Dissolution in Sulfate Solutions

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