Cyclic Voltammetry in Solutions of Aluminum Bromide and KBr in Aromatic Hydrocarbons: I . Surface Processes

Elam, M.; Gileadi, E.

doi:10.1149/1.2129310

Cited by 13 publications

(10 citation statements)

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“…This potential depends heavily on the solvent, which acts as a scavenger for the bromine molecules formed. 26 The value in Table II is that found in benzene, which reacts relatively slowly with bromine. For the / 2 couple, values in the range of 1.02-1.05 V (RA1E) were found.…”

Section: Discussionmentioning

confidence: 99%

“…The methods of purification of the electrolyte and the solvent have been described previously. 26 The electrodes were cleaned in the following manner: Sn (BDH 99.5%) in 1:1 HC1 (AR); Pb (Merck AR) in 20:1 glacial acetic acid (AR) and a 30% solution of H202 (AR); Ag (Engelhard 99.9%) and Cu (Johnson Matthey Chemicals, Grade 1) in 1:1 nitric acid (AR). All electrodes were rinsed with distilled water and dried with AR acetone.…”

Section: Methodsmentioning

confidence: 99%

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Nernst plots and formal potentials in a nonpolar solvent consisting of aluminum bromide (Al2Br6) and potassium bromide in ethylbenzene

Elam¹,

Bahatt²,

Peled³

et al. 1984

J. Phys. Chem.

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Nernst plots and formal potentials were determined for four metals (Pb, Sn, Cu, Ag). The two divalent ions (Sn, Pb) yield the expected slope of 2.3RT/2F. A maximum is observed when the concentration of the salt approaches that of free A1,Br6. This is accounted for quantitatively in terms of the various ionic species, i.e. [M(A12Br,)]+, [M(AI,Br,),]-and [M(AlBr4)]+, [M(AIBr,),]-for a divalent metal (M), which can be stable in this nonpolar solvent system. Copper is found to occur in solution only in the monovalent state, even when CuBr, is dissolved. The Nernst slope is (5/6)(2.3RT/F), which is consistent with the participation of both the positive ( [Cu2(AI2Br7)]+ or [Cu,(AIBr,)]+) and negative ([Cu(AI,Br,),]-or [Cu(AlBr,),]-) complex ions in setting the equilibrium at the interface.For silver a Nernst slope of 2.3RT/F is observed. Oxidation of lead or tin to the tetravalent state was not observed in the range of potential available up to bromine evolution. When CuBr, was dissolved, a disproportionation reaction took place, with formation of free bromine and monovalent copper, as evidenced by the appearance of the bromo derivative of the solvent. A listing of formal potentials, measured here and in earlier publications, shows that the scale of emf values is considerably compressed compared to that of aqueous solutions (from 2.75 V to 1.5

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Section: Discussionmentioning

confidence: 99%

Section: Methodsmentioning

confidence: 99%

Nernst plots and formal potentials in a nonpolar solvent consisting of aluminum bromide (Al2Br6) and potassium bromide in ethylbenzene

Elam¹,

Bahatt²,

Peled³

et al. 1984

J. Phys. Chem.

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“…The cell, electrodes, and electrochemical equipment employed for measurements of cyclic voltammograms were described in a previous publication (21). Steadystate Tafel plots were measured with the same setup, in which the function generator was replaced by a "first drop" polarographic unit (homemade), triggered by a Radiometer Type DLT-1 drop-life timer.…”

Section: Methodsmentioning

confidence: 99%

“…Some of the chemical and electrochemical properties of this system have been studied recently in our laboratory (16)(17)(18)(19)(20)(21)(22). A review of earlier work was given in Ref.…”

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The Electrochemical Oxidation of I− in a Nonpolar Solvent Consisting of Al2Br6 and KBr in an Aromatic Hydrocarbon

Elam

Gileadi

1980

J. Electrochem. Soc.

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The mechanism of oxidation of I− in a nonpolar solvent consisting of 1.0MAl2Br6 and 0.80MnormalKBr in an aromatic hydrocarbon was studied. A chemical step following charge transfer, in which I− is regenerated, was observed. It was postulated that bromination of the solvent occurred. Oxidation of Br−by I2 to normalIBr or Br2 is possible in this system since the standard potentials for different redox couples are much closer than in aqueous solutions. Qualitative mechanistic information obtained from analysis of cyclic voltammograms was consistent with the mechanism derived on the basis of steady‐state current/potential measurements. It was observed that iodine is reduced rapidly in this system if mesitylene is used as the solvent and much more slowly in benzene. The half‐wave potential for the oxidation of I− is about 1.10V vs.RAlE, compared to about 2.2V in aqueous solutions.

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Non-aqueous electrolyte solutions

Gores

Barthel

1983

Naturwissenschaften

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Cyclic Voltammetry in Solutions of Aluminum Bromide and KBr in Aromatic Hydrocarbons: I . Surface Processes

Abstract: in the SDS gel) probably extend through the S~-A. In any case, the S~-A layer represents a significant anion-depleted (cation-rich) zone just below the surface of the membrane.

Cited by 13 publications

References 4 publications

Nernst plots and formal potentials in a nonpolar solvent consisting of aluminum bromide (Al2Br6) and potassium bromide in ethylbenzene

Nernst plots and formal potentials in a nonpolar solvent consisting of aluminum bromide (Al2Br6) and potassium bromide in ethylbenzene

The Electrochemical Oxidation of I− in a Nonpolar Solvent Consisting of Al2Br6 and KBr in an Aromatic Hydrocarbon

Non-aqueous electrolyte solutions

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