ChemInform Abstract: ELECTRODE REACTIONS AT EXTREMELY NEGATIVE POTENTIALS. PART I. THE KINETICS OF F THE EUROPIUM(II)/EUROPIUM(MERCURY) ELECTRODE REACTION IN DMF AND DMF + WATER MIXTURES

1985 ◽  
Vol 16 (50) ◽  
Author(s):  
J. CHLISTUNOFF ◽  
Z. GALUS
Keyword(s):  
Mercury Electrode ◽  
Electrode Reaction ◽  
Electrode Reactions ◽  
Kinetics Of

The Kinetics of Electrode Reactions on Metallic Bismuth in Pure Molten Bismuth Chloride

1992 ◽  
Vol 57 (5) ◽  
pp. 1015-1022
Author(s):  
Adolf Kisza ◽  
Jerzy Każmierczak
Keyword(s):  
Activation Parameters ◽  
Electrode Reaction ◽  
Molten Chlorides ◽  
Electrode Reactions ◽  
Metallic Bismuth ◽  
Kinetics Of ◽  
Bismuth Chloride

The relaxation and impendance methods were applied to the study of electrode reaction on bismuth electrode immersed in pure molten bismuth chloride. The found kinetic and activation parameters are compared with the similar ones for other pure molten chlorides.

The Effects of Adsorbed Ions on Simple Electrode Reactions. II. The Reduction Of Chromium(III) Ion in The Presence of TolueneP-Sulfonate Anions

1974 ◽  
Vol 52 (18) ◽  
pp. 3165-3169 ◽  
Author(s):  
Kamaruzzaman Alias ◽  
W. Ronald Fawcett
Keyword(s):  
Double Layer ◽  
Mercury Electrode ◽  
Diffuse Layer ◽  
Reaction Site ◽  
Electrode Reactions ◽  
Reaction Acceleration ◽  
Kinetics Of ◽  
Outer Helmholtz Plane

The kinetics of electroreduction of Cr3+ ion have been studied at a mercury electrode both in the absence and in the presence of chemisorbed toluene p-sulfonate ions. The rate of the reaction was considerably accelerated in the presence of the chemisorbed anions. Analysis of the data has shown that the reaction acceleration can be accounted for on the basis of Frumkin's theory for double layer effects suggesting that the reaction site is at the outer Helmholtz plane or close to it in the diffuse layer.

scholarly journals The kinetics of electrode reactions. I and II

1938 ◽  
Vol 169 (937) ◽  
pp. 206-234 ◽  
Keyword(s):  
Electrode Potential ◽  
Surface Reaction ◽  
Reference Electrode ◽  
Electrode Reaction ◽  
Potential Difference ◽  
Concentration Difference ◽  
Electrode Processes ◽  
Electrode Reactions ◽  
Concentration Changes ◽  
Kinetics Of

In any surface reaction taking place in a Solution, it is clear that the concentration of the reactants in the vicinity of the surface must fall. If the concentration in the bulk of the solution remains constant, a steady state may finally be reached, in which the rate of replenishment of the solution in this region, from the bulk, is equal to the rate at which the reactant in question is used up. But, in general, such a state is only attained when the concentration at the surface is less than that in the rest of the solution. If the reaction considered is an electrode reaction, these concentration changes may affect the electrode potential. This question is therefore of importance in the study of overpotential, and of the kinetics of electrode processes generally. The overpotential at an electrode is defined as the potential difference between this electrode and a similar unpolarized reversible electrode in the same solution. In practice this reference electrode is usually situated outside the region affected by the concentration changes near the electrode at which the reaction is taking place. The measured potential difference between the two electrodes, i.e. the measured overpotential, may therefore include a term due to the concentration difference.

Electrode kinetics of the system V(III)/V(II) in aqueous dimethylsulphoxide

1991 ◽  
Vol 56 (1) ◽  
pp. 90-95 ◽  
Author(s):  
Libuše Kišová ◽  
Libor Reichstädter ◽  
Jaro Komenda
Keyword(s):  
Organic Solvent ◽  
Double Layer ◽  
Rate Constants ◽  
Electrode Surface ◽  
Reaction Rate ◽  
Mercury Electrode ◽  
Electrode Reaction ◽  
Electrode Kinetics ◽  
Kinetics Of ◽  
Lower Basicity

The rate constants for the reduction of V(III) and oxidation of V(II) were measured on a mercury electrode in water and water-dimethylsulphoxide mixtures. Their dependance on the concentration of DMSO differs from that in mixtures of water with an organic solvent of lower basicity. This can be attributed to the existence of different solvates of vanadium in solutions and to different values of the rate constant for these solvates on the electrode surface at different coverages with the organic component. The influence of DMSO both in the primary solvation sphere and in the electrode double layer on the electrode reaction rate is discussed.

Kinetics of electrode reaction of Eu3+/Eu2+ studied by cyclic voltammetry and tast polarography

1990 ◽  
Vol 55 (7) ◽  
pp. 1666-1672 ◽  
Author(s):  
Jaroslav Němec ◽  
Tomáš Loučka
Keyword(s):  
Cyclic Voltammetry ◽  
Kinetic Parameters ◽  
Electrochemical Behaviour ◽  
Mercury Electrode ◽  
Electrode Reaction ◽  
Dropping Mercury Electrode ◽  
Sulphate Media ◽  
First Time ◽  
Kinetics Of ◽  
The Eu

The electrochemical behaviour of europium at the dropping mercury electrode was studied in the medium of 1M-NaClO4, 1M-NaCl, 1M-NaNO3, and 1M-Na2SO4. The curves obtained by Tast polarography and the kinetic parameters (ks, α) for the Eu3+/Eu2+ system in the medium of perchlorate and chloride solutions are in accord with the results published earlier. The kinetic parameters in nitrate and sulphate media are given for the first time. In the medium of nitrates, the electrode reaction is probably accompanied by a chemical reaction.

Isopotential points in square-wave voltammetry of reversible electrode reactions

2009 ◽  
Vol 74 (10) ◽  
pp. 1489-1501 ◽  
Author(s):  
Marina Zelić ◽  
Milivoj Lovrić
Keyword(s):  
Square Wave Voltammetry ◽  
Electrode Reaction ◽  
Time Model ◽  
Model Calculations ◽  
Square Wave ◽  
Electrode Reactions ◽  
Wave Voltammetry ◽  
Electron Transfer Processes ◽  
Diagnostic Criterion ◽  
First Time

Isopotential points in square-wave voltammetry are described for the first time. Model calculations and real measurements (performed with UO22+ and Eu3+ in perchlorate and bromide solutions, respectively) indicate that such an intersection could be observed when backward components of the net response, resulting from an increase in frequency or reactant concentration, are presented together. The electrode reaction should be fully reversible because quasireversible or slower electron transfer processes give the isopoints only at increasing reactant concentrations but not at increasing square-wave frequencies. The effect could be used as an additional diagnostic criterion for recognition of reversible electrode reactions where products remain dissolved in the electrolyte solution.

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