ChemInform Abstract: ELECTROCHEMICAL BEHAVIOR OF ETHYLENE GLYCOL AND ITS OXIDATION PRODUCTS ON A PLATINUM ELECTRODE. III. EFFECT OF CHEMISORPTION ON THE KINETICS OF OXIDATION N OF GLYOXAL AND GLYOXALIC ACID

1979 ◽  
Vol 10 (13) ◽  
Author(s):  
G. INZELT ◽  
G. HORANYI
Keyword(s):  
Ethylene Glycol ◽  
Electrochemical Behavior ◽  
Platinum Electrode ◽  
Oxidation Products ◽  
Kinetics Of Oxidation ◽  
Glyoxalic Acid ◽  
Kinetics Of

The electrochemical behavior of flavin adenine dinucleotide in neutral solutions

1988 ◽  
Vol 66 (1) ◽  
pp. 86-96 ◽  
Author(s):  
V. I. Birss ◽  
H. Elzanowska ◽  
R. A. Turner
Keyword(s):  
Electrochemical Behavior ◽  
Electrode Surface ◽  
Flavin Adenine Dinucleotide ◽  
Cyclic Voltammetric ◽  
Kinetics Of Oxidation ◽  
Glassy Carbon Electrodes ◽  
Peak Separation ◽  
Standard Rate ◽  
Kinetics Of ◽  
Standard Rate Constant

A detailed investigation of the electrochemical behavior of flavin adenine dinucleotide (FAD) in neutral solutions has been carried out at Hg and glassy carbon electrodes. At FAD concentrations of about 10−4 M, cyclic voltammetry (CV) shows a pair of anodic and cathodic peaks having a peak separation at low sweep rates indicative of a two-electron transfer process and yielding a formal redox potential for FAD of −0.206 ± 0.003 V vs. NHE at pH 7. Evidence for FAD adsorption was obtained in experiments at high sweep rates, from the effect of time of exposure of the electrode surface to FAD in solution and from the effect of the potential limits on the cyclic voltammetric response. The process of FAD adsorption was studied in detail in dilute FAD solutions (ca 10−6 M) using a hanging mercury drop electrode and the techniques of CV and ac voltammetry. Three distinct stages of FAD adsorption were observed and a model of the orientation of FAD on the electrode surface as a function of time and potential is presented. In addition, the kinetics of oxidation and reduction of adsorbed FAD was studied for each of the stages of FAD deposition, and a surface standard rate constant of ca. 40 s−1 was obtained for Stages II and III of FAD adsorption.

Kinetics of oxidation of α-ketoglutaric acid with Ce(IV) ions in relation to Belousov-Zhabotinskii reaction

1982 ◽  
Vol 47 (11) ◽  
pp. 2831-2837 ◽  
Author(s):  
Ľudovít Treindl ◽  
Vasil Dorovský
Keyword(s):  
Redox Reaction ◽  
Platinum Electrode ◽  
Activation Parameters ◽  
Enol Form ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
Redox Catalyst ◽  
Oscillation Reaction ◽  
Belousov Zhabotinskii Reaction ◽  
Kinetics Of

Oxidation of α-ketoglutaric acid with Ce(IV) ions in a solution of sulphuric acid is a reaction of the first order with respect to both Ce(IV) ions and substrate, is acid catalysed, and its rate is proportional to the reciprocal square of the equilibrium HSO4- concentration. From the temperature dependence of the rate constant in 1.5M-H2SO4, the activation parameters were determined as ΔH##f = 57 kJ/mol and ΔS##f = -45 J mol-1 K-1. The redox reaction proper consists apparently of two steps: in the first one, the enol form of α-ketoglutaric acid reacts with Ce(IV) ions with the formation of the corresponding radical; in the second one, the latter is oxidized further with Ce(IV) to give malonic and succinic acids. Conditions are indicated under which α-ketoglutaric acid serves as substrate for the Belousov-Zhabotinskii oscillation reaction in the presence of Ce(IV)-Ce(III) redox catalyst. Oscillations of Ce(IV) and Br2 concentrations, shifted in phase, can be recorded polarographically with a rotating platinum electrode.

Gas Corrosion of Chromium-Manganese Steel in Atmospheres with Low Oxygen Partial Pressure

2013 ◽  
Vol 212 ◽  
pp. 157-162
Author(s):  
Roman Przeliorz ◽  
Jaroslaw Piątkowski
Keyword(s):  
Oxygen Partial Pressure ◽  
Partial Pressure ◽  
Oxidation Products ◽  
Manganese Steel ◽  
Low Oxygen ◽  
Kinetics Of Oxidation ◽  
Self Diffusion ◽  
Weight Growth ◽  
Steel Weight ◽  
Kinetics Of

Studies were conducted on the kinetics and mechanism of oxidation of chromium-manganese steel under partial oxygen pressure pO2from 10-11to 10-2Pa at a temperature of 1173 K. The low oxygen partial pressure was produced in a gas mixture of CO-CO2and helium containing 0.2 ppm of oxygen. The kinetics of oxidation was examined by thermogravimetry using a thermobalance made by Setaram Company. Scale growth mechanism was determined with the use of markers. The oxidation products were analyzed by scanning electron microscopy (SEM, EDS). It was found that at low partial pressure of oxygen, MnO oxide was forming on the steel surface. From an analysis of the curves of the steel weight growth per unit surface in function of time it followed that the oxidation assumed a parabolic course. A relationship has been determined between the coefficient of self-diffusion of manganese in MnO and the oxygen partial pressure.

scholarly journals Kinetics of Oxidation of Metochlopramide withChloramine-T in HClO4 Medium

2009 ◽  
Vol 6 (2) ◽  
pp. 545-552 ◽  
Author(s):  
K. M. Meenakshi ◽  
K. Vasant Kumar Pai
Keyword(s):  
Thermodynamic Parameters ◽  
Fractional Order ◽  
Reaction Rate ◽  
Oxidation Products ◽  
Perchloric Acid Solution ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
Different Temperatures ◽  
Negative Effect ◽  
Kinetics Of

The kinetics of oxidation of metochlopramide hydrochloride (MCP) with sodiumN-chlorop-toluenesulfonamide (CAT) in perchloric acid solution has been studied at 313K. The reaction rate shows a first order dependence on [CAT], fractional order on [MCP] and inverse fractional order on [H+]. There is a negative effect of dielectric constant of the solvent. The addition of the reduction product of CAT has no significant effect on the rate. The rate remained unchanged with the variation in the ionic strength of the medium. The reaction fails to induce the polymerization of acrylonitrile. Thermodynamic parameters have been computed by Arrhenius plot. The stoichiometry of the reaction was found to be 1:2 and oxidation products were identified. The Michaelis-Menten type of kinetics has been proposed. CH3C6H4SO2NHCl have been assumed to be the reactive oxidizing species. Thermodynamic parameters were computed by studying reactions at different temperatures. A mechanism consistent with observed kinetics is proposed.

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