Kinetics and mechanism of oxidation of n-butylamine and 1,3-propanediamine by potassium ferrate

The kinetics of oxidation of n-butylamine and 1,3-propanediamine by home-made potassium ferrate(VI) at different conditions has been studied spectrophotometrically in the temperature range of 283.2-298.2 K. The results show first order dependence on potassium ferrate (VI) and on each reductant. The observed rate constant (kobs) decreases with the increase of [OH-], and the reaction rate has a negative fraction order with respect to [OH-]. A plausible mechanism is proposed and the rate equations derived from the mechanism was shown to fit all the experimental results. The rate constants of the rate-determining step and the thermodynamic activation parameters are calculated

The oxidation of 2-(2-methoxyethoxy)-ethanol and 2-(2-ethoxyethoxy)-ethanol by dihydroxydiperiodato nickelate(IV): A kinetic and mechanistic study

The kinetics of oxidation of 2-(2-methoxyethoxy)-ethanol and 2-(2-ethoxyethoxy)-ethanol by dihydroxydiperiodato nickelate(IV) (DPN) had been studied spectrophotometrically in alkaline medium in the temperature range of 293.2 to 313.2 K. The reaction rate showed first order dependence on DPN, 2-(2-methoxyethoxy)-ethanol and 2-(2-ethoxyethoxy)-ethanol. It was found that the pseudo-first-order rate constant kobs increased with an increase in concentration of OH- and a decrease in concentration of IO4-. There was a positive salt effect and no free radicals were detected. A plausible mechanism is proposed and the rate equations derived from the mechanism can explain all the experimental observations

Oxidation of triethylene glycol and tetraethylene glycol by ditelluratocuprate(III) in alkaline medium - A kinetic and mechanistic study

The kinetics of oxidation of triethylene glycol (TEG) and tetraethylene glycol (TTEG) by ditelluratocuprate(III) (DTC) in alkaline liquids were investigated spectrophotometrically in the temperature range of 20oC to 40oC. It was found that the reaction followed pseudo-first order in DTC and less than unit order in reductants. The rate constant kobs of pseudo-first order reaction decreased with an increase of [TeO42-], whereas adding [OH-] enhanced the constant. In addition, there was a negative salt effect. A suitable assumption involving pre-equilibriums before the rate controlling step and a free radical mechanism was proposed from the kinetics study. The rate equations derived from mechanism can explain all experimental phenomena. Moreover, the activation parameters at 298.2K and rate constants of the rate-determining step were evaluated

Kinetics and Mechanism of Oxidation of Diethanolamine and Triethanolamine by Potassium Ferrate

Abstract: The kinetics of oxidation of diethanolamine and triethanolamine by potassium ferrate(VI) in alkaline liquids at a constant ionic strength has been studied spectrophotometrically in the temperature range of 278.2 K-293.2 K. The reaction shows first order dependence on potassium ferrate(VI), first order dependence on each reductant, The observed rate constant (k obs ) decreases with the increase in [OH -], the reaction is negative fraction order with respect to [OH -]. A plausible mechanism is proposed and the rate equations derived from the mechanism can explain all the experimental results. The rate constants of the ratedetermining step and the thermodynamic activation parameters are calculated

Kinetics and Mechanism of Oxidation of Triethylene Glycol and Tetraethylene Glycol by Ditelluratoargentate (III) in Alkaline Medium

The kinetics of oxidation of triethylene glycol and tetraethylene glycol by ditelluratoargentate (III) (DTA) in alkaline liquids has been studied spectrophotometrically in the temperature range of 293.2 K–313.2 K. The reaction rate showed first-order dependence in DTA and fractional order with respect to triethylene glycol or tetraethylene glycol. It was found that the pseudo-first-order rate constant (kobs) increased with an increase in concentration of OH− and a decrease in concentration of H4TeO6 2−. There was a negative salt effect and no free radicals were detected. A plausible mechanism involving a two-electron transfer was proposed, and the rate equations derived from the mechanism explained all the experimental results and observations. The activation parameters along with the rate constants of the rate-determining step were calculated

Kinetics and Mechanism of Oxidation of Isobutylamine and 1,4-Butanediamine by Potassium Ferrate

The kinetics of oxidation of isobutylamine and 1,4-butanediamine by home-made potassium ferrate(VI) at different conditions has been studied spectrophotometrically in the temperature range of 288.2 -303.2 K. The results show first order dependence on potassium ferrate(VI) and on each reductant. The observed rate constant (kobs) decreases with the increase of [OH-], the reaction was negative fraction order with respect to [OH-]. A plausible mechanism was proposed and the rate equations derived from the mechanism can explain all the experimental results. The rate constants of the rate-determining step and the thermodynamic activation parameters were calculated

Kinetics and Mechanism of Oxidation of Leucine and Alanine by Ag(III) Complex in Alkaline Medium

Kinetics and mechanism of oxidation of leucine and alanine by Ag(III) complex were studied spectrophotometrically in alkaline medium at constant ion strength. The reaction was in first order with respect to Ag(III) complex and amino acids (leucine, alanine). The second-order rate constant, k−, decreased with the increasing in [OH−] and [IO4−]. A plausible mechanism was proposed from the kinetics study, and the rate equations derived from mechanism can explain all experimental phenomena. The activation parameters were calculated at 298.2 K