The kinetics of oxidation of l-methoxy-2-propanol and 1-ethoxy-2-propanol by ditelluratocuprate(Ⅲ) (DTC) in alkaline liquids has been studied spectrophotometrically in the temperature range of 293.2-313.2 K. The reaction rate showed first order dependence in DTC and fractional order with respect to 1-methoxy-2-propanol or 1-ethoxy-2-propanol. 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 TeO24-. There is a negative salt effect. A plausible mechanism involving a pre-equilibrium of a adduct formation between the complex and l-methoxy-2-propanol or l-ethoxy-2-propanol was proposed. The rate equations derived from mechanism can explain all experimental observations. The activation parameters along with the rate constants of the rate-determining step were calculated.
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