Abstract

The kinetics of oxidation of 2-amino-1-Butanol and 3-Amino-1-propanol by potassium ferrate(VI) in alkaline
liquids at a constant ionic strength has been studied spectrophotometrically in the temperature range of 293.2
K-313.2 K. The reaction shows first order dependence on potassium ferrate(VI), first order dependence on each
reductant. The observed rate constant (kobs) 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 rate-determining step and the
activation parameters are calculated.

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