In chemical kinetics, the rate and mechanism of a chemical reaction is to determine the overall stoichiometry of the reaction and to identify any side‐reaction. This study involves the determination of the effect of changes in the concentrations of reactant and product species. One reason for studying the rates of the reaction is to predict how quickly a reaction mixture approaches equilibrium. Another is that the study of reaction rates leads to an understanding of the mechanism of a reaction and analysis into a sequence of elementary steps. The kinetics study on oxidation of benzaldehyde and p-nitro benzaldehyde has been investigated at 313 K by isoquinolinium bromochromate in aqueous acetic acid medium. The reaction is first order with respect to [IQBC], [substrate] and [H+]. The benzoic acid was identified as end - product by existing standard methods. The stoichiometric determination confirms 3:1 mole ratio of substrates - IQBC system. Activation parameters were evaluated and suitable mechanism was proposed. The rate law in consistent with the observed kinetic results have been discussed. This work can better and suitably be utilized in drugs and pharmaceutical industries and also in soft drink or cold drink industries.
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