Abstract

Sayyed Hossein Rasa and Mohammad Taha Badri

DOI : http://dx.doi.org/10.13005/ojc/350142

This research paper aims to determine of the rate equation for the reaction that is described in this article. Experiments carried out by using iodometric method for determine the concentration of potassium permanganate at different times. The results are very similar to the results of the UV-Visible spectrophotometric method. These results showed that order of reaction for acetone, potassium permanganate and sulfuric acid were 1, 1 and 1, respectively. Therefore, the rate equation is according to the chemical equation. In addition, it was demonstrated that there was no relationship between products concentration and rate of reaction. A suitable mechanism is also suggested. Thus, the reaction rate law implies a complicated reaction mechanism with low acetone concentrations. In addition, elevated temperature and reactants concentrations are required for a fast acetone oxidation. A reaction mechanism in good consistent with the kinetic results will be suggested and discussed.

Iodometric Method; Mechanism; Potassium Permanganate; Rate Equation; Spectrophotometric Method

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