Lab Repor Chemical Kinetics

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Abstract

The “Chemical Kinetics” experiment was done to investigate the changes in the rate of reaction under the effect of concentration, temperature, and presence of a catalyst. It was determined that as the concentration of reactants and the temperature increases, the rate of the reaction increases as well. Also, the reaction was run by the presence of catalyst, and the rate of the reaction increased drastically in the presence of it. The order of the reaction with respect to each reactant was calculated to be: x = 1 [I-], y = 1 [BrO3-], z = 2 [H+] by the method of initial rates. The average rate constant was determined to be 26.7 M-3s-1, and the activation energy was calculated to be 49.6 kJ/mol.

Introduction
The whole purpose of this experiment is to deal with the laws of chemical kinetics, and by doing the experiment, compare the experimental results with the theories and see if they were followed. From the kinetics studies, it is obvious that the rate of a reaction increases as the temperature of the reaction increases and as the concentration of the reactants increases. Also, the catalyst increases the rate of the reaction and decreases the activation energy. Thus, this experiment is divided into three sections and the dependence of the reaction rate from different factors is observed step by step.
The idea of the first part of this experiment is to find the reaction orders with respect to each reactant and the rate constant, k. The method of initial rates to calculate the order with respect to each reagent will be used. With different times, the concentrations will vary in each trial. In this experiment, the following type of reaction is considered: aA + bB → cC + dD (1)
The rate law is:
Rate = k[A]x[B]y (2)
The reaction that occurs between the iodine ion and bromate ion will be studied, which is as follows:
6I-(aq) + BrO3-(aq) + 6H+(aq) > 3I2(aq) + Br-(aq) + 3H2O(1) (3)
Then, the rate of the reaction is concluded to be:
Rate =

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