The decomposition of hydrogen peroxide H2O2 with potassium iodide KI as a catalyst is a well-known reaction in chemistry. The overall reaction can be represented as:2H2O2 aq 2H2O l + O2 g The rate law for this reaction can be expressed as:Rate = k[H2O2]^m[KI]^nwhere k is the rate constant, m and n are the orders of the reaction with respect to H2O2 and KI, respectively.To determine the order of the reaction, we can perform a series of experiments by varying the initial concentrations of H2O2 and KI and measuring the initial rate of the reaction. Here's a summary of the experimental data:Experiment | [H2O2]_0 M | [KI]_0 M | Initial Rate M/s -----------|--------------|------------|-------------------1 | 0.1 | 0.1 | 1.0 x 10^-42 | 0.2 | 0.1 | 2.0 x 10^-43 | 0.1 | 0.2 | 2.0 x 10^-4By comparing the initial rates and concentrations between experiments, we can deduce the order of the reaction:- Comparing experiments 1 and 2, we see that doubling the concentration of H2O2 while keeping the concentration of KI constant doubles the initial rate. This suggests that the reaction is first-order with respect to H2O2 m = 1 .- Comparing experiments 1 and 3, we see that doubling the concentration of KI while keeping the concentration of H2O2 constant also doubles the initial rate. This suggests that the reaction is first-order with respect to KI n = 1 .Thus, the overall order of the reaction is the sum of the individual orders: m + n = 1 + 1 = 2. The rate law for this reaction can be written as:Rate = k[H2O2][KI]This means that the rate of the reaction is directly proportional to the product of the concentrations of H2O2 and KI. As the concentration of either reactant increases, the rate of the reaction will also increase. Conversely, as the concentration of either reactant decreases, the rate of the reaction will decrease. This is supported by the experimental data provided.