The reaction between hydrogen peroxide H2O2 and potassium iodide KI can be represented by the following equation:H2O2 aq + 2 KI aq 2 H2O l + 2 KI aq + I2 s The rate law for this reaction can be determined experimentally by measuring the initial rates of the reaction at different initial concentrations of the reactants. The rate law is given by: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 rate law experimentally, follow these steps:1. Prepare a series of reaction mixtures with varying initial concentrations of H2O2 and KI, keeping the concentration of one reactant constant while varying the other.2. Measure the initial rate of the reaction for each mixture. This can be done by monitoring the formation of I2, which can be detected spectrophotometrically due to its color.3. Analyze the data by plotting the initial rates against the initial concentrations of the reactants. This will help you determine the order of the reaction with respect to each reactant.4. Determine the values of m and n by comparing the initial rates and initial concentrations. For example, if doubling the concentration of H2O2 doubles the initial rate, then the reaction is first-order with respect to H2O2 m = 1 . If doubling the concentration of KI quadruples the initial rate, then the reaction is second-order with respect to KI n = 2 .5. Once the values of m and n are determined, the rate law can be written as:rate = k [H2O2]^m [KI]^nFor the reaction between hydrogen peroxide and potassium iodide, it is generally found that the reaction is first-order with respect to both H2O2 and KI:rate = k [H2O2]^1 [KI]^1However, it is important to note that the rate law and the reaction orders may vary depending on the specific experimental conditions, such as the presence of catalysts or other species in the reaction mixture.