The activation energy for the decomposition of hydrogen peroxide H2O2 in the presence of a catalyst depends on the specific catalyst and temperature being used. Common catalysts for this reaction include potassium iodide KI , manganese dioxide MnO2 , and catalase enzyme. The activation energy for the uncatalyzed reaction is typically higher than that for the catalyzed reaction.To determine the activation energy for the catalyzed reaction, you would need to conduct experiments at different temperatures and measure the reaction rates. Then, you can use the Arrhenius equation to calculate the activation energy:k = Ae^-Ea/RT where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant 8.314 J/molK , and T is the temperature in Kelvin.By plotting the natural logarithm of the rate constant ln k against the inverse of the temperature 1/T , you can obtain a straight line with a slope equal to -Ea/R. From this, you can calculate the activation energy for the catalyzed reaction.In general, the activation energy for the decomposition of hydrogen peroxide in the presence of a catalyst is lower than that for the uncatalyzed reaction. This is because the catalyst provides an alternative reaction pathway with a lower energy barrier, allowing the reaction to proceed more quickly and at lower temperatures.