The reaction rate of the decomposition of hydrogen peroxide typically increases with temperature. This is because, as temperature increases, the kinetic energy of the molecules also increases, leading to more frequent and energetic collisions between the reactant molecules. As a result, a greater number of these collisions have enough energy to overcome the activation energy barrier, leading to an increased reaction rate.The relationship between reaction rate and temperature can be described by the Arrhenius equation:k = Ae^-Ea/RT where k is the reaction 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.To determine the activation energy Ea of the decomposition of hydrogen peroxide, you would need to perform a series of experiments at different temperatures and measure the reaction rate constants k at each temperature. By plotting the natural logarithm of the rate constants 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.The activation energy for the decomposition of hydrogen peroxide varies depending on the presence of catalysts and the specific conditions of the reaction. In the absence of a catalyst, the activation energy is typically around 75 kJ/mol. However, this value can be significantly reduced in the presence of a catalyst, such as manganese dioxide or potassium iodide, which lowers the activation energy barrier and increases the reaction rate.