The effect of temperature on the reaction rate of the decomposition of hydrogen peroxide catalyzed by manganese dioxide can be explained using the Arrhenius equation, which relates the rate constant k of a reaction to the temperature T and the activation energy Ea of the reaction:k = Ae^-Ea/RT where A is the pre-exponential factor, R is the gas constant 8.314 J/molK , and T is the temperature in Kelvin.As the temperature increases, the reaction rate generally increases due to the increased kinetic energy of the molecules. This increased kinetic energy allows more molecules to overcome the activation energy barrier, leading to a higher rate of successful collisions and thus a faster reaction rate.To determine the activation energy of the reaction, you would need to perform experiments at different temperatures and measure the reaction rates. 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 of the reaction.In summary, the reaction rate of the decomposition of hydrogen peroxide catalyzed by manganese dioxide increases as the temperature increases. The activation energy of the reaction can be determined experimentally by measuring the reaction rates at different temperatures and applying the Arrhenius equation.