The effect of temperature on the reaction rate of the decomposition of hydrogen peroxide catalyzed by manganese dioxide can be explained using the collision theory and the Arrhenius equation. According to the collision theory, an increase in temperature leads to an increase in the kinetic energy of the reacting molecules. As a result, the molecules move faster and collide more frequently with greater energy. This increases the probability of successful collisions, where the reacting molecules have enough energy to overcome the activation energy barrier and form products.The Arrhenius equation, which relates the reaction rate constant k to the temperature T and activation energy Ea , is given by:k = Ae^-Ea/RT where A is the pre-exponential factor, R is the gas constant, and T is the temperature in Kelvin. As the temperature increases, the exponential term becomes larger, leading to an increase in the reaction rate constant k .In the case of the decomposition of hydrogen peroxide catalyzed by manganese dioxide, an increase in temperature will generally lead to an increase in the reaction rate. This is because the higher temperature provides the reacting molecules with more kinetic energy, resulting in more frequent and energetic collisions between the hydrogen peroxide and manganese dioxide. Consequently, the decomposition of hydrogen peroxide occurs at a faster rate.However, it is important to note that there may be an optimal temperature range for this reaction, beyond which the reaction rate may decrease due to factors such as the denaturation of the catalyst or a decrease in the solubility of the reactants.