The reaction rate of the decomposition of hydrogen peroxide H2O2 catalyzed by manganese dioxide MnO2 is affected by temperature. As the temperature increases, the reaction rate also increases. This is because an increase in temperature provides more energy to the molecules involved in the reaction, causing them to move faster and collide more frequently with each other.According to the Arrhenius equation, the rate constant k of a reaction is related to the temperature T by the following equation:k = Ae^-Ea/RT where A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin. As the temperature increases, the exponential term becomes smaller, and the rate constant k increases, leading to a faster reaction rate.In the case of the decomposition of hydrogen peroxide catalyzed by manganese dioxide, the increase in temperature will cause the hydrogen peroxide molecules to collide more frequently and with greater energy with the manganese dioxide catalyst. This will result in a higher probability of successful collisions and the formation of the products, water H2O and oxygen gas O2 .However, it is important to note that there is an optimal temperature range for this reaction. If the temperature becomes too high, the hydrogen peroxide may decompose too rapidly, potentially causing safety hazards or loss of control over the reaction. Additionally, at extremely high temperatures, the manganese dioxide catalyst may lose its effectiveness or undergo unwanted side reactions.