Increasing the temperature generally increases the reaction rate of a chemical reaction, including the decomposition of hydrogen peroxide H2O2 catalyzed by manganese dioxide MnO2 . This is because higher temperatures provide more energy to the reacting molecules, which increases the frequency of collisions between them and the likelihood of successful collisions that lead to a reaction.In the case of the decomposition of hydrogen peroxide catalyzed by manganese dioxide, the reaction can be represented by the following equation:2 H2O2 aq 2 H2O l + O2 g Manganese dioxide acts as a catalyst, meaning it speeds up the reaction without being consumed in the process. It does this by providing an alternative reaction pathway with a lower activation energy, making it easier for the reaction to occur.When the temperature is increased, the kinetic energy of the hydrogen peroxide molecules also increases, leading to more frequent and energetic collisions between the molecules and the manganese dioxide catalyst. This results in a higher probability of successful collisions and a faster reaction rate.However, it is important to note that there is an optimal temperature range for this reaction. If the temperature is increased too much, the reaction rate may decrease due to the denaturation of the catalyst or other factors that negatively affect the reaction. Additionally, very high temperatures may cause the hydrogen peroxide to decompose without the catalyst, which could lead to an uncontrollable reaction.In summary, increasing the temperature generally increases the reaction rate of the decomposition of hydrogen peroxide catalyzed by manganese dioxide, as it provides more energy for successful collisions between the reacting molecules. However, there is an optimal temperature range for this reaction, and excessively high temperatures may have negative effects on the reaction rate.