The activity of a catalyst influences the reaction rate of the decomposition of hydrogen peroxide by providing an alternative reaction pathway with a lower activation energy. This allows the reaction to proceed at a faster rate, increasing the reaction rate.Hydrogen peroxide H2O2 decomposes into water H2O and oxygen O2 naturally, but the process is slow. The decomposition reaction is as follows:2H2O2 2H2O + O2When a catalyst, such as manganese dioxide MnO2 or catalase an enzyme , is introduced, it speeds up the reaction without being consumed in the process. The catalyst works by temporarily binding to the hydrogen peroxide molecules, forming an intermediate complex. This complex has a lower activation energy than the uncatalyzed reaction, allowing the reaction to proceed more quickly.The activity of the catalyst is determined by factors such as its surface area, concentration, and temperature. A higher surface area allows for more contact between the catalyst and the hydrogen peroxide molecules, increasing the reaction rate. Similarly, a higher concentration of the catalyst or an optimal temperature can also increase the reaction rate.In summary, the activity of a catalyst influences the reaction rate of the decomposition of hydrogen peroxide by providing an alternative reaction pathway with a lower activation energy, allowing the reaction to proceed more quickly. Factors such as surface area, concentration, and temperature can affect the activity of the catalyst and, consequently, the reaction rate.