The decomposition of hydrogen peroxide H2O2 catalyzed by potassium iodide KI can be represented by the following reaction:2 H2O2 aq 2 H2O l + O2 g In this reaction, potassium iodide acts as a catalyst, which means it speeds up the reaction without being consumed in the process. The actual reaction mechanism involves the formation of iodine I2 and iodide ions I- as intermediate species.Now, let's consider the effect of increasing pressure on the reaction rate. The reaction rate depends on the frequency of collisions between reactant molecules and the energy of these collisions. According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in pressure, the system will adjust to counteract the change and re-establish equilibrium.In the case of the decomposition of hydrogen peroxide catalyzed by potassium iodide, increasing the pressure will have the following effects:1. Increasing the pressure will increase the concentration of the reactants H2O2 in the reaction mixture. This will lead to a higher frequency of collisions between reactant molecules, which in turn will increase the reaction rate.2. The reaction involves the formation of a gas O2 as a product. According to Le Chatelier's principle, increasing the pressure will shift the equilibrium position to the side with fewer moles of gas. In this case, the reaction will shift to the left toward the reactants , which will decrease the reaction rate.However, it is important to note that the effect of pressure on the reaction rate may not be significant in this case, as the reaction is catalyzed by potassium iodide. The presence of the catalyst will help to lower the activation energy of the reaction, which will increase the reaction rate regardless of the pressure change.In summary, increasing the pressure in the decomposition of hydrogen peroxide catalyzed by potassium iodide may have a mixed effect on the reaction rate. While it may increase the reaction rate due to higher reactant concentrations, it may also decrease the reaction rate by shifting the equilibrium position. The presence of the catalyst, however, will likely have a more significant impact on the reaction rate than the pressure change.