The use of a catalyst in the reaction between hydrogen peroxide H2O2 and potassium iodide KI significantly increases the rate of the reaction. A catalyst is a substance that increases the rate of a chemical reaction without being consumed or changed in the process. In this case, the catalyst lowers the activation energy required for the reaction to occur, allowing it to proceed at a faster rate.The reaction between hydrogen peroxide and potassium iodide can be represented by the following equation:2H2O2 aq + 2KI aq 2H2O l + 2KOH aq + I2 aq In the presence of a catalyst, such as iron III chloride FeCl3 or sodium thiosulfate Na2S2O3 , the reaction rate increases dramatically. The catalyst works by providing an alternative reaction pathway with a lower activation energy. This allows more reactant molecules to have sufficient energy to undergo the reaction, leading to a faster rate of product formation.In summary, the use of a catalyst in the reaction between hydrogen peroxide and potassium iodide significantly increases the rate of the reaction by lowering the activation energy required for the reaction to proceed. This results in a faster formation of products and a more efficient reaction process.