Why is it important to use a catalyst in the decomposition of hydrogen peroxide?

Using a catalyst in the decomposition of hydrogen peroxide is essential because it speeds up the reaction without being consumed in the process. In this reaction, hydrogen peroxide (H₂O₂) breaks down into water (H₂O) and oxygen (O₂). In the absence of a catalyst, this decomposition occurs very slowly, and the reaction may take a considerable amount of time to proceed to completion.

By introducing a catalyst, typically manganese dioxide or catalase, the activation energy required for the reaction is lowered. This allows the hydrogen peroxide to decompose more rapidly, leading to a quicker release of oxygen and the formation of water. The use of a catalyst is particularly beneficial in industrial and laboratory settings, where time efficiency is important.

The other options do not accurately reflect the role of a catalyst in this reaction. A catalyst does not lower the temperature of the reaction or change the products formed; instead, it facilitates the reaction at the same temperature and produces the same products. Additionally, catalysts do not increase the concentration of reactants; they simply enhance the rate at which the existing reactants convert to products.