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Catalysts are substances that increase the rate of a chemical reaction without being consumed in the process. One of the primary ways they achieve this is by lowering the activation energy required for the reaction to occur. Activation energy is the minimum energy that reacting molecules must have to collide and react. By providing an alternative pathway with a lower activation energy, catalysts enable more reactant molecules to have sufficient energy to undergo the reaction, thus speeding up the reaction rate.

In contrast, catalysts do not increase the temperature of the reaction; they facilitate more efficient reactions at existing temperatures. Additionally, they do not shift the position of equilibrium in reversible reactions, which is a property associated with changes in concentration, pressure, or temperature. Therefore, the ability of catalysts to lower the activation energy is a fundamental characteristic that distinguishes them from other substances involved in chemical reactions.