If the activation energy required for a chemical reaction were reduced, what would happen to the rate of the reaction?

The activation energy as per the definition given by Svante Arrhenius is the minimum amount of energy that is needed for the chemical reaction to proceed. If the amount of the activation energy is decreased then, the reaction would be completed faster.

A catalyst is defined as the substance that lowers the activation energy of a chemical reaction without itself getting consumed so that there will be increase in rate of reaction.

As catalyst lowers the activation energy so, reactant molecules with lower energy also participates in the reaction. Hence, more collisions occur due to which there is rapid formation of products.

Thus, we can conclude that if the activation energy required for a chemical reaction were reduced then there will occur an increase in the rate of the reaction.