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

The rate would increase.

Explanation:

Activation energy is the minimum energy for a chemical reaction to occur, ie it is one of the determining factors for the occurrence of a reaction, together with contact and favorable collision between the reactant molecules. The reaction rate corresponds to the rate at which the chemical reaction occurs. In chemistry and specifically chemical kinetics, the activation energy and activation rate are inversely proportional, which means that when the activation energy is reduced, the reaction rate increases.

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