Which statement best describes the relationship between activation energy and rate of reaction? Increasing the activation energy can increase the rate of a reaction
Reducing the activation energy can increase the rate of a reaction.
Increasing the reaction energy does not alter the rate of reaction
Reducing the activation energy can decrease the rate of a reaction

Reducing the activation energy can increase the rate of a reaction.

Explanation:

Activation energy is the extra energy that must be supplied to reactants in order to cross the energy barrier and thus convert to products.

A catalyst is a substance which increases the rate of a reaction by taking the reaction through a different path which involves lower activation energy and thus more molecules can cross the energy barrier and convert to products leading to increased rate of reaction.

Thus a catalyst speeds up the reaction by decreasing the activation energy.

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