Question

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

Answer 1

Answer: The rate would increase.

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 chemical reaction which involves lower activation energy, means more molecules will gain sufficient energy to cross the energy barrier, thus  effective collisions increase and more products will be formed and hence the rate of reaction would increase.

The effect of catalyst on activation energy is shown in the image below:

Answer 2

The rate would increase because more molecules would collide at the activation energy, which will cause more molecules to react, and thus it will speed up the reaction rate.