If the activation energy required for a chemical reaction were reduced

The rate of the reaction would increase.

Explanation:

The activation energy in chemistry and biology is the energy that a system needs before it can start a certain process. The activation energy is usually used to designate the minimum energy necessary for a given chemical reaction to occur. For a reaction to occur between two molecules, they must collide in the correct orientation and have a minimum amount of energy. As the molecules approach, their electron clouds repel. This requires energy (activation energy) and comes from the heat of the system, that is, the translational, vibrational energy of each molecule.

The activation energy of the reaction corresponds to the energy necessary for the reaction to be carried out with less reagent energy. The lower the activation energy of a reaction, the higher the speed of the reaction.

A reaction is called exothermic when it provides for the medium a higher energy than is necessary to reach the activated complex.

When a reaction is endothermic, it provides for the environment a lower energy than is necessary to reach the activated complex.

Catalysts are substances that decrease the activation energy for a given reaction, without altering its ΔH. The catalysts do not alter during the reactions.