When comparing the activation energy between different exothermic reactions, as the activation energy decreases at a given temperature, the reaction rate increases because the

The rate increases because there will be more molecules and atoms that contain the required amount of energy to surpass the activation threshold. As this ratio increases, the speed of the reaction will increase to match. As this ratio increases, the rate of collisions between molecules will increase as well, which will continue to speed the process.

This in turn determines whether the substance exists in the solid, liquid, or gaseous state. Molecules in the solid phase have the least amount of energy, while gas particles have the greatest amount of energy. The temperature of a substance is a measure of the average kinetic energy of the particles.

Explanation: