Question

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

Answer 1

if activation energy is reduced the rate of reactin increases

Answer 2

The relation between rate of reaction and activation energy is given by Arrhenius equation : k = Ae^-Ea/RT  We can see that as activation energy decrease, rate increases in an exponential manner.  Conceptually, we can think of the activation energy as a hill in front of the reactants. For the reactants to become products, energy is required to go over the hill. Higher the hill, higher the energy, lesser products. Hence, by decreasing activation energy, we are reducing the height of the hill and making it easier for reactants to become products.