According to the Arrhenius equation:

Rate constant increases with increases in temperature. This is mainly due to a greater number of collisions whose energy exceeds the activation energy.

 In Arrhenius equation, factor  $e^{-Ea/RT}$ corresponds to fraction of reactant molecules that have kinetic energy equal to activation energy.

The pre-exponential factor depends on the frequency at which collision between reactant molecules per unit volume per unit time occur, irrespective of their energy.

Higher the magnitude  of activation energy of a reaction, stronger is the temperature dependence of its rate constant.