An increase in temperature by `10^(@)` , can increase the number of collisions only by 2% , but the rate of reaction increases by 100%. Why?

Explanation

Temperature is directly proportional to kinetic energy. Number of collisions is proportional to velocity or square root of temperature. However, in the Arrhenius rate expression, rate increases exponentionally but not linearly, with a change in temperature. The number of molecules exceeding the activation energy approximately doubles by a `10^(@)` rise in temperature. Hence rate increases by `100%`.