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 velcoity or square root of temperature .
However , in the Arrhenius rate expression, rate increases exponentially but not linearly, with a change in temperature . The number of molecules exceeding the activation energy approoxid double by a `10^(@)` rise in temperature . Hence rate increase by 100%.