Assertion (A):  According to collision theory $\log \frac{{\text{k}}_{\text{2}}}{{\text{k}}_{\text{1}}}=\frac{{\text{E}}_{\text{a}}}{2.303\text{R}}\left[\frac{{\text{T}}_{\text{2}}{\text{-T}}_{\text{1}}}{{\text{T}}_{\text{1}}{\text{T}}_{\text{2}}}\right]$

Reason (R): Collision theory is applicable to all reactions.

The variation of rate constant with temperature is expressed in terms of 

Arrhenius Equation i.e  $\text{k}={\text{Ae}}^{-{\text{E}}_{\text{a}}\text{/RT}}$

At two different temperatures ${\text{T}}_{\text{1}}{\text{ and T}}_{\text{2}}$ , Arrhenius rate equation is written as

          $\text{log}\frac{k_2}{k_1}=\frac{{\text{E}}_{\text{a}}}{2.303\text{R}}\left[\frac{{\text{T}}_2-{\text{T}}_1}{{\text{T}}_{\text{1}}{\text{T}}_{\text{2}}}\right]$

Collision theory is applicable for bimolecular reactions only but not to all reactions.