The rate constant increases with increase in temperature and becomesalmost double for every 10° increase in temperature. Swedish chemist,Arrhenius derived a quantitative relation between rate of reaction andtemperature. According to Arrhenius, $k=A e^{-\frac{E_{a}}{R T}}$ or, $\log k = \log A - \frac{E_{a}}{R T}$ or, $\log \frac{k_{2}}{k_{1}} = \frac{E_{a}}{2.303 R} \left[ \frac{1}{T_{1}} - \frac{1}{T_{2}} \right]$ where$\; \; \; \; \; \; k_1$ = rate constant at temperature $T_1$,$\; \; \; \; \; \; k_2$ = rate constant at temperature $T_2$,$\; \; \; \; \; \; E_a$ = energy of activation, R = universal gas constant.