Write the Arrhenius equation representing the relationship between the rate constants $k_1$ and $k_2$ at two different temperatures $T_1$ and $T_2$.

(N/A) The Arrhenius equation at two different temperatures is given by: $\log \frac{k_2}{k_1} = \frac{E_a}{2.303R} [\frac{T_2 - T_1}{T_1 T_2}]$
Where:
$k_1$ and $k_2$ are the rate constants at temperatures $T_1$ and $T_2$ respectively.
$E_a$ is the activation energy.
$R$ is the universal gas constant.