Write the Arrhenius equation to calculate the activation energy $(E_a)$ at two different temperatures.
(N/A) The Arrhenius equation at two different temperatures $T_1$ and $T_2$ with rate constants $k_1$ and $k_2$ is given by:
$\ln\left(\frac{k_2}{k_1}\right) = \frac{E_a}{R} \left[\frac{T_2 - T_1}{T_1 T_2}\right]$
where:
$E_a$ = Activation energy
$R$ = Universal gas constant
$k_1, k_2$ = Rate constants at temperatures $T_1$ and $T_2$ respectively.
$\ln\left(\frac{k_2}{k_1}\right) = \frac{E_a}{R} \left[\frac{T_2 - T_1}{T_1 T_2}\right]$
where:
$E_a$ = Activation energy
$R$ = Universal gas constant
$k_1, k_2$ = Rate constants at temperatures $T_1$ and $T_2$ respectively.
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