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The temperature dependence of rate constant (k) of a chemical reactions is written in terms of
Arrhenius equation, k ${= A. e}^{{-E}_{a}}$ Activation energy $(E_{a})$ of the reaction can be calculated by
Plotting.

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$k vs. \frac{1}{log T}$

$log k vs \frac{1}{T}$

$log k vs. \frac{1}{log T}$

$k vs. T$

answer is B.

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Detailed Solution

${k = Ae}^{{-E}_{a} /RT} log k = log A - \frac{E_{a}}{2.303R} . \frac{1}{T}$

$Plot of log k Vs. \frac{1}{T}$

$Straight line slope = \frac{{-E}_{a}}{2.303R}$

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