The temperature dependence of rate constant $(k)$ of a chemical reaction is written in terms of Arrhenius equation, $k = A . e^{- ε a / R T}$ .Activation energy $(E_{a})$ of the reaction can calculated by plotting

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$k v s . \frac{1}{\log T}$

$\log k v s . \frac{1}{\log T}$

$k v s . T$

$\log k v s \frac{1}{T}$

answer is B.

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Detailed Solution

Use the formula,

$k = A e^{- E_{a} / R T}$

Where,

K = rate constant

A = Frequency

$E_{a}$ = Activation energy

R = Universal gas constant

T = Temperature

$\log K = \log A - \frac{E a}{2.303 R} . \frac{1}{T}$

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

Straight line Slope $= \frac{- E_{a}}{2.303 R}$

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