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The temperature dependence of rate constant $(k)$ of a chemical reaction is written in terms of Arrhenius equation, $\mathrm{k}=\mathrm{A} \cdot e^{-\mathrm{Ea} / \mathrm{RT}}$. Activation energy $\left(\mathrm{E}_a\right)$ of the reaction can be calculated by ploting:
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$\log k$ vs $\frac{1}{\mathrm{T}}$
We can calculate the Activation Energy by graphing ln k versus 1/T. When the $\ln k$ (rate constant) is plotted versus the inverse of the temperature (kelvin), the slope is a straight line. The value of the slope $(\mathrm{m})$ is equal to $-\mathrm{Ea} / \mathrm{R}$ where $\mathrm{R}$ is a constant equal to $8.314 \mathrm{~J} / \mathrm{mol}-\mathrm{K}$.
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