How is the energy of activation determined ?

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For the given reaction, rate constants $k_{1} a n d k_{2}$ are measured at two different temperatures $T_{1}$ and $T_{2}$ respectively. Then
${log}_{10} . \frac{k_{2}}{k_{1}} = E_{a} \frac{T_{2} - T_{1}}{2.303 R \times T_{1} \times T_{2}}$
where $E_{a}$ is the energy of activation.
Hence by substituting appropriate values, energy of activation $E_{a}$ for the reaction is determined.

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Updated on:21/07/2023

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