For the first order reaction $\mathrm{A} ightarrow \mathrm{B}+\mathrm{C}$ is carried out at $27^{\circ} \mathrm{C}$. If $3.8 imes 10^{-16} \%$ of the reactant molecules exists in the activated state, the $\mathrm{E}_{e}$ (activation energy) of the reaction is:

Question

For the first order reaction $\mathrm{A} ightarrow \mathrm{B}+\mathrm{C}$ is carried out at $27^{\circ} \mathrm{C}$. If $3.8 	imes 10^{-16} \%$ of the reactant molecules exists in the activated state, the $\mathrm{E}_{e}$ (activation energy) of the reaction is:

Aicharya · Accepted Answer

$\mathrm{e}^{-\frac{\mathrm{E}_{\mathrm{a}}}{\mathrm{RT}}}=3.8 \times-\frac{10^{-16}}{100}$
$-\frac{\mathrm{E}_{\mathrm{a}}}{\mathrm{RT}}=\ln 3.8 \times 10^{-18}$
$\mathrm{E}_{\mathrm{a}}=100 \mathrm{~kJ} / \mathrm{mol}$

For the first order reaction $\mathrm{A} ightarrow \mathrm{B}+\mathrm{C}$ is carried out at $27^{\circ}…

Solution