For the first order reaction $A \overset{}{\to} B + C$ , carried out at 27°C. If $3.8 \times 10^{- 16} %$ of the reactant molecules exists in the activated state, the Ea (activation energy) of the reaction is:

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Detailed Solution

$\begin{array}{l} e^{- \frac{E_{a}}{R T}} = 3.8 \times \frac{10 -^{16}}{100} \\ - \frac{E_{a}}{R T} = i n 3.8 \times 10^{- 18} \\ E_{a} = 100 k j / m o l \end{array}$

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