$
\begin{aligned}
& \mathrm{A} \longrightarrow \mathrm{~B} ext { (first reaction) } \
& \mathrm{C

Question

$
\begin{aligned}
& \mathrm{A} \longrightarrow \mathrm{~B} 	ext { (first reaction) } \
& \mathrm{C} \longrightarrow \mathrm{D} 	ext { (second reaction) }
\end{aligned}
$
Consider the above two first-order reactions. The rate constant for first reaction at 500 K is double of the same at 300 K . At $500 \mathrm{~K}, 50 \%$ of the reaction becomes complete in 2 hour. The activation energy of the second reaction is half of that of first reaction. If the rate constant at 500 K of the second reaction becomes double of the rate constant of first reaction at the same temperature; then rate constant for the second reaction at 300 K is $\_\_\_\_$ $	imes 10^{-1}$ hour $^{-1}$ (nearest integer).

Professor PC Thomas Classes · Answer

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