A reaction takes place in various steps. The rate constant for first, second, third and fifth st...
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A reaction takes place in various steps. The rate constant for first, second, third and fifth steps are \( k_{1}, k_{2}, k_{3} \) and \( k_{5} \) respectively. The overall rate constant is given by
\[
k=\frac{k_{2}}{k_{3}}\left(\frac{k_{1}}{k_{5}}\right)^{1 / 2}
\]
If activation energy are \( 40,60,50 \) and \( 10 \mathrm{~kJ} / \mathrm{mol} \) respectively, the overall energy of activation \( (\mathrm{kJ} / \mathrm{mol}) \) is :
(a) 10
(b) 20
(c) 25
(d) none of these
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