question_answer

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 kJ/mol respectively, find the overall energy of activation (kJ/mol).

Answer:

25