question_answer

A reaction takes place in three steps with activation energy \[{{E}_{{{a}_{1}}}}=180\,\,kJ/mol\], \[{{E}_{{{a}_{2}}}}=80\,\,kJ/mol\] and \[{{E}_{{{a}_{3}}}}=50\,\,kJ/mol\] respectively. Overall rate constant of the reaction is \[k={{\left[ \frac{{{k}_{1}}{{k}_{2}}}{{{k}_{3}}} \right]}^{2/3}}\] The activation energy of the reaction will be-

A) 140 kJ/mol                    

B) 150 kJ/mol

C) 43.44 kJ/mol     

D) 100 kJ/mol