A reaction takes place in three steps with activation energy E a 1 = 180 kJ / mol , E a 2 = 80 kJ / mol , E a 3 = 50 kJ / mol respectively overall rate contstant of the reaction is k = [ k

Question

A reaction takes place in three steps with activation energy $E_{a_{1}} = 180 kJ / mol, E_{a_{2}} = 80 kJ / mol, E_{a_{3}} = 50 kJ / mol$ respectively overall rate contstant of the reaction is $k = [\frac{k _{1} k _{2}}{k _{3}}]^{2/3}$

the overall activation energy of reaction will be (Here $k_{1}, k_{2}$ & $k_{3}$ are rate constant of first, second and third step respectively.)

TestHub · Accepted Answer

E a ( overall ) ​ = 3 2 ​ ( E a 1 ​ ​ + E a 2 ​ − E a 3 ​ ) ​ = 3 2 ​ ( 180 + 80 − 50 ) ​ = 140 kJ / mol ​

Chemistry - Chemical Kinetics Question with Solution | TestHub

Options:

Doubts & Discussion