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For a reaction taking place in three steps, the rate constants are k1,k2,k3.The overall rate constant k=k1k2/k3.If the energy of activation values for the first , second and third stages are respectively 40 , 50 , 60 kJ per mole , then the overall energy of activation in kJ / mol is ??please explain the solution

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Solution

Given k=k1(k2)^1/2/k3 Taking log both the side lnk=lnk1+lnk2(1/2)-lnk3 We know that k=Ae^-Ea/RT;lnk=lnA-Ea/RT let every step have same arrhenius constant(i.e.A) and Ea1,Ea2 and Ea3 are the corresponding activation energy for 1^st,2nd and the third step respectively. So, k=lnA-Ea/RT=lnA-Ea1/RT..+(1/2)[lnA-Ea2/RT]-lnA+Ea3/RT So if we have value of A then we can get the value of Ea using the equation

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