For a reaction, if effective rate constant k' is given b
`k=(2k_2)/k_3(k_1/k_5)^(1//5)`
where `k_1,k_2,k_3,k_5` are rate constants for different steps of the reaction
The effective frequency factor

For a reaction, if effective rate constant k' is given b k=(2k_2)/k_3(k_1/k_5)^(1//5) where k_1,k_2,k_3,k_5 are rate constants for different steps of the reaction The effective activation energy is

For a reaction, if effective rate constant k' is given b k=(2k_2)/k_3(k_1/k_5)^(1//5) where k_1,k_2,k_3,k_5 are rate constants for different steps of the reaction Which one is correct ?

For a reaction A overset (k) rarr product, the reaction occurs as : A overset (k_1) rarr A^(**) overset (k_2) rarr B^(**) overset (k_3) rarr product The overall rate constant k is given as: k= 2k_1 (k_2/k_3)^(2//3) If E_(a1) , E_(a2) and E_(a3) are the activation energies of these steps, then what is the relation between overall activation energy E_(a) and the activation energies of these steps.

A reaction is represented by A to^(k_1) B (slow). A+B to^(k_2) C (fast). Where k_1 and k_2 are the rate constants of the mechanistic steps. The rate of production of C will be given by

A reaction is represented by A to^(k_1) B (slow). A+B to^(k_2) C (fast). Where k_1 and k_2 are the rate constants of the mechanistic steps. The rate of production of C will be given by

A reaction is represented by : A to B slow and A+B to C (fast) where k_1 and k_2 are the rate constants of the mechanistic steps. The rate of production of B will be given by :

A reaction is represented by : A to B slow and A+B to C (fast) where k_1 and k_2 are the rate constants of the mechanistic steps. The rate of production of B will be given by :

60.A consecutive reaction occurs with two equilibria which co-exist together P(k_(1))/(k_(2) Q (k_(3))/(k_(4) R Where k_(1) , k_(2) , k_(3) and k_(4) are rate constants.Then the equilibrium constant for the reaction P harr R is (1) (k_(1)*k_(2)) / (k_(3)*k_(4) ) (2) (k_(1)*k_(4)) / (k_(2)k_(3) ) (3) k_(1) * k_(2) * k_(3)*k_(4) (4) (k_(1)*k_(3)) / (k_(2)k_(4)) ]]

A reaction takes place in various steps. The rate constant for first, second, third and fifth steps are k1, k2, k3 and k5 respectively. The overall rate constant is is given by: k = k_(2)/k_(1) (k_(1)/k_(2))^(1/2) activation energy are 40,60, 50 and 10 kJ/mol respectively, find the overall energy of activation (kJ/mol).