Two reactions `A rarr` products and `B rarr` products have rate constants `k_(a)` and `k_(b)` respectively at temperature `T` and activation energies are `E_(a)` and `E_(b)` respectively.
If `k_(a) gt k_(b)` and `E_(a) lt E_(b)` and assuming the freuency factor `A` in both the reactions are same then

Two reaction : X rarr Products and Y rarr Products have rate constants k_(1) and k_(2) at temperature T and activation energies E_(1) and E_(2) , respectively. If k_(1) gt k_(2) and E_(1) lt E_(2) (assuming that the Arrhenius factor is same for both the Products), then (I) On increaisng the temperature, increase in k_(2) will be greater than increaisng in k_(1) . (II) On increaisng the temperature, increase in k_(1) will be greater than increase in k_(2) . (III) At higher temperature, k_(1) will be closer to k_(2) . (IV) At lower temperature, k_(1) lt k_(2)

The rate constants k_(1) and k_(2) for two different reactions are 10^(25)e^(-4000//T) and 10^(25)e^(-1000//T) , respectively. The temperature at which k_(2)=k_(2) is

The rate constant k_(1) and k_(2) for two different reactions are 10^(16) e^(-2000//T) and 10^(15) e^(-1000//T) , respectively. The temperature at which k_(1) = k_(2) is

A certain endothermic reaction: Ararr Product, DeltaH=+ve proceeds in a sequence of three elementary steps with the rate constants K_(1), K_(2) and K_(3) and each one having energy of activation E_(a), E_(2) and E_(3) respectively at 25^(@)C . The observed rate constant for the reaction is equal to K_(3) sqrt(K_(1)/K_(2)). A_(1), A_(2) and A_(3) are Arrhenius parameters respectively. The observed energy of activation for the reaction is: