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)`

Options

A. At higher temperature `K_(A)` will be greater than `K_(B)`
B. At lower temperature `K_(A)` and `K_(B)` will differ more and `K_(A) gt K_(B)`
C. As temperature rises `K_(A)` and `K_(B)` will be close to each other in magnitude
D. All of these

Answer

d

Explanation

`K_(A)=Ae^(-E_(A)//RT)` and `K_(B)=Ae^(-E_(B)//RT)`
Also `K_(A) gt K_(B)`
`E_(A) lt E_(B)`
Now notice that all the given facts are satisfied.