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. I
B. II
C. I, III
D. I, III, IV

Answer

B

Explanation

Since `k_(2) lt k_(2)` and `E_(2) gt E_(1)`
form Arrehenius equation `(k = Ae^(-E_(a)//RT))`, if `k_(1)` is high then `E_(1)` is low. Therefore, with increase in temperature increase in `k_(1)` will be greater than increase in `k_(2)`.