The activation energies of two reactions are `E_(1)` & `E_(2)` with `E_(1)gtE_(2)`. If temperature of reacting system is increased from `T_(1)` (rate constant are `k_(1)` and `k_(2)`) to `T_(2)` (rate constant are `k_(1)^(1)` and `k_(2)^(1)`) predict which of the following alternative is incorrect.

Options

A. `(k_(1)^(1))/(k_(1))=(k_(2)^(1))/(k_(2))`
B. `(k_(1)^(1))/(k_(1))gt(k_(2)^(1))/(k_(2))`
C. `(k_(1)^(1))/(k_(1))lt(k_(2)^(1))/(k_(2))`
D. `k_(1)^(1)ltk_(2)^(1)`

Answer

B

Explanation

Greater the activation energy of a reaction, greater is the temperature dependence of rate constant of reaction.