The activation energies of two reactions are `E_(a1)` and `E_(a2)` with `E_(a1) gt E_(a2)`. If the temperature of the reacting systems is increased from `T` to `T'`, which of the following is correct?

Options

A. `(K'_(1))/(K_(1)) = (K'_(2))/(K_(2))`
B. `(K'_(1))/(K_(1)) lt 2 (K'_(2))/(K_(2))`
C. `(K'_(1))/(K_(1)) gt (K'_(2))/(K_(2))`
D. `(K'_(1))/(K_(1)) lt (K_(2))/(K_(2))`

Answer

C

Explanation

ln `(K')/(K) = (E_(a))/(R )((1)/(T) - (1)/(T')) = (E_(a))/(R ) xx (Delta T)/(T T')`
`Delta T` is positive, therefore greater the `E_(a)` value, greater will be value of `(K')/(K)`
`:. (K'_(1))/(K'_(1)) gt (K'_(2))/(K_(2))`