The activation energies of two reactions are E_1" and "E_2 (E_1 gt E_2). If the temperature of the system is increased from T_1" to "T_2, the rate constant changes from k_1" to "k'_1 in the first reaction and k_2" to "k'_2 in the second reaction. Predict which of the following expressions is/are incorrect?

The activation energies of two reactions are E_1" and "E_2 (E_1 gt E_2

1.	The activation energies of two reactions are E_1" and "E_2 (E_1 gt E_2). If the temperature of the system is increased from T_1" to "T_2, the rate constant changes from k_1" to "k'_1 in the first reaction and k_2" to "k'_2 in the second reaction. Predict which of the following expressions is/are incorrect?
Answer» `(k'_1)/(k_1)=(k'_2)/(k_2)` `(k'_1)/(k_1)GT(k'_2)/(k_2)` `(k'_1)/(k_1)lt(k'_2)/(k_2)` `(k'_1)/(k_1)=(k'_2)/(k_2)=1` SOLUTION : `LOG(k_1.)/(k_1)=(E_1)/(2.303R)((T_2-T_1)/(T_1T_2))`…(i) `[thereforeT_2 gtT_1]` `log(k_2.)(k_2)=(E_2)/(2.303R)((T_2-T_1)/(T_1T_2))`…(ii) As, `E_1 gt E_2` From (i) and (ii), we GET `log(k_1.)/(k_1) gt log (k_2.)/(k_2) implies (k_1.)/(k_1) gt (k_2.)/(k_2)`