A substance A reacts by parallel reactions to give B and C as shown

 

 

 

Reaction-1:$k_1={10}^{-3}{\sec }^{-1}$ 

${\mathrm{E}}_{{\mathrm{A}}_1}=80\mathrm{Kcal}/\mathrm{mole}$

Reaction-2 :${\mathrm{k}}_2={10}^{-2}{\sec }^{-1}$

${\mathrm{E}}_{{\mathrm{A}}_2}=100\mathrm{Kcal}/\mathrm{mole}$

Identify the correct statement.

The net activation energy for conversion of A is 90 Kcal/mole.

The pre-exponential factor for $1^{\mathrm{st}}$ reaction is smaller as compared to$2^{\mathrm{nd}}$ reaction.

$\left|\mathrm{\Delta H}\right|$ for reaction-1 must be greater than reaction-2

Fraction of A reacting by either of the reaction will be same.