The substance undergoes first order decomposition.The decomposition follows two parallel first order reactons as :

`K_1=10^(-2) sec^(-1) and K_2=4 * 10^(-2)sec^(-1)`
If the corresponding activation energies of parallel reaction are 100 and 120 kJ `"mol"^(-1)` then the net activation energy of A is/are:

Options

A. 120 kJ `"mol"^(-1)`
B. 116 kJ `"mol"^(-1)`
C. 100 kJ `"mol"^(-1)`
D. 150 kJ `"mol"^(-1)`

Answer

B

Explanation

`E=(k_1E_1+k_2E_2)/(k_1+k_2)=(10^(-2)xx100+120xx4xx10^(-2))/(10^(-2)+4xx10^(-2))=116 kJ mol^(-1)`