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The substance undergoes first order deco...

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

`K_1=10^(-2) sec^(-1) and K_2=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:

A

120 kJ `"mol"^(-1)`

B

116 kJ `"mol"^(-1)`

C

100 kJ `"mol"^(-1)`

D

150 kJ `"mol"^(-1)`

Text Solution

Verified by Experts

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