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Conisder the following reaction at 300 K...

Conisder the following reaction at `300 K`:
`Ararr B` (uncatalyzed reaction)
`ArarrB` (catalyzed reaction)
The activation energy is lowered by `8.314 kJ mol^(-1)` for the catalyzed reaction. The rate of this reaction is

A

`15` times

B

`38` times

C

`22` times

D

`28` times

Text Solution

Verified by Experts

The correct Answer is:
D
`log.(k_(2))/(k_(1)) = (E_(a)-E_(ac))/(2.303 RT) = (8.314 xx 10^(3))/(8.314 xx 300) xx (1)/(2.303)`
`rArr (k_(2))/(k_(1)) ~~ 28`
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