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The activation energies for the two reac...

The activation energies for the two reactions are Ea and `Ea^(')` with `E_(a)gtE_(a)^(')`. If the temperature of the reaction system is increased from `T_(1)` to `T_(2)`. Predict which alternative is correct. `(k^('))` are the rate constants at highest temperature.

A

`(k_(1)^('))/(k+(1)) = (k_(2)^('))/(k_(2))`

B

`k_(1) lt k_(2)` and `k_(2)^(') lt k_(1)^(')`

C

`k_(1) lt k_(2)`

D

`(k_(1)^(')/k_(1)) lt (2k_(2)^('))/(k_(2))`

Text Solution

Verified by Experts

The correct Answer is:
B
b) We know that
`k=Ae^((-Ea)/(RT))`
This means that more is the activation energy, lesser is the rate constant.
Since `E_(a) gt E_(a)^(')`
`therefore k_(1) lt k_(2)` and `k_(1)^(')` and `k_(2)^(')`
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