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Two reaction, $A ⟶$ products and $B ⟶$ products have rate constant $k_{a} a n d k_{b}$ at temperature $T$ and activation energies $E_{a} a n d E_{b}$ respectively. If $k_{a} > k_{b} a n d E_{a} < E_{b}$ and assuming that $A$ for both the reactions is same then:

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at lower temperature $k_{a}$ and $k_{b}$ will differ more and $k_{a} > k_{b}$

all of the above

at higher temperature $k_{a}$ will be greater than $k_{b}$

as temperature rises $k_{a}$ and $k_{b}$ will be close to each other in magnitude

answer is D.

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Detailed Solution

The fact is,

$K_{a} = {Ae}^{- E_{a} R T} and K_{b} = {Ae}^{- E_{b} R T}$

Also given,

$K_{a} > K_{b}$

$E_{a} < E_{b}$

so, at a greater temperature $k_{a}$ will be greater than $k_{b}$

Additionally, at lower temperatures $k_{a}$ and $k_{b}$ will differ more and $k_{a} > k_{b}$ .

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