The activation energies of two reactions are ${E_a}$ and ${E'_a}$ with ${E_a} > {E'_a}.$ If the temperature of the reacting systems is increased from ${T_1}$ to ${T_2}$, predict which alternative is correct. $K'$ are rate constants at higher temperature. Assume $A$ being same for both the reactions:

$\frac{{{{K'}_1}}}{{{K_1}}} = \frac{{{{K'}_2}}}{{{K_2}}}$

${K_1} > {K_2}$ and ${K'_1} > {K'_2}$

$\frac{{{{K'}_1}}}{{{K_1}}} < \frac{{2{{K'}_2}}}{{{K_2}}}$

NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

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Analyzing +4 | -1

The activation energies of two reactions are

{E_a}

and

{E'_a}

with

{E_a} > {E'_a}.

If the temperature of the reacting systems is increased from

{T_1}

{T_2}

, predict which alternative is correct.

K'

are rate constants at higher temperature. Assume

A

being same for both the reactions:

View answer and explanation

Correct option: B

{K_1} < {K_2}

and

{K'_2} < {K'_1}

Option B (

{K_1} < {K_2}

and

{K'_2} < {K'_1}

) is correct because the reaction with the lower activation energy will have a greater increase in rate constant with increasing temperature.