The two reactions $\text{(I) } \mathrm{A} \rightarrow \text{Products},$ and $\text{(II) } \mathrm{B}\rightarrow \text{Products}$ follow first-order kinetics. The rate of reaction-I is doubled when temperature is raised from $300$ to $310 \mathrm{~K}.$ The half-life for this reaction at $310 \mathrm{~K}$ is 30 minutes. At the same temperature, B decomposes twice as fast as A. If the energy of activation for the reaction-II is half that of reaction-I, the rate constant of reaction-II at 300 K is

NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

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The two reactions

\text{(I) } \mathrm{A} \rightarrow \text{Products},

and

\text{(II) } \mathrm{B}\rightarrow \text{Products}

follow first-order kinetics. The rate of reaction-I is doubled when temperature is raised from

300

310 \mathrm{~K}.

The half-life for this reaction at

310 \mathrm{~K}

is 30 minutes. At the same temperature, B decomposes twice as fast as A. If the energy of activation for the reaction-II is half that of reaction-I, the rate constant of reaction-II at 300 K is

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Correct option: B

0.0327 \mathrm{~min}^{-1}

Option B (0.0327 min⁻¹) is correct because it is calculated by using the Arrhenius equation and the given information about the rate constants and activation energies of the two reactions.

NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

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