AIIMS 2018 Chemistry Arrhenius Equation MCQ Question with Solution

Rate of two reaction whose rate constants are $k_1$ & $k_2$ are equal at $300\text{ K}$ such that : $E_{a_2} - E_{a_1} = 2RT$ So calculate $\ln \frac{A_2}{A_1}$

A

$\ln 4$

B

$2$

C

$\log 2$

D

$2 - \ln 2$

Correct Answer

Option B

Detailed Explanation

The equation derived from the logarithmic relationship shows that ln(A₂/A₁) equals 2, which implies that the ratio of the rate constants (k₂/k₁) is equal to e². This indicates a significant increase in the reaction rate due to the change in activation energy (Eₐ). Other options are not applicable as they do not provide relevant information or correct interpretations of the logarithmic relationship in the context of reaction kinetics. Understanding this relationship is crucial for analyzing how changes in activation energy affect reaction rates in chemical kinetics.

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AIIMS 2018 Chemistry Arrhenius Equation MCQ Question

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