(C) The Arrhenius equation is $k = A e^{-E_a/RT}$.Statement $A$ is incorrect because the Arrhenius equation is applicable to both elementary and compl

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(C) The Arrhenius equation is $k = A e^{-E_a/RT}$.Statement $A$ is incorrect because the Arrhenius equation is applicable to both elementary and complex reactions.Statement $B$ is correct because $A$ (the frequency factor) has the same units as the rate constant $k$.Statement $C$ is correct because a lower activation energy $(E_a)$ results in a larger value of $e^{-E_a/RT}$,leading to a faster reaction rate.Statement $D$ is incorrect because $A$ and $E_a$ are generally considered temperature-independent constants for a given reaction.Statement $E$ is incorrect as $A$ and $E_a$ are independent parameters.Therefore,only statements $B$ and $C$ are correct.

Class 12 Chemistry Chemical Kinetics Collision theory, Energy of activation and Arrhenius equation

Difficult

Consider the following statements related to the temperature dependence of rate constants. Identify the correct statements:
$A.$ The Arrhenius equation holds true only for an elementary homogeneous reaction.
$B.$ The unit of $A$ is the same as that of $k$ in the Arrhenius equation.
$C.$ At a given temperature,a low activation energy means a fast reaction.
$D.$ $A$ and $E_a$ as used in the Arrhenius equation depend on temperature.
$E.$ When $E_a > RT$,$A$ and $E_a$ become interdependent.
Choose the correct answer from the options given below:

JEE MAIN 2025 All JEE MAIN

A
$A, C$ and $D$ Only
B
$B, D$ and $E$ Only
C
$B$ and $C$ Only
D
$A$ and $B$ Only

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Class 12

Chemistry Questions

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

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For the reaction,$A \rightleftharpoons B$,$E_a = 50 \ kJ \ mol^{-1}$ and $\Delta H = -20 \ kJ \ mol^{-1}$. When a catalyst is added,$E_a$ decreases by $10 \ kJ \ mol^{-1}$. What is the $E_a$ for the backward reaction in the presence of the catalyst?

MediumKCET 2024

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The rate of a reaction quadruples when the temperature changes from $300 \, K$ to $310 \, K$. The activation energy of this reaction is ........... $kJ \, mol^{-1}$ (Assume activation energy and pre-exponential factor are independent of temperature; $\ln 2 = 0.693$; $R = 8.314 \, J \, mol^{-1} \, K^{-1}$)

DifficultJEE MAIN 2017

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For an exothermic reaction $A \rightarrow B$,the activation energy is $15 \, K \, cal/mol$ and the heat of reaction is $5 \, K \, cal/mol$. The activation energy for the reverse reaction $B \rightarrow A$ will be ......... $K \, cal/mol$.

Medium

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For an endothermic reaction,the energy of activation is $E_a$ and the enthalpy of reaction is $\Delta H$ (both in $kJ/mol$). The minimum value of $E_a$ will be:

MediumAIPMT 2010

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An increase in temperature by $10\,^{\circ}C$,generally increases the rate of a reaction by .......... times.

Easy

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For the reaction,$A \rightleftharpoons B$,$E_a = 50 \ kJ \ mol^{-1}$ and $\Delta H = -20 \ kJ \ mol^{-1}$. When a catalyst is added,$E_a$ decreases by $10 \ kJ \ mol^{-1}$. What is the $E_a$ for the backward reaction in the presence of the catalyst?

For an exothermic reaction $A \rightarrow B$,the activation energy is $15 \, K \, cal/mol$ and the heat of reaction is $5 \, K \, cal/mol$. The activation energy for the reverse reaction $B \rightarrow A$ will be ......... $K \, cal/mol$.

For an endothermic reaction,the energy of activation is $E_a$ and the enthalpy of reaction is $\Delta H$ (both in $kJ/mol$). The minimum value of $E_a$ will be:

An increase in temperature by $10\,^{\circ}C$,generally increases the rate of a reaction by .......... times.

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