(A) The enthalpy change $(\Delta H)$ of a reaction is given by the difference between the activation energy of the forward reaction $(E_{af})$ and the

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(A) The enthalpy change $(\Delta H)$ of a reaction is given by the difference between the activation energy of the forward reaction $(E_{af})$ and the activation energy of the backward reaction $(E_{ab})$.$\Delta H = E_{af} - E_{ab}$Given $E_{af} = 50 \ kJ$ and $E_{ab} = 30 \ kJ$.$\Delta H = 50 \ kJ - 30 \ kJ = 20 \ kJ$.Since $\Delta H$ is positive,the reaction is endothermic.

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

Easy

Given the activation energy for the forward direction $(E_{af})$ is $50 \ kJ$ and for the backward direction $(E_{ab})$ is $30 \ kJ$. The reaction would be:

A
Endothermic
B
Exothermic
C
Can't be predicted
D
Equilibrium

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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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MediumJEE MAIN 2022

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KVPY 2019

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Given the activation energy for the forward direction $(E_{af})$ is $50 \ kJ$ and for the backward direction $(E_{ab})$ is $30 \ kJ$. The reaction would be:

Similar Questions

How much faster would a reaction proceed at $25\,^{\circ}C$ than at $0\,^{\circ}C$ if the activation energy is $65\,kJ/mol$?

The temperature coefficient of a reaction is defined as:

In a reaction,the rate of reaction doubles with a $10^\circ C$ rise in temperature. If the temperature is increased from $10^\circ C$ to $100^\circ C$,by how many times will the rate of reaction increase?

For a reaction,given below is the graph of $\ln k$ vs $\frac{1}{T}$. The activation energy for the reaction is equal to $...... \ cal \ mol^{-1}$. (Nearest integer). (Given : $R = 2 \ cal \ K^{-1} \ mol^{-1}$)

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