(B) For an exothermic reaction,the relationship between the activation energy of the forward reaction $(E_{a(f)})$,the activation energy of the backwa

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(B) For an exothermic reaction,the relationship between the activation energy of the forward reaction $(E_{a(f)})$,the activation energy of the backward reaction $(E_{a(b)})$,and the enthalpy change $(\Delta H)$ is given by:$\Delta H = E_{a(f)} - E_{a(b)}$Given:$E_{a(f)} = 65 \ kJ \ mol^{-1}$$\Delta H = -42 \ kJ \ mol^{-1}$Substituting the values:$-42 = 65 - E_{a(b)}$$E_{a(b)} = 65 + 42 = 107 \ kJ \ mol^{-1}$

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

Medium

For an exothermic reaction $A \to B$,the activation energy is $65 \ kJ \ mol^{-1}$ and the heat of reaction is $-42 \ kJ \ mol^{-1}$. The activation energy for the reverse reaction $B \to A$ would be....... $kJ \ mol^{-1}$

A
$23$
B
$107$
C
$65$
D
$42$

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

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For an exothermic reaction $A \to B$,the activation energy is $65 \ kJ \ mol^{-1}$ and the heat of reaction is $-42 \ kJ \ mol^{-1}$. The activation energy for the reverse reaction $B \to A$ would be....... $kJ \ mol^{-1}$

Similar Questions

If the definition of the temperature coefficient of the reaction holds good for a reaction between $27^{\circ} C$ and $37^{\circ} C$,the activation energy for the reaction in $kJ \cdot mol^{-1}$ is

Which statement is incorrect according to the Arrhenius equation?

The activation energy of a reaction at a given temperature is found to be $2.303 \ RT \ J \ mol^{-1}$. The ratio of rate constant to the Arrhenius factor is

Oxygen is available in plenty in air,yet fuels do not burn by themselves at room temperature. Explain.

Assertion : If the activation energy of a reaction is zero,temperature will have no effect on the rate constant.Reason : Lower the activation energy,faster is the reaction.

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Assertion : If the activation energy of a reaction is zero,temperature will have no effect on the rate constant.
Reason : Lower the activation energy,faster is the reaction.