(D) The activation energy for the reverse reaction depends on the enthalpy change $(\Delta H)$ of the reaction. For an endothermic reaction,$\Delta H

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can be less than or more than $E_a$

(D) The activation energy for the reverse reaction depends on the enthalpy change $(\Delta H)$ of the reaction. For an endothermic reaction,$\Delta H > 0$,so $E_{a(\text{reverse})} = E_{a(\text{forward})} - \Delta H$,which is less than $E_a$. For an exothermic reaction,$\Delta H Therefore,the activation energy in the reverse direction can be less than or more than $E_a$.

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

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For a chemical reaction $A \rightarrow B$,the activation energy in the forward direction is $E_a$. Then the activation energy in the reverse direction is.........

A
will be double of $E_a$
B
will be equal to $-E_a$
C
will always be less than $E_a$
D
can be less than or more than $E_a$

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Class 12

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

At room temperature,the reaction between $NO$ and $O_2$ to form $NO_2$ is fast,whereas the reaction between $CO$ and $O_2$ is slow because:

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For the reaction $X \rightleftharpoons Y$,the pre-exponential factors for the forward and backward reactions are equal. What will be the equilibrium constant of the reaction?

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Activation energy is defined as:

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The variation of the rate constant with temperature is given by the Arrhenius equation $k = A e^{-E_a / (RT)}$. If $T \to \infty$,the rate constant $k$ will be equal to:

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In a multistep reaction such as $A + B$ $\longrightarrow Q$ $\longrightarrow C$,the potential energy diagram is shown below. What is $E_{a}$ for the reaction $Q \longrightarrow C$?

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For a chemical reaction $A \rightarrow B$,the activation energy in the forward direction is $E_a$. Then the activation energy in the reverse direction is.........

Similar Questions

At room temperature,the reaction between $NO$ and $O_2$ to form $NO_2$ is fast,whereas the reaction between $CO$ and $O_2$ is slow because:

For the reaction $X \rightleftharpoons Y$,the pre-exponential factors for the forward and backward reactions are equal. What will be the equilibrium constant of the reaction?

Activation energy is defined as:

The variation of the rate constant with temperature is given by the Arrhenius equation $k = A e^{-E_a / (RT)}$. If $T \to \infty$,the rate constant $k$ will be equal to:

In a multistep reaction such as $A + B$ $\longrightarrow Q$ $\longrightarrow C$,the potential energy diagram is shown below. What is $E_{a}$ for the reaction $Q \longrightarrow C$?

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