For a reverse reaction, `A rarr B,` which one of the following statement is wrong from the given energy. Profile diagram?

Options

A. Activation energy of forward reaction is greater than backward reaction
B. The forward reaction is endothermic
C. The threshold energy is less than that of activation energy
D. The energy of activation of forward reaction is equal to the sum of heat of reaction and the energy of activation of backward reaction

Explanation

To solve the question regarding the energy profile diagram for the reverse reaction \( A \rightarrow B \), we will analyze the energy changes involved in the reaction and identify which statement is incorrect based on the energy profile.

### Step-by-Step Solution:

1. **Understanding the Energy Profile Diagram**:
- The energy profile diagram typically plots the potential energy of the reactants and products against the reaction coordinate.
- On the left side, we have the energy of reactants (A), and on the right side, we have the energy of products (B).

2. **Identifying Activation Energies**:
- The activation energy for the forward reaction (from A to B) is represented as \( E_A \).
- The activation energy for the reverse reaction (from B to A) is represented as \( E_{A'} \).

3. **Analyzing Energy Levels**:
- If the energy of product B is higher than that of reactant A, it indicates that the reaction is endothermic in the forward direction.
- The difference in energy between the reactants and products gives us the overall energy change for the reaction.

4. **Determining Threshold Energy**:
- The threshold energy is the minimum energy required to initiate the reaction. It is represented by the peak of the energy profile.
- The activation energy for the forward reaction is the energy difference between the reactants and the peak, while the activation energy for the reverse reaction is the energy difference between the products and the peak.

5. **Conclusion on Statements**:
- If the potential energy of the product (B) is greater than that of the reactant (A), then the activation energy for the reverse reaction (\( E_{A'} \)) will be less than the activation energy for the forward reaction (\( E_A \)).
- Therefore, any statement claiming that the activation energy for the reverse reaction is greater than that for the forward reaction would be incorrect.