A reaction having equal energies of activation for forward and reverse reactions has

Options

A. `DeltaS=0`
B. `DeltaG=0`
C. `DeltaH=0`
D. `DeltaH=DeltaG=DeltaV=0`

Explanation

To solve the question regarding a reaction with equal energies of activation for the forward and reverse reactions, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Activation Energy**:
- Activation energy (Ea) is the minimum energy required for a reaction to occur. For a reaction, we have two activation energies: one for the forward reaction (Ea_forward) and one for the reverse reaction (Ea_reverse).

2. **Given Condition**:
- The problem states that the activation energies for the forward and reverse reactions are equal:
\[ Ea_{forward} = Ea_{reverse} \]

3. **Relation Between Activation Energy and Enthalpy Change**:
- The relationship between activation energies and the change in enthalpy (ΔH) is given by:
\[ Ea_{reverse} = Ea_{forward} + \Delta H \]
- Since we know that \(Ea_{forward} = Ea_{reverse}\), we can substitute this into the equation:
\[ Ea_{forward} = Ea_{forward} + \Delta H \]

4. **Solving for ΔH**:
- Rearranging the equation gives:
\[ 0 = \Delta H \]
- Therefore, we conclude that:
\[ \Delta H = 0 \]

5. **Conclusion**:
- Since the enthalpy change (ΔH) is zero, this indicates that the energy of the products is equal to the energy of the reactants. This means that the reaction is at equilibrium, and there is no net change in energy.

### Final Answer:
The correct answer is that the reaction has:
\[ \Delta H = 0 \]