In a reaction, all reactant and products are liquid, then

Options

A. `Delta H gt Delta E`
B. `Delta H lt Delta E`
C. `Delta H = Delta E`
D. Can't predicted

Answer

To solve the question, we need to analyze the relationship between the change in enthalpy (ΔH) and the change in internal energy (ΔE) for a reaction where all reactants and products are in the liquid phase.

### Step-by-Step Solution:

1. **Understanding the Reaction**:
- The question states that all reactants and products are liquids. This means we are dealing with a reaction where no gases are involved.

2. **Identifying Δn**:
- Δn is defined as the change in the number of moles of gas during the reaction. Since all species are in the liquid phase, there are no gaseous reactants or products.
- Therefore, Δn (the change in the number of moles of gas) is equal to 0.

3. **Using the Relationship Between ΔH and ΔE**:
- The relationship between the change in enthalpy (ΔH) and the change in internal energy (ΔE) is given by the equation:
\[ ΔH = ΔE + Δn \cdot R \cdot T \]
- Here, R is the universal gas constant and T is the temperature in Kelvin.

4. **Substituting Δn into the Equation**:
- Since we have established that Δn = 0, we can substitute this into the equation:
\[ ΔH = ΔE + 0 \cdot R \cdot T \]
- This simplifies to:
\[ ΔH = ΔE \]

5. **Conclusion**:
- From our analysis, we conclude that when all reactants and products are in the liquid phase, the change in enthalpy (ΔH) is equal to the change in internal energy (ΔE).
- Therefore, the correct answer is:
\[ \text{ΔH = ΔE} \]

### Final Answer:
C) ΔH = ΔE