Which of the following is true for a reaction in which all the reactant & product are liquids

Options

A. `DeltaH=DeltaE`
B. `DeltaH`=`DeltaW`
C. `DeltaHgtDeltaE`
D. None of the above

Answer

To solve the question regarding the relationship between enthalpy (ΔH) and internal energy (ΔE) for a reaction where all reactants and products are liquids, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Reaction**:
- We are dealing with a reaction where all reactants and products are in the liquid state. This means that there are no gaseous reactants or products involved in the reaction.

2. **Identifying the Change in Moles**:
- In thermodynamics, the change in the number of moles of gas (Δng) is important for understanding the relationship between enthalpy and internal energy.
- Since all species are liquids, we can conclude that Δng = 0 because there are no gaseous products or reactants.

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

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

5. **Conclusion**:
- Therefore, for a reaction where all reactants and products are liquids, the enthalpy change (ΔH) is equal to the internal energy change (ΔE). This means that the correct answer to the question is that ΔH = ΔE.

### Final Answer:
The correct statement for a reaction in which all the reactants and products are liquids is:
**ΔH = ΔE**