For which of the following change `DeltaH ne DeltaE` ?
(Where `DeltaH` is change in enthaply , `DeltaE` is change in internal energy ).

Options

A. `H_2(g)+I_2(g)rarr2HI(g)`
B. `HCl(aq)+NaOH(aq)rarrNaCl(aq)+H_2O(l)`
C. `C(s)+O_2(g)rarrCO_2(g)`
D. `N_2(g)+3H_2(g)rarr2NH_2(g)`

Answer

To determine for which of the following changes ΔH (change in enthalpy) is not equal to ΔE (change in internal energy), we will use the relationship between these two quantities:

\[ \Delta H = \Delta E + \Delta N_g RT \]

Where:
- \(\Delta N_g\) is the change in the number of moles of gaseous products minus the change in the number of moles of gaseous reactants.
- \(R\) is the gas constant.
- \(T\) is the temperature.

### Step-by-Step Solution:

1. **Identify the Reactions**: We need to analyze each reaction provided in the options to find out the value of \(\Delta N_g\).

2. **Calculate \(\Delta N_g\)**:
- **Reaction 1**: \(H_2 + I_2 \rightarrow 2HI\)
- Reactants: 1 mole of \(H_2\) + 1 mole of \(I_2\) = 2 moles (gaseous)
- Products: 2 moles of \(HI\) (gaseous)
- \(\Delta N_g = 2 - 2 = 0\)
- Conclusion: \(\Delta H = \Delta E\)

- **Reaction 2**: All reactants and products are in liquid or aqueous state.
- Since there are no gaseous reactants or products, \(\Delta N_g = 0\).
- Conclusion: \(\Delta H = \Delta E\)

- **Reaction 3**: \(A(g) \rightarrow B(g)\)
- Reactants: 1 mole of \(A\) (gaseous)
- Products: 1 mole of \(B\) (gaseous)
- \(\Delta N_g = 1 - 1 = 0\)
- Conclusion: \(\Delta H = \Delta E\)

- **Reaction 4**: \(3A(g) + B(g) \rightarrow 2C(g)\)
- Reactants: 3 moles of \(A\) + 1 mole of \(B\) = 4 moles (gaseous)
- Products: 2 moles of \(C\) (gaseous)
- \(\Delta N_g = 2 - 4 = -2\)
- Conclusion: \(\Delta H \neq \Delta E\)

3. **Final Conclusion**: The only reaction where \(\Delta H\) is not equal to \(\Delta E\) is in Reaction 4.

### Answer:
The correct option is **Reaction 4**.