Identify the reaction for which `Delta H != Delta E`

Options

A. `s("rhombic") + O_(2)(g) rarr SO_(2)(g)`
B. `N_(2)(g) + O_(2)(g) rarr 2NO(g)`
C. `H_(2)(g) + Cl_(2)(g) rarr 2HCl(g)`
D. `CO(g) + 1/2 O_(2)(g) rarr CO_(2)(g)`

Explanation

To identify the reaction for which ΔH is not equal to ΔE, we need to analyze the relationship between the change in enthalpy (ΔH) and the change in internal energy (ΔE) for different reactions. The relationship can be summarized by the equation:

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

Where:
- ΔN_g = Number of moles of gaseous products - Number of moles of gaseous reactants
- R = Universal gas constant (8.314 J/mol·K)
- T = Temperature in Kelvin

From this equation, we can conclude that:
- If ΔN_g = 0, then ΔH = ΔE
- If ΔN_g ≠ 0, then ΔH ≠ ΔE

Now, let's analyze the provided reactions one by one to determine ΔN_g for each reaction.

### Step 1: Analyze each reaction

1. **Reaction A**:
\[ \text{S (s)} + \text{O}_2 (g) \rightarrow \text{SO}_2 (g) \]
- Gaseous products: 1 (SO₂)
- Gaseous reactants: 1 (O₂)
- ΔN_g = 1 - 1 = 0

**Conclusion**: ΔH = ΔE (not the answer).

2. **Reaction B**:
\[ \text{N}_2 (g) + \text{O}_2 (g) \rightarrow 2 \text{NO} (g) \]
- Gaseous products: 2 (NO)
- Gaseous reactants: 2 (N₂ + O₂)
- ΔN_g = 2 - 2 = 0

**Conclusion**: ΔH = ΔE (not the answer).

3. **Reaction C**:
\[ \text{H}_2 (g) + \text{Cl}_2 (g) \rightarrow 2 \text{HCl} (g) \]
- Gaseous products: 2 (HCl)
- Gaseous reactants: 2 (H₂ + Cl₂)
- ΔN_g = 2 - 2 = 0

**Conclusion**: ΔH = ΔE (not the answer).

4. **Reaction D**:
\[ \text{CO} (g) + \frac{1}{2} \text{O}_2 (g) \rightarrow \text{CO}_2 (g) \]
- Gaseous products: 1 (CO₂)
- Gaseous reactants: 1.5 (CO + 0.5 O₂)
- ΔN_g = 1 - 1.5 = -0.5 (not equal to 0)

**Conclusion**: ΔH ≠ ΔE (this is the answer).

### Final Answer:
The reaction for which ΔH is not equal to ΔE is:
\[ \text{CO} (g) + \frac{1}{2} \text{O}_2 (g) \rightarrow \text{CO}_2 (g) \]