Which of the following chemical equilibrium is favoured in temperature ?

Options

A. `N_(2)O_(4) hArr 2NO_(2)DeltaH=+59kJ mol ^(-1)`
B. `N_(2)+3H_(2) hArr 2NH_(3) DeltaH=-22k cal mol^(-1)`
C. `2SO_(2)+O_(2)hArr2SO_(3) DeltaH=-47k cal mol^(-1)`
D. both 2 and 3

Explanation

To determine which chemical equilibrium is favored by an increase in temperature, we can apply Le Chatelier's principle. This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.

### Step-by-Step Solution:

1. **Identify the Nature of the Reactions**:
- Look at the enthalpy change (ΔH) values given for each reaction.
- Reactions can be classified as either endothermic (ΔH > 0) or exothermic (ΔH < 0).

2. **Analyze the Given Options**:
- **Option A**: Endothermic reaction (ΔH > 0)
- **Option B**: Exothermic reaction (ΔH < 0)
- **Option C**: Exothermic reaction (ΔH < 0)

3. **Apply Le Chatelier's Principle**:
- For endothermic reactions (like Option A), increasing the temperature will favor the forward reaction because the system will absorb the added heat.
- For exothermic reactions (like Options B and C), increasing the temperature will favor the reverse reaction as the system will try to release heat to counteract the change.

4. **Conclusion**:
- Since only Option A is endothermic, it will shift to the right (forward direction) with an increase in temperature. Therefore, the equilibrium of Option A is favored by an increase in temperature.

### Final Answer:
**The equilibrium favored by an increase in temperature is Option A (endothermic reaction).**