Chemistry · THERMODYNAMICS

Given the following thermochemical equations: (i) \( \text{C}(\text{graphite}) + \text{O}_2(g) \to \text{CO}_2(g);\; \Delta_r H^\ominus = -393.5\text{ kJ mol}^{-1} \) (ii) \( \text{CO}(g) + \frac{1}{2}\text{O}_2(g) \to \text{CO}_2(g);\; \Delta_r H^\ominus = -283.0\text{ kJ mol}^{-1} \) The enthalpy change for \( \text{C}(\text{graphite}) + \frac{1}{2}\text{O}_2(g) \to \text{CO}(g) \) is:

1. A
   \( -676.5\text{ kJ mol}^{-1} \)
2. B
   \( +110.5\text{ kJ mol}^{-1} \)
3. C
   \( -283.0\text{ kJ mol}^{-1} \)
4. D
   \( -110.5\text{ kJ mol}^{-1} \)