At 25°C, the enthalpy of the following processes are given:
$$H_2(g) + O_2(g) \rightarrow 2OH(g) \quad \Delta H^o = 78 \text{ kJ mol}^{-1}$$
$$H_2(g) + \frac{1}{2}O_2(g) \rightarrow H_2O(g) \quad \Delta H^o = -242 \text{ kJ mol}^{-1}$$
$$H_2(g) \rightarrow 2H(g) \quad \Delta H^o = 436 \text{ kJ mol}^{-1}$$
$$\frac{1}{2}O_2(g) \rightarrow O(g) \quad \Delta H^o = 249 \text{ kJ mol}^{-1}$$
What would be the value of X for the following reaction? (Nearest integer)
$$H_2O(g) \rightarrow H(g) + OH(g) \quad \Delta H^o = X \text{ kJ mol}^{-1}$$