Chemical Thermodynamics: JEE Main 2023 Chemistry question

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