The enthalpy change for the conversion of $\frac{1}{2} \mathrm{Cl}_2(\mathrm{~g})$ to $\mathrm{Cl}^{-}(\mathrm{aq})$ is (-) $\_\_\_\_$ $\mathrm{kJ} \mathrm{mol}^{-1}$ (Nearest integer) Given: $\Delta_{\text {dis }} \mathrm{H}_{\mathrm{C}_{2(g)}}^{\circ}=240 \mathrm{kJmol}^{-1}, \Delta_{\mathrm{eg}} \mathrm{H}_{\mathrm{C}_{(g)}}^{\circ}=-350 \mathrm{kJmol}^{-1}, \Delta_{\mathrm{hyd}} \mathrm{H}_{\mathrm{C}_{(g)}}^{\circ}=-380 \mathrm{kJmol}^{-1}$