The enthalpy change for the conversion of \( \frac{1}{2}\text{Cl}_{2}(g) \) to \( \text{Cl}^{-}(aq) \) is \( ( - ) \) _____ \( \text{kJ mol}^{-1} \) (nearest integer):
Given: \( \Delta_{\text{dis}} H^{\theta}_{\text{Cl}_{2}(g)} = 240 \, \text{kJ mol}^{-1} \), \( \Delta_{\text{eg}} H^{\theta}_{\text{Cl}(g)} = -350 \, \text{kJ mol}^{-1} \), \( \Delta_{\text{hyd}} H^{\theta}_{\text{Cl}^{-}(g)} = -380 \, \text{kJ mol}^{-1} \)
