Chemistry · CHEMICAL BONDING AND MOLECULAR STRUCTURE

Given the net enthalpy for \( \text{Na}^+(\text{g}) + \text{Cl}^-(\text{g}) \) formation from atoms is \( +147.1\text{ kJ mol}^{-1} \) and the enthalpy of lattice formation of \( \text{NaCl(s)} \) is \( -788.0\text{ kJ mol}^{-1} \), what is the total enthalpy change (\( \Delta H_{\text{rxn}} \)) for \( \text{Na(g)} + \text{Cl(g)} \to \text{NaCl(s)} \)?

1. \( +640.9\text{ kJ mol}^{-1} \)
2. \( -935.1\text{ kJ mol}^{-1} \)
3. \( +788.0\text{ kJ mol}^{-1} \)
4. \( -640.9\text{ kJ mol}^{-1} \)