OnlineCBT
Chemistry · THERMODYNAMICS
हिन्दीGiven that lattice enthalpy of \( \text{NaCl(s)} \) is \( +788\text{ kJ mol}^{-1} \) and hydration enthalpy \( \Delta_{\text{hyd}}H^\ominus \) of \( \text{NaCl} \) is \( -784\text{ kJ mol}^{-1} \), the standard enthalpy of solution (\( \Delta_{\text{sol}}H^\ominus \)) of \( \text{NaCl} \) is:
Correct answer · Option 3
+4 kJ mol\( ^{-1} \)
Explanation
\( \Delta_{\text{sol}}H^\ominus = \Delta_{\text{lattice}}H^\ominus + \Delta_{\text{hyd}}H^\ominus = +788 - 784 = +4\text{ kJ mol}^{-1} \).
