The enthalpy change of solution of is -2 kJ/mol and the lattice dissociation enthalpy of is +772 kJ/mol. If the enthalpy of hydration of is -390 kJ/mol, what is the enthalpy of hydration of ?

Question

The enthalpy change of solution of $NaCl(s)$ is -2 kJ/mol and the lattice dissociation enthalpy of $NaCl$ is +772 kJ/mol. If the enthalpy of hydration of $Na^+(g)$ is -390 kJ/mol, what is the enthalpy of hydration of $Cl^-(g)$?

Prashant Kotian · Accepted Answer

Correct answer: A. Enthalpy of solution is the sum of lattice dissociation enthalpy and the hydration enthalpies of the separated ions. . . Solving gives kJ/mol.

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