The enthalpy of solution of sodium chloride is `4 kJ mol^(-1)` and its enthalpy of hydration of ion is `-784 kJ mol^(-1)`. Then the lattice enthalpy of `NaCl` (in `kJ mol^(-1)`) is

The enthalpy of solution of sodium chloride is 4 kj mol^-1 and its enthalpy of hydration of ions is -784 kJ mol^-1 .Then the lattice enthalpy of NaCl (in kJ mol^-1 ) is (1) +788 (2) +4 (3) +398 (4) +780 +394

Lattice energy of NaCl(s) is -790 kJ " mol"^(-1) and enthalpy of hydration is -785 kJ " mol"^(-1) . Calculate enthalpy of solution of NaCl(s).

Lattice energy of NaCl(s) is -790 kJ " mol"^(-1) and enthalpy of hydration is -785 kJ " mol"^(-1) . Calculate enthalpy of solution of NaCl(s).

Lattice energy of NaCl_((s)) is -788kJ mol^(-1) and enthalpy of hydration is -784kJ mol^(-1) . Calculate the heat of solution of NaCl_((s)) .

Lattice energy of NaCl_((s)) is -788kJ mol^(-1) and enthalpy of hydration is -784kJ mol^(-1) . Calculate the heat of solution of NaCl_((s)) .

The enthalpy of neutralisation of a strong acid by a string base is -57.32 kJ mol^(-1) . The enthalpy of formation of water is -285.84 kJ mol^(-1) . The enthalpy of formation of hydroxy 1 ion is

The enthalpy of neutralisation of a strong acid by a strong base is -57.32 kJ mol^(-1) . The enthalpy of formation of water is -285.84 kJ mol^(-1) . The enthalpy of formation of hydroxyl ion is