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 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 ion is -784 kJ mol^(-1) . Then the lattice enthalpy of NaCl (in kJ mol^(-1) ) is

The lattice enthalpy of solid NaCl is 772 kJ mol^(-1) and enthalpy of solution is 2 kJmol^(-1) . If the hydration enthaply of Na^(+) & Cl^(-) ions are in the ratio of 3 : 2.5 , what is the enthalpy of hydration of chloride ion ?

The lattice enthalpy of solid NaCI is 772 kJ mol^(-1) and enthalpy of solution is 2kJ mol^(-1) . If the hydration enthalpy of Na^(+) &CI^(-) ions are in the ratio of 3: 25, what is the magnitude of enthalpy of hydration (in kJ) of chloride ion ?