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 -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).

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 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 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 ?

When a mole of magnesium bromide is prepared from 1 mole of magnesium and 1 mole of liquid bromine, 524 kJ of energy is released. The heat of sublimation of Mg metal is 148 "kJ mol"^(-1) . The heat of dissociation of bromine gas into atoms is 193 "kJ mol"^(-1) . The heat of vaporization of liquid bromine is 31 kJ "mol"^(-1) . The ionisation energy of magnesium is 2187 kJ mol^(-1) and the electron affinity of bromine is - 662 "kJ mol"^(-1) . Calculate the lattice energy of magnesium bromide.

Heat of solution of BaCl_(2).2H_(2)O=200 kJ mol^(-1) Heat of hydration of BaCl_(2)=-150 kJ mol^(-1) Hence heat of solution of BaCl_(2) is