The heat of formation of crystalline sodium chloride is `-410 kJ mol^(-1)`. The heat of sublimation of sodium metal is `108.8 kJ mol^(-1)`. The heat of dissociation of chlorine gas into atoms is `242.7 kJ mol^(-1)`. The ionisation energy of `Na` and electron affinity of `Cl` are `493. 7 kJ` and `-368.2 kJ` respectively. Calculate the lattice energy of `NaCl`.

When a mole of crystalline sodium chloride is prepared, 410 kJ of heat is produced. The heat of sublimation of sodium metal is 180.8kJ . The heat of dissociation fo chloride gas into atoms is 242.7kJ . The ionisation energy of Na and electron affinity of CI are 493.kJ and -368.2 kJ , respectively. calculate the lattice enegry of NaCI .

When a mole of crystalline sodium chloride is prepared, 410 kJ of heat is produced. The heat of sublimation of sodium metal is 180.8kJ . The heat of dissociation fo chlorine gas into chlorine atoms is 242.7kJ . The ionization energy of Na and electron affinity of Cl are 493.kJ and -368.2 kJ , respectively. calculate the lattice enegry of NaCl .

The standard heat of sublimation of sodium metal is 108.4 kJ*mol^(-1) . What is its standard heat of atomisation?

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.

The heat of combustion of carbon and monoxide are -394 and -285 KJ mol^(-1) respectively. The heat of formation of CO in KJ mol^(-1) is :-

The heat of combustion of carbon and monoxide are -394 and -285 KJ mol^(-1) respectively. The heat of formation of CO 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