If the enthalpy of sublimation of Li is 155 kJ mol^-1, enthalpy of dissociation of F_2 is 150 kJ mol^-1, ionization enthalpy of Li is 520 kJ mol^-1,…

If the enthalpy of sublimation of Li is $\displaystyle 155 \mathrm{~kJ} \mathrm{~mol}^{-1}$, enthalpy of dissociation of $\displaystyle \mathrm{F}_2$ is $\displaystyle 150 \mathrm{~kJ} \mathrm{~mol}^{-1}$, ionization enthalpy of Li is $\displaystyle 520 \mathrm{~kJ} \mathrm{~mol}^{-1}$, electron gain enthalpy of F is $\displaystyle -313 \mathrm{~kJ} \mathrm{~mol}^{-1}$, standard enthalpy of formation of LiF is -$\displaystyle 594$ $\displaystyle \mathrm{kJ} \mathrm{mol}^{-1}$. The magnitude of lattice enthalpy of LiF is $\displaystyle \_\_\_\_$ $\displaystyle \mathrm{kJ} \mathrm{mol}^{-1}$. (Nearest Integer)