Chemistry Question from JEE Main 2026 · 22 January, Shift 2

If the enthalpy of sublimation of Li is $155\,\text{kJ mol}^{-1}$, enthalpy of dissociation of $\mathrm{F_2}$ is $150\,\text{kJ mol}^{-1}$, ionization enthalpy of Li is $520\,\text{kJ mol}^{-1}$, electron gain enthalpy of F is $-313\,\text{kJ mol}^{-1}$, and standard enthalpy of formation of LiF is $-594\,\text{kJ mol}^{-1}$, then the magnitude of lattice enthalpy of LiF is _____ $\text{kJ mol}^{-1}$ (Nearest integer).