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Calculate the lattice enthalpy of \( \mathrm{LiF} \) give that the enthalpy of (i) Sublimation of lithium is \( 155.2 \mathrm{~kJ} \mathrm{~mol}^{-1} \); (ii) Dissociation of \( 1 / 2 \) mole of \( \mathrm{F}_{2} \) is \( 75.3 \mathrm{~kJ} \); (iii) Ionization energy of lithium is \( 520 \mathrm{~kJ} \mathrm{~mol}^{-1} \); (iv) Electron gain enthalpy of \( \mathrm{F}(\mathrm{g}) \) is \( -333 \mathrm{~kJ} \mathrm{~mol}^{-1} ;(\mathrm{v}) \Delta H_{f}^{0} \) overall is \( -594.1 \mathrm{~kJ} \mathrm{~mol}^{-1} \).
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