## Related questions with answers

Determine the molar enthalpy of formation, $\Delta_f H^{\circ}$, of solid lithium fluoride from the lattice energy (table below) and other thermochemical data. The enthalpy of formation of ${Li}({g}), \Delta_f H^{\circ}[{Li}({g})]=$ 159.37 kJ/mol. Other required data can be found in Appendices F and L.

Lattice Energies of Some Ionic Compounds

$\begin{array}{l|r} \hline \text { Compound } & \begin{array}{r} \Delta_{\text {lattice }} U \\ (\mathrm{~kJ} / \mathrm{mol}) \end{array} \\ \hline \mathrm{LiF} & -1037 \\ \hline \mathrm{LiCl} & -852 \\ \hline \mathrm{LiBr} & -815 \\ \hline \mathrm{Lil} & -761 \\ \hline \mathrm{NaF} & -926 \\ \hline \mathrm{NaCl} & -786 \\ \hline \mathrm{NaBr} & -752 \\ \hline \mathrm{Nal} & -702 \\ \hline \mathrm{KF} & -821 \\ \hline \mathrm{KCl} & -717 \\ \mathrm{KBr} & -689 \\ \mathrm{KI} & -649 \\ \hline \end{array}$

Solution

VerifiedThe problem asks to determine the molar enthalpy of formation of solid lithium fluoride ($\mathrm{LiF}$) from a set of thermochemical data and its lattice energy.

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