Use the following data to calculate the lattice energy of lithium chloride, LiCl. $$\begin{array} { l c }
{ \text { Quantity } } & \text { Magnitude } ( \mathbf { k J } / \mathbf { m o l } ) \
\text { Ionization energy of } \mathrm { Li } ( g ) & 519 \
\text { Electron affinity of } \mathrm { Cl } ( g ) & - 349 \
\text { Vaporization energy of } \mathrm { Li } ( s ) & 147 \
\text { Bond energy of } \mathrm { Cl } _ { 2 } ( g ) & 240 \
\text { Reaction enthalpy: } \mathrm{Li}(s)+\frac{1}{2} \mathrm{Cl}_{2}(g) \rightarrow \mathrm{LiCl}(s)& - 409
\end{array}$$
A) -603 kJ/mol
B) -11.0 kJ/mol
C) +405 kJ/mol
D) -846 kJ/mol
E) -131 kJ/mol

Question

Use the following data to calculate the lattice energy of lithium chloride, LiCl. $$\begin{array} { l c } 
 { \text { Quantity } } & \text { Magnitude } ( \mathbf { k J } / \mathbf { m o l } ) \
\text { Ionization energy of } \mathrm { Li } ( g ) & 519 \
\text { Electron affinity of } \mathrm { Cl } ( g ) & - 349 \
\text { Vaporization energy of } \mathrm { Li } ( s ) & 147 \
\text { Bond energy of } \mathrm { Cl } _ { 2 } ( g ) & 240 \
\text { Reaction enthalpy: } \mathrm{Li}(s)+\frac{1}{2} \mathrm{Cl}_{2}(g) \rightarrow \mathrm{LiCl}(s)& - 409
\end{array}$$
A) -603 kJ/mol
B) -11.0 kJ/mol
C) +405 kJ/mol
D) -846 kJ/mol
E) -131 kJ/mol

Quizplus · Accepted Answer

The lattice energy can be calculated using the Born-Haber cycle: Lattice Energy = ΔHf - (Ionization Energy + Electron Affinity + Vaporization Energy + 1/2 Bond Energy). Substituting the given values: -409 - (519 - 349 + 147 + 120) = -846 kJ/mol.

Use the Following Data to Calculate the Lattice Energy of Lithium