Consider the following information.

The lattice energy of $CsCl$ is $H_{\text{l}\text{a}\text{t}\text{t}\text{i}\text{c}\text{e}}=-657k\frac{J}{m}ol.$

The enthalpy of sublimation of Cs is $H_{\text{s}\text{u}\text{b}}=76\mathrm{.}5k\frac{J}{m}ol.$

The first ionization energy of $Cs$ is $I{E}_1=376k\frac{J}{m}ol.$

The electron affinity of $Cl$ is $H_{EA}=-349k\frac{J}{m}ol.$

The bond energy of $C{l}_2$ is $BE=243k\frac{J}{m}ol.$

Determine the enthalpy of formation, $H_f,$ for $CsCl(s).$

$H_f=$

$k\frac{J}{m}ol$