(A) The enthalpy of sublimation of cesium is 78.2 kJ mol -1 , and f H[CsCl(s)]...

(A) The enthalpy of sublimation of cesium is 78.2 kJ mol^-1, and Δ_fH°[CsCl(s)] = -442.8 kJ mol^-1. Use these values, together with other data from the text, to calculate the lattice energy of CsCl(s).

(B) Given the following data, together with data included in Example 12-12, calculate Δ_fH° of CaCl₂(s): Enthalpy of sublimation of Ca(s), +178.2 kJ mol^-1; first ionization energy of Ca(g), +590 kJ mol^-1 ; second ionization energy of Ca(g), +1145 kJ mol^-1; lattice energy of CaCl₂(s), -2223 kJ mol^-1.

Example 12-12

With the following data, calculate Δ_fH° of MgCl(s): Enthalpy of sublimation of Mg(s): +146 kJ mol^-1; enthalpy of dissociation of Cl₂(g): +244 kJ mol^-1 ; first ionization energy of Mg(g): +738 kJ mol^-1; electron affinity of Cl(g): -349 kJ mol^-1; lattice energy of MgCl(s): -676 kJ mol^-1.