Lattice Enthalpy — MCQ Practice

Given the following standard enthalpy changes for the formation of potassium iodide (KI): Enthalpy of sublimation of K(s) = $+89\,\text{kJ/mol}$ Ionization enthalpy of K(g) = $+419\,\text{kJ/mol}$ Dissociation enthalpy of $I_2(g)$ = $+151\,\text{kJ/mol}$ Electron gain enthalpy of I(g) = $-295\,\text{kJ/mol}$ Standard enthalpy of formation of KI(s) = $-327\,\text{kJ/mol}$ Calculate the lattice enthalpy of KI(s).

Which of the following ionic compounds is expected to have the highest magnitude of lattice enthalpy?

Which of the following statements about lattice enthalpy is INCORRECT?

Arrange the following ionic compounds in increasing order of their lattice enthalpy magnitude: NaCl, CsCl, LiCl, KCl.

Which of the following processes represents the lattice enthalpy of magnesium oxide (MgO)?

Given the following data, calculate the second electron gain enthalpy of oxygen ($O^-(g) + e^- \rightarrow O^{2-}(g)$): $\Delta H_f^\circ (MgO(s)) = -602\,\text{kJ/mol}$ $\Delta H_{sub} (Mg(s)) = +148\,\text{kJ/mol}$ $IE_1 (Mg(g)) = +738\,\text{kJ/mol}$ $IE_2 (Mg(g)) = +1451\,\text{kJ/mol}$ $\Delta H_{diss} (O_2(g)) = +498\,\text{kJ/mol}$ $EA_1 (O(g)) = -141\,\text{kJ/mol}$ $\Delta H_{lattice} (MgO(s)) = -3791\,\text{kJ/mol}$