We’re being asked to **calculate the lattice energy** of **calcium chloride (CaCl _{2})**.

Recall that ** lattice energy** is the energy required to combine two gaseous ions into a solid ionic compound:

M^{x+}(g) + N^{y–}(g) → M_{y}N_{x}(s)

To calculate for lattice energy, we need to do the ** Born-Haber cycle for CaCl_{2}**.

We start with the corresponding formation equation for CaCl_{2}:

Ca(s) + Cl_{2}(g) → CaCl_{2}(s), **ΔH˚ _{f}**

Calculate the lattice energy of calcium chloride given that the heat of sublimation of Ca is 121 kJ/mol and ΔH°_{f}(CaCl_{2}) = -795kJ/mol.

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Our tutors have indicated that to solve this problem you will need to apply the Born Haber Cycle concept. You can view video lessons to learn Born Haber Cycle. Or if you need more Born Haber Cycle practice, you can also practice Born Haber Cycle practice problems.

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