Problem: Calculate the lattice energy of calcium chloride given that the heat of sublimation of Ca is 121 kJ/mol and ΔH°f(CaCl2) = -795kJ/mol.

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We’re being asked to calculate the lattice energy of calcium chloride (CaCl2)


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


Mx+(g) + Ny–(g)  MyNx(s)


To calculate for lattice energy, we need to do the Born-Haber cycle for CaCl2


We start with the corresponding formation equation for CaCl2:

Ca(s) + Cl2(g)  CaCl2(s), ΔH˚f


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Problem Details

Calculate the lattice energy of calcium chloride given that the heat of sublimation of Ca is 121 kJ/mol and ΔH°f(CaCl2) = -795kJ/mol.

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What scientific concept do you need to know in order to solve this problem?

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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Based on our data, we think this problem is relevant for Professor Davis' class at UCF.