Use the following to calculate H°lattice of MgF2. Mg(s) Mg(g) H° = 148 kJ F2(g) 2 F(g) H° = 159 kJ Mg(g) Mg+(g) + e- H° = 738 kJ Mg+(g) Mg+2(g) + e- H° = 1450 kJ F(g) + e- F -(g) H° = -328 kJ Mg(s) + F2(g) MgF2(s) H° = -1123 kJ kJ/mol

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jbferrado jbferrado · Answer 1 · 2019-11-25T19:41:10+01:00

Answer:

The correct answer is -2952 KJ/mol

Explanation:

Attached is the diagram for Born- Haber cycle. According to the cycle:

ΔHf= ΔH1 + ΔH2 + ΔH3 + ΔH4 + ΔH5 + LE

In order to calculate the lattice energy (LE):

LE= ΔHf - ΔH1 - ΔH2 - ΔH3 - ΔH4 - ΔH5

LE= -1123 KJ/mol - 148 KJ/mol - 159 KJ/mol - 728 KJ/mol - 1450 KJ/mol - (2 x (-328 KJ/mol)

LE= -2952 KJ/mol

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nikitarahangdaleVT nikitarahangdaleVT · Answer 2 · 2022-03-23T09:28:57+01:00

The lattice energy of MgF₂ is -2952 KJ/mol which can be calculated by using given values.

Lattice energy for the given question will be calculated by using the Born Haber cycle equation as:

ΔH₀ = ΔH₁ + ΔH₂ + ΔH₃ + ΔH₄ + ΔH₅ + Lattice Energy

Lattice Energy = ΔH₀ - ΔH₁ - ΔH₂ - ΔH₃ - ΔH₄ - ΔH₅, where

According to question,

ΔH₀ = -1123 kJ/mol

ΔH₁ = 148 kJ/mol

ΔH₂ = 159 kJ/mol

ΔH₃ = 738 kJ/mol

ΔH₄ = 1450 kJ/mol

ΔH₅ = -328 kJ/mol (In the cycle 2 moles of fluorine is present so we multiply this value by 2)

On putting all these values on the above equation we get,

L.E = -1123 KJ/mol - 148 KJ/mol - 159 KJ/mol - 728 KJ/mol - 1450 KJ/mol - (2 x (-328 KJ/mol)

L.E = -2952 KJ/mol

Hence, -2952 KJ/mol is the lattice energy.

To know more about Born Haber cycle, visit the below link:

https://brainly.com/question/11730518