Calculate the lattice energy (kJ/mol) of the hypothetical ionic compound MX from the information given below....

Calculate the lattice energy (kJ/mol) of the hypothetical ionic compound MX from the information given below. IE1(M) = 499 kJ/mol M(s) => M(g) ΔHo = 70.6 kJ/mol ΔHof(MX) = -147.5 kJ/mol X2(g) => 2X(g) ΔH = 179 kJ EA (X) = -352 kJ/mol IE1 (X) = 271 kJ/mol

Answer is -455 ± 2%

Please show all work

Expert Solution

The Lattice energy can be calculated via:

dHf = dHsub + IE + dH(X-X) + EA + U

where U is the value of interest

list:

Heat of formation = -147.5 kJ/mol (energy required to form element)

Het of atomization = 70.6 kJ/mol (energy from solid to gas)

Dissociation Energy = 179 kJ/mol (energy required to split X2 to 2X)

Sum of ionization energes = IE1(M) + IE1(X) = 499 + 271 = 770 kJ/mol

Sum of Electorn affinites (of the nonmetal, X) = EA(X) = -352 kJ/mol

Then

substitute

Lattice energy= Heat of formation- Heat of atomization- Dissociation energy- (sum of Ionization energies)- (sum of Electron Affinities)

dHf = dHsub + IE + dH(X-X) + EA + U

U = dHf - (dHsub + IE(M) + dH(X-X) + EA)

U = (-147.5) - (70.6 + 499 + 1/2*179 + -352) = -454.6 kJ/mol, to +/- 2 % it is correct

queen_honey_blossom answered 2 years ago

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