Question

In: Chemistry

Given the following thermodynamic data, calculate the lattice energy of CsF: ΔH°f[CsF(s)] = -554 kJ/mol ΔH°sublimation...

Given the following thermodynamic data, calculate the lattice energy of CsF:

ΔH°f[CsF(s)] = -554 kJ/mol
ΔH°sublimation [Cs] = 76.5 kJ/mol
Bond energy [F-F] = 159 kJ/mol
IE1 (Cs) = 376 kJ/mol
EA1 (F) = -328 kJ/mol

-1414 kJ/mol

-1493 kJ/mol

-714 kJ/mol

-758 kJ/mol

-837 kJ/mol

Solutions

Expert Solution

Cs(s) + 1/2F2(g) --------------> CsF(s)           ΔH°f[CsF(s)] = -554 kJ/mol

sublimation energy

Cs(s) ------------------> Cs(g)                             ΔH°sublimation [Cs] = 76.5 kJ/mol

Cs(g) --------------> Cs^+ (g) + e^-                    IE1 (Cs) = 376 kJ/mol

bond dissociation energy

F2(g) ---------------> 2F(g)                                 Bond energy [F-F] = 159 kJ/mol

1/2F2(g) ---------------> F(g)                                 Bond energy [F-F] = 159/2kJ/mol   = 79.5Kj/mole

electron affinity

F(g) + e^- -------------->F^- (g)                             Bond energy [F-F] = -328 kJ/mol

lattice energy

Cs^+(g) + F^- (g) -----------------> CsF(s)              ΔH° lattice =

from Hess law

ΔH°f[CsF(s)]   = ΔH°sublimation [Cs] + IE1 (Cs) + Bond energy [F-F] + Bond energy [F-F] + ΔH° lattice

-554                 = 76.5 + 376 + 79.5 -328+ ΔH° lattice

ΔH° lattice         = -758Kj/mole >>>>answer

-758 kJ/mol >>>.answer

queen_honey_blossom answered 2 years ago
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