Question

In: Chemistry

What is ΔGrxno (in kJ) at 1354 K for the following reaction? 2POCl3(g) → 2PCl3(g) +...

What is ΔGrxno (in kJ) at 1354 K for the following reaction?

2POCl3(g) → 2PCl3(g) + O2(g)

POCl3(g): ΔHfo = -592.7 kJ/mol and Sº = 324.6 J/K mol)
PCl3(g): ΔHfo = -287.0 kJ/mol and Sº = 311.7 J/K mol)
O2(g): ΔHfo = ? kJ/mol and Sº = 205.0 J/K mol)

Expert Solution

we have:

Hof(POCl3(g)) = -592.7 KJ/mol

Hof(PCl3(g)) = -287.0 KJ/mol

Hof(O2(g)) = 0.0 KJ/mol

we have the Balanced chemical equation as:

2 POCl3(g) ---> 2 PCl3(g) + O2(g)

deltaHo rxn = 2*Hof(PCl3(g)) + 1*Hof(O2(g)) - 2*Hof( POCl3(g))

deltaHo rxn = 2*(-287.0) + 1*(0.0) - 2*(-592.7)

deltaHo rxn = 611.4 KJ/mol

we have:

Sof(POCl3(g)) = 324.6 J/mol.K

Sof(PCl3(g)) = 311.7 J/mol.K

Sof(O2(g)) = 205.0 J/mol.K

we have the Balanced chemical equation as:

2 POCl3(g) ---> 2 PCl3(g) + O2(g)

deltaSo rxn = 2*Sof(PCl3(g)) + 1*Sof(O2(g)) - 2*Sof( POCl3(g))

deltaSo rxn = 2*(311.7) + 1*(205.0) - 2*(324.6)

deltaSo rxn = 179.2 J/mol.K

deltaH = 611.4 KJ/mol

deltaS = 179.2 J/mol.K= 0.1792 KJ/mol.K

T = 1354 K

we have below equation to be used:

deltaG = deltaH - T*deltaS

deltaG = 611.4 - 1354.0 * 0.1792

deltaG = 368.8 KJ/mol

Answer: 368.8 KJ/mol

queen_honey_blossom answered 2 years ago

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