## ZnO (s) + 1 CO (g) → Zn (s) + CO2 (g)

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## Stoichiometry

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 Heat Added: kJ ZnO            Mass: g CO             Mass: g or Gas Volume: L Zn             Mass: g CO2            Mass: g or Gas Volume: L

## Enthalpy of Reaction

[1ΔHf(Zn (s)) + 1ΔHf(CO2 (g))] - [1ΔHf(ZnO (s)) + 1ΔHf(CO (g))]
[1(0) + 1(-393.51)] - [1(-348.28) + 1(-110.54)] = 65.31 kJ
65.31 kJ     (endothermic)

## Entropy Change

[1ΔSf(Zn (s)) + 1ΔSf(CO2 (g))] - [1ΔSf(ZnO (s)) + 1ΔSf(CO (g))]
[1(41.63) + 1(213.68)] - [1(43.64) + 1(197.9)] = 13.77 J/K
13.77 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Zn (s)) + 1ΔGf(CO2 (g))] - [1ΔGf(ZnO (s)) + 1ΔGf(CO (g))]
[1(0) + 1(-394.38)] - [1(-318.32) + 1(-137.28)] = 61.22 kJ
61.22 kJ     (nonspontaneous)

From ΔG = ΔH - TΔS:
61.20 kJ     (nonspontaneous)

## Equilibrium Constant, K (at 298.15 K)

1.8798501783e-011
This process is not favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 138.