## 2 CuO (s) + 1 C (s graphite) → 2 Cu (s) + CO2 (g)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

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 CuO            Mass: g C              Mass: g Cu             Mass: g CO2            Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(Cu (s)) + 1ΔHf(CO2 (g))] - [2ΔHf(CuO (s)) + 1ΔHf(C (s graphite))]
[2(0) + 1(-393.51)] - [2(-157.32) + 1(0)] = -78.87 kJ
-78.87 kJ     (exothermic)

## Entropy Change

[2ΔSf(Cu (s)) + 1ΔSf(CO2 (g))] - [2ΔSf(CuO (s)) + 1ΔSf(C (s graphite))]
[2(33.15) + 1(213.68)] - [2(42.63) + 1(5.69)] = 189.03 J/K
189.03 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(Cu (s)) + 1ΔGf(CO2 (g))] - [2ΔGf(CuO (s)) + 1ΔGf(C (s graphite))]
[2(0) + 1(-394.38)] - [2(-129.7) + 1(0)] = -134.98 kJ
-134.98 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-135.23 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

4.4543949221e+023
This process is favorable at 25°C.

## Reference(s):

Zumdahl, Steven and Zumdahl, Susan A. Chemistry 9th ed.; Brooks/Cole: Belmont, CA, 2014; p 132.