## 14 HNO3 (aq) + 3 Cu2O (s) → 6 Cu(NO3)2 (aq) + 2 NO (g) + 7 H2O (ℓ)

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## Stoichiometry

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 HNO3           Mass: g or Solution Volume: mL of Concentration: mol/L Cu2O           Mass: g Cu(NO3)2       Mass: g NO             Mass: g or Gas Volume: L H2O            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[6ΔHf(Cu(NO3)2 (aq)) + 2ΔHf(NO (g)) + 7ΔHf(H2O (ℓ))] - [14ΔHf(HNO3 (aq)) + 3ΔHf(Cu2O (s))]
[6(-349.95) + 2(90.25) + 7(-285.83)] - [14(-207.36) + 3(-168.62)] = -511.11 kJ
-511.11 kJ     (exothermic)

## Entropy Change

[6ΔSf(Cu(NO3)2 (aq)) + 2ΔSf(NO (g)) + 7ΔSf(H2O (ℓ))] - [14ΔSf(HNO3 (aq)) + 3ΔSf(Cu2O (s))]
[6(193.3) + 2(210.65) + 7(69.91)] - [14(146.44) + 3(93.14)] = -259.11 J/K
-259.11 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[6ΔGf(Cu(NO3)2 (aq)) + 2ΔGf(NO (g)) + 7ΔGf(H2O (ℓ))] - [14ΔGf(HNO3 (aq)) + 3ΔGf(Cu2O (s))]
[6(-157.16) + 2(86.57) + 7(-237.18)] - [14(-111.34) + 3(-146.02)] = -433.26 kJ
-433.26 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-433.86 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

8.0926651404e+075
This process is favorable at 25°C.