6 HNO3 (aq) + 5 H2C2O4 (aq) + 2 KMnO4 (aq) → 10 CO2 (g) + 2 Mn(NO3)2 (aq) + 2 KNO3 (aq) + 8 H2O (ℓ)

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Stoichiometry

Enter a mass or volume in one of the boxes below. Upon hitting submit, the stoichiometric equivalents will be calculated for the remaining reactants and products. All gases are assumed to be at STP.

HNO3           Mass: g  or Solution Volume: mL of Concentration: mol/L
H2C2O4         Mass: g  or Solution Volume: mL of Concentration: mol/L
KMnO4          Mass: g  or Solution Volume: mL of Concentration: mol/L
CO2            Mass: g  or Gas Volume: L
Mn(NO3)2       Mass: g  or Solution Volume: mL of Concentration: mol/L
KNO3           Mass: g  or Solution Volume: mL of Concentration: mol/L
H2O            Mass: g

Enthalpy of Reaction

[10ΔHf(CO2 (g)) + 2ΔHf(Mn(NO3)2 (aq)) + 2ΔHf(KNO3 (aq)) + 8ΔHf(H2O (ℓ))] - [6ΔHf(HNO3 (aq)) + 5ΔHf(H2C2O4 (aq)) + 2ΔHf(KMnO4 (aq))]
[10(-393.51) + 2(-635.55) + 2(-459.76) + 8(-285.83)] - [6(-207.36) + 5(-825.1) + 2(-793.81)] = -1455.08 kJ
-1,455.08 kJ     (exothermic)

Entropy Change

[10ΔSf(CO2 (g)) + 2ΔSf(Mn(NO3)2 (aq)) + 2ΔSf(KNO3 (aq)) + 8ΔSf(H2O (ℓ))] - [6ΔSf(HNO3 (aq)) + 5ΔSf(H2C2O4 (aq)) + 2ΔSf(KMnO4 (aq))]
[10(213.68) + 2(219.24) + 2(248.94) + 8(69.91)] - [6(146.44) + 5(45.6) + 2(293.71)] = 1938.38 J/K
1,938.38 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[10ΔGf(CO2 (g)) + 2ΔGf(Mn(NO3)2 (aq)) + 2ΔGf(KNO3 (aq)) + 8ΔGf(H2O (ℓ))] - [6ΔGf(HNO3 (aq)) + 5ΔGf(H2C2O4 (aq)) + 2ΔGf(KMnO4 (aq))]
[10(-394.38) + 2(-450.71) + 2(-394.64) + 8(-237.18)] - [6(-111.34) + 5(-673.9) + 2(-730.57)] = -2033.26 kJ
-2,033.26 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-2033.01 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)