## 2 N2H4 (ℓ) + 1 N2O4 (ℓ) → 3 N2 (g) + 4 H2O (g)

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## Stoichiometry

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 N2H4           Mass: g N2O4           Mass: g N2             Mass: g or Gas Volume: L H2O            Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[3ΔHf(N2 (g)) + 4ΔHf(H2O (g))] - [2ΔHf(N2H4 (ℓ)) + 1ΔHf(N2O4 (ℓ))]
[3(0) + 4(-241.82)] - [2(50.63) + 1(-19.58)] = -1048.96 kJ
-1,048.96 kJ     (exothermic)

## Entropy Change

[3ΔSf(N2 (g)) + 4ΔSf(H2O (g))] - [2ΔSf(N2H4 (ℓ)) + 1ΔSf(N2O4 (ℓ))]
[3(191.5) + 4(188.72)] - [2(121.21) + 1(209.24)] = 877.72 J/K
877.72 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[3ΔGf(N2 (g)) + 4ΔGf(H2O (g))] - [2ΔGf(N2H4 (ℓ)) + 1ΔGf(N2O4 (ℓ))]
[3(0) + 4(-228.59)] - [2(149.24) + 1(97.4)] = -1310.24 kJ
-1,310.24 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-1310.65 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

3.6048682348e+229
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 215.