## N2H4 (ℓ) + 1 O2 (g) → N2 (g) + H2O (ℓ)

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## Stoichiometry

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 N2H4           Mass: g O2             Mass: g or Gas Volume: L N2             Mass: g or Gas Volume: L H2O            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(N2 (g)) + 1ΔHf(H2O (ℓ))] - [1ΔHf(N2H4 (ℓ)) + 1ΔHf(O2 (g))]
[1(0) + 1(-285.83)] - [1(50.63) + 1(0)] = -336.46 kJ
-336.46 kJ     (exothermic)

## Entropy Change

[1ΔSf(N2 (g)) + 1ΔSf(H2O (ℓ))] - [1ΔSf(N2H4 (ℓ)) + 1ΔSf(O2 (g))]
[1(191.5) + 1(69.91)] - [1(121.21) + 1(205.03)] = -64.83 J/K
-64.83 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(N2 (g)) + 1ΔGf(H2O (ℓ))] - [1ΔGf(N2H4 (ℓ)) + 1ΔGf(O2 (g))]
[1(0) + 1(-237.18)] - [1(149.24) + 1(0)] = -386.42 kJ
-386.42 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-317.13 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

5.0306255583e+067
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 223.