NH4OH (aq) → NH3 (g) + H2O (ℓ)

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Reaction Type:

Decomposition

Stoichiometry

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Heat Added: kJ
NH4OH          Mass: g  or Solution Volume: mL of Concentration: mol/L
NH3            Mass: g  or Gas Volume: L
H2O            Mass: g

Enthalpy of Reaction

[1ΔHf(NH3 (g)) + 1ΔHf(H2O (ℓ))] - [1ΔHf(NH4OH (aq))]
[1(-46.11) + 1(-285.83)] - [1(-362.5)] = 30.56 kJ
30.56 kJ     (endothermic)

Entropy Change

[1ΔSf(NH3 (g)) + 1ΔSf(H2O (ℓ))] - [1ΔSf(NH4OH (aq))]
[1(192.34) + 1(69.91)] - [1(102.64)] = 159.61 J/K
159.61 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(NH3 (g)) + 1ΔGf(H2O (ℓ))] - [1ΔGf(NH4OH (aq))]
[1(-16.48) + 1(-237.18)] - [1(-236.65)] = -17.01 kJ
-17.01 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-17.03 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

955.40803194
This process is favorable at 25°C.