(NH4)2SO4 (aq) + 2 NaOH (s) → Na2SO4 (aq) + 2 H2O (ℓ) + 2 NH3 (g)

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Reaction Type:

Double Displacement/Decomposition of Ammonium Hydroxide

Stoichiometry

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(NH4)2SO4      Mass: g  or Solution Volume: mL of Concentration: mol/L
NaOH           Mass: g
Na2SO4         Mass: g
H2O            Mass: g
NH3            Mass: g  or Gas Volume: L
Heat Released: kJ

Enthalpy of Reaction

[1ΔHf(Na2SO4 (aq)) + 2ΔHf(H2O (ℓ)) + 2ΔHf(NH3 (g))] - [1ΔHf((NH4)2SO4 (aq)) + 2ΔHf(NaOH (s))]
[1(-1389.47) + 2(-285.83) + 2(-46.11)] - [1(-1174.29) + 2(-426.73)] = -25.5999999999999 kJ
-25.60 kJ     (exothermic)

Entropy Change

[1ΔSf(Na2SO4 (aq)) + 2ΔSf(H2O (ℓ)) + 2ΔSf(NH3 (g))] - [1ΔSf((NH4)2SO4 (aq)) + 2ΔSf(NaOH (s))]
[1(138.08) + 2(69.91) + 2(192.34)] - [1(246.86) + 2(64.43)] = 286.86 J/K
286.86 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Na2SO4 (aq)) + 2ΔGf(H2O (ℓ)) + 2ΔGf(NH3 (g))] - [1ΔGf((NH4)2SO4 (aq)) + 2ΔGf(NaOH (s))]
[1(-1268.43) + 2(-237.18) + 2(-16.48)] - [1(-903.37) + 2(-379.07)] = -114.24 kJ
-114.24 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-111.13 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

1.0353703922e+020
This process is favorable at 25°C.