NH4Cl (aq) + 1 NaOH (aq) → NH3 (g) + H2O (ℓ) + 1 NaCl (aq)

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Stoichiometry

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NH4Cl          Mass: g  or Solution Volume: mL of Concentration: mol/L
NaOH           Mass: g  or Solution Volume: mL of Concentration: mol/L
NH3            Mass: g  or Gas Volume: L
H2O            Mass: g
NaCl           Mass: g  or Solution Volume: mL of Concentration: mol/L

Enthalpy of Reaction

[1ΔHf(NH3 (g)) + 1ΔHf(H2O (ℓ)) + 1ΔHf(NaCl (aq))] - [1ΔHf(NH4Cl (aq)) + 1ΔHf(NaOH (aq))]
[1(-46.11) + 1(-285.83) + 1(-407.25)] - [1(-299.66) + 1(-470.09)] = 30.5599999999999 kJ
30.56 kJ     (endothermic)

Entropy Change

[1ΔSf(NH3 (g)) + 1ΔSf(H2O (ℓ)) + 1ΔSf(NaCl (aq))] - [1ΔSf(NH4Cl (aq)) + 1ΔSf(NaOH (aq))]
[1(192.34) + 1(69.91) + 1(115.48)] - [1(169.87) + 1(48.25)] = 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(NaCl (aq))] - [1ΔGf(NH4Cl (aq)) + 1ΔGf(NaOH (aq))]
[1(-16.48) + 1(-237.18) + 1(-393.15)] - [1(-210.62) + 1(-419.18)] = -17.01 kJ
-17.01 kJ     (spontaneous)

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

Equilibrium Constant, K (at 298.15 K)

955.408031940303
This process is favorable at 25°C.

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 129.

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