NH3 (g) + 1 CO2 (g) + 1 H2O (ℓ)1 NaCl (aq) → NaHCO3 (s) + NH4Cl (aq)

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Stoichiometry

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NH3            Mass: g  or Gas Volume: L
CO2            Mass: g  or Gas Volume: L
H2O            Mass: g
NaCl           Mass: g  or Solution Volume: mL of Concentration: mol/L
NaHCO3         Mass: g
NH4Cl          Mass: g
Heat Released: kJ

Enthalpy of Reaction

[1ΔHf(NaHCO3 (s)) + 1ΔHf(NH4Cl (aq))] - [1ΔHf(NH3 (g)) + 1ΔHf(CO2 (g)) + 1ΔHf(H2O (ℓ)) + 1ΔHf(NaCl (aq))]
[1(-947.68) + 1(-299.66)] - [1(-46.11) + 1(-393.51) + 1(-285.83) + 1(-407.25)] = -114.64 kJ
-114.64 kJ     (exothermic)

Entropy Change

[1ΔSf(NaHCO3 (s)) + 1ΔSf(NH4Cl (aq))] - [1ΔSf(NH3 (g)) + 1ΔSf(CO2 (g)) + 1ΔSf(H2O (ℓ)) + 1ΔSf(NaCl (aq))]
[1(102.09) + 1(169.87)] - [1(192.34) + 1(213.68) + 1(69.91) + 1(115.48)] = -319.45 J/K
-319.45 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(NaHCO3 (s)) + 1ΔGf(NH4Cl (aq))] - [1ΔGf(NH3 (g)) + 1ΔGf(CO2 (g)) + 1ΔGf(H2O (ℓ)) + 1ΔGf(NaCl (aq))]
[1(-851.86) + 1(-210.62)] - [1(-16.48) + 1(-394.38) + 1(-237.18) + 1(-393.15)] = -21.29 kJ
-21.29 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-19.40 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

5370.9878463
This process is favorable at 25°C.

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 181.

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