2 NaHCO3 (s) → Na2CO3 (s) + H2O (g) + 1 CO2 (g)

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Stoichiometry

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Heat Added: kJ
NaHCO3         Mass: g
Na2CO3         Mass: g
H2O            Mass: g  or Gas Volume: L
CO2            Mass: g  or Gas Volume: L

Enthalpy of Reaction

[1ΔHf(Na2CO3 (s)) + 1ΔHf(H2O (g)) + 1ΔHf(CO2 (g))] - [2ΔHf(NaHCO3 (s))]
[1(-1130.94) + 1(-241.82) + 1(-393.51)] - [2(-947.68)] = 129.09 kJ
129.09 kJ     (endothermic)

Entropy Change

[1ΔSf(Na2CO3 (s)) + 1ΔSf(H2O (g)) + 1ΔSf(CO2 (g))] - [2ΔSf(NaHCO3 (s))]
[1(135.98) + 1(188.72) + 1(213.68)] - [2(102.09)] = 334.2 J/K
334.20 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Na2CO3 (s)) + 1ΔGf(H2O (g)) + 1ΔGf(CO2 (g))] - [2ΔGf(NaHCO3 (s))]
[1(-1047.67) + 1(-228.59) + 1(-394.38)] - [2(-851.86)] = 33.0800000000002 kJ
33.08 kJ     (nonspontaneous)

From ΔG = ΔH - TΔS:
29.45 kJ     (nonspontaneous)

Equilibrium Constant, K (at 298.15 K)

1.6007085419e-006
This process is not favorable at 25°C.

Reference(s):

Swaddle, T.W. Inorganic Chemistry; Academic Press: San Diego, 1997; p 211.
Zumdahl, Steven and Zumdahl, Susan A. Chemistry 9th ed.; Brooks/Cole: Belmont, CA, 2014; p 131.
Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 226.

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