## 2 NaOH (s) + 1 CO2 (g) → Na2CO3 (s) + H2O (ℓ)

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## Stoichiometry

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 NaOH           Mass: g CO2            Mass: g or Gas Volume: L Na2CO3         Mass: g H2O            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(Na2CO3 (s)) + 1ΔHf(H2O (ℓ))] - [2ΔHf(NaOH (s)) + 1ΔHf(CO2 (g))]
[1(-1130.94) + 1(-285.83)] - [2(-426.73) + 1(-393.51)] = -169.8 kJ
-169.80 kJ     (exothermic)

## Entropy Change

[1ΔSf(Na2CO3 (s)) + 1ΔSf(H2O (ℓ))] - [2ΔSf(NaOH (s)) + 1ΔSf(CO2 (g))]
[1(135.98) + 1(69.91)] - [2(64.43) + 1(213.68)] = -136.65 J/K
-136.65 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Na2CO3 (s)) + 1ΔGf(H2O (ℓ))] - [2ΔGf(NaOH (s)) + 1ΔGf(CO2 (g))]
[1(-1047.67) + 1(-237.18)] - [2(-379.07) + 1(-394.38)] = -132.33 kJ
-132.33 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-129.06 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

1.529336211e+023
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 94.