H2CO3 (aq) → CO2 (g) + H2O (ℓ)

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Reaction Type:

Decomposition

Stoichiometry

Enter a mass or volume in one of the boxes below. Upon hitting submit, the stoichiometric equivalents will be calculated for the remaining reactants and products. All gases are assumed to be at STP.

H2CO3          Mass: g  or Solution Volume: mL of Concentration: mol/L
CO2            Mass: g  or Gas Volume: L
H2O            Mass: g

Enthalpy of Reaction

[1ΔHf(CO2 (g)) + 1ΔHf(H2O (ℓ))] - [1ΔHf(H2CO3 (aq))]
[1(-393.51) + 1(-285.83)] - [1(-677.14)] = -2.19999999999993 kJ
-2.20 kJ     (exothermic)

Entropy Change

[1ΔSf(CO2 (g)) + 1ΔSf(H2O (ℓ))] - [1ΔSf(H2CO3 (aq))]
[1(213.68) + 1(69.91)] - [1(-56.9)] = 340.49 J/K
340.49 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(CO2 (g)) + 1ΔGf(H2O (ℓ))] - [1ΔGf(H2CO3 (aq))]
[1(-394.38) + 1(-237.18)] - [1(-527.9)] = -103.66 kJ
-103.66 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-103.72 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

1.45029649619679E+18
This process is favorable at 25°C.