## H2CO3 (aq) → CO2 (g) + H2O (ℓ)

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Decomposition

## Stoichiometry

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

## 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)

1.4502964962e+018
This process is favorable at 25°C.