## 2 LiOH (s) + 1 CO2 (g) → Li2CO3 (s) + H2O (ℓ)

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## Stoichiometry

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 LiOH           Mass: g CO2            Mass: g or Gas Volume: L Li2CO3         Mass: g H2O            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(Li2CO3 (s)) + 1ΔHf(H2O (ℓ))] - [2ΔHf(LiOH (s)) + 1ΔHf(CO2 (g))]
[1(-1216.04) + 1(-285.83)] - [2(-484.93) + 1(-393.51)] = -138.5 kJ
-138.50 kJ     (exothermic)

## Entropy Change

[1ΔSf(Li2CO3 (s)) + 1ΔSf(H2O (ℓ))] - [2ΔSf(LiOH (s)) + 1ΔSf(CO2 (g))]
[1(90.17) + 1(69.91)] - [2(42.8) + 1(213.68)] = -139.2 J/K
-139.20 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Li2CO3 (s)) + 1ΔGf(H2O (ℓ))] - [2ΔGf(LiOH (s)) + 1ΔGf(CO2 (g))]
[1(-1132.19) + 1(-237.18)] - [2(-438.9) + 1(-394.38)] = -97.1900000000003 kJ
-97.19 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-97.00 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

1.0663475289e+017
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; pp 183, 227.