2 HCl (aq) + 1 K2CO3 (s) → 2 KCl (aq) + H2O (ℓ) + 1 CO2 (g)

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Reaction Type:

Double Displacement/Decomposition of a Carbonate

Stoichiometry

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HCl            Mass: g  or Solution Volume: mL of Concentration: mol/L
K2CO3          Mass: g
KCl            Mass: g  or Solution Volume: mL of Concentration: mol/L
H2O            Mass: g
CO2            Mass: g  or Gas Volume: L

Enthalpy of Reaction

[2ΔHf(KCl (aq)) + 1ΔHf(H2O (ℓ)) + 1ΔHf(CO2 (g))] - [2ΔHf(HCl (aq)) + 1ΔHf(K2CO3 (s))]
[2(-419.55) + 1(-285.83) + 1(-393.51)] - [2(-167.15) + 1(-1150.18)] = -33.96 kJ
-33.96 kJ     (exothermic)

Entropy Change

[2ΔSf(KCl (aq)) + 1ΔSf(H2O (ℓ)) + 1ΔSf(CO2 (g))] - [2ΔSf(HCl (aq)) + 1ΔSf(K2CO3 (s))]
[2(158.98) + 1(69.91) + 1(213.68)] - [2(56.48) + 1(155.52)] = 333.07 J/K
333.07 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(KCl (aq)) + 1ΔGf(H2O (ℓ)) + 1ΔGf(CO2 (g))] - [2ΔGf(HCl (aq)) + 1ΔGf(K2CO3 (s))]
[2(-414.55) + 1(-237.18) + 1(-394.38)] - [2(-131.25) + 1(-1064.41)] = -133.75 kJ
-133.75 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-133.26 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

2.71200228506908E+23
This process is favorable at 25°C.