2 HF (aq) + 1 K2CO3 (s) → 2 KF (aq) + H2O (ℓ) + 1 CO2 (g)

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Reaction Type:

Double Displacement/Decomposition of a Carbonate

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.

 HF             Mass: g or Solution Volume: mL of Concentration: mol/L K2CO3          Mass: g KF             Mass: g H2O            Mass: g CO2            Mass: g or Gas Volume: L Heat Released: kJ

Enthalpy of Reaction

[2ΔHf(KF (aq)) + 1ΔHf(H2O (ℓ)) + 1ΔHf(CO2 (g))] - [2ΔHf(HF (aq)) + 1ΔHf(K2CO3 (s))]
[2(-508.04) + 1(-285.83) + 1(-393.51)] - [2(-255.64) + 1(-1150.18)] = -33.9599999999998 kJ
-33.96 kJ     (exothermic)

Entropy Change

[2ΔSf(KF (aq)) + 1ΔSf(H2O (ℓ)) + 1ΔSf(CO2 (g))] - [2ΔSf(HF (aq)) + 1ΔSf(K2CO3 (s))]
[2(247.98) + 1(69.91) + 1(213.68)] - [2(145.48) + 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(KF (aq)) + 1ΔGf(H2O (ℓ)) + 1ΔGf(CO2 (g))] - [2ΔGf(HF (aq)) + 1ΔGf(K2CO3 (s))]
[2(-545.64) + 1(-237.18) + 1(-394.38)] - [2(-262.34) + 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)

2.7120022851e+023
This process is favorable at 25°C.