2 HCl (aq) + 1 PbCO3 (s) → PbCl2 (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
PbCO3          Mass: g
PbCl2          Mass: g  or Solution Volume: mL of Concentration: mol/L
H2O            Mass: g
CO2            Mass: g  or Gas Volume: L

Enthalpy of Reaction

[1ΔHf(PbCl2 (aq)) + 1ΔHf(H2O (ℓ)) + 1ΔHf(CO2 (g))] - [2ΔHf(HCl (aq)) + 1ΔHf(PbCO3 (s))]
[1(-336) + 1(-285.83) + 1(-393.51)] - [2(-167.15) + 1(-699.15)] = 18.1100000000001 kJ
18.11 kJ     (endothermic)

Entropy Change

[1ΔSf(PbCl2 (aq)) + 1ΔSf(H2O (ℓ)) + 1ΔSf(CO2 (g))] - [2ΔSf(HCl (aq)) + 1ΔSf(PbCO3 (s))]
[1(123.46) + 1(69.91) + 1(213.68)] - [2(56.48) + 1(130.96)] = 163.13 J/K
163.13 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(PbCl2 (aq)) + 1ΔGf(H2O (ℓ)) + 1ΔGf(CO2 (g))] - [2ΔGf(HCl (aq)) + 1ΔGf(PbCO3 (s))]
[1(-286.9) + 1(-237.18) + 1(-394.38)] - [2(-131.25) + 1(-625.51)] = -30.4499999999999 kJ
-30.45 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-30.53 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

216225.063871828
This process is favorable at 25°C.