PbCO3 (s) + 2 HNO3 (aq) → Pb(NO3)2 (aq) + H2O (ℓ) + 1 CO2 (g)

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Reaction Type:

Double Displacement/Decomposition of a Carbonate

Stoichiometry

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Heat Added: kJ
PbCO3          Mass: g
HNO3           Mass: g  or Solution Volume: mL of Concentration: mol/L
Pb(NO3)2       Mass: g
H2O            Mass: g
CO2            Mass: g  or Gas Volume: L

Enthalpy of Reaction

[1ΔHf(Pb(NO3)2 (aq)) + 1ΔHf(H2O (ℓ)) + 1ΔHf(CO2 (g))] - [1ΔHf(PbCO3 (s)) + 2ΔHf(HNO3 (aq))]
[1(-416.42) + 1(-285.83) + 1(-393.51)] - [1(-699.15) + 2(-207.36)] = 18.1099999999999 kJ
18.11 kJ     (endothermic)

Entropy Change

[1ΔSf(Pb(NO3)2 (aq)) + 1ΔSf(H2O (ℓ)) + 1ΔSf(CO2 (g))] - [1ΔSf(PbCO3 (s)) + 2ΔSf(HNO3 (aq))]
[1(303.38) + 1(69.91) + 1(213.68)] - [1(130.96) + 2(146.44)] = 163.13 J/K
163.13 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Pb(NO3)2 (aq)) + 1ΔGf(H2O (ℓ)) + 1ΔGf(CO2 (g))] - [1ΔGf(PbCO3 (s)) + 2ΔGf(HNO3 (aq))]
[1(-247.08) + 1(-237.18) + 1(-394.38)] - [1(-625.51) + 2(-111.34)] = -30.4499999999999 kJ
-30.45 kJ     (spontaneous)

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

Equilibrium Constant, K (at 298.15 K)

216225.06387
This process is favorable at 25°C.

Reference(s):

Kotz, John C., Treichel, Paul, and Weaver, Gabriela. Chemistry & Chemical Reactivity 6th ed.; Thomson Brooks/Cole: Belmont, CA, 2006; p 160.

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