Pb(NO3)2 (aq) + 1 H2SO4 (aq) → PbSO4 (s) + 2 HNO3 (aq)

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Reaction Type:

Double Displacement

Stoichiometry

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Pb(NO3)2       Mass: g  or Solution Volume: mL of Concentration: mol/L
H2SO4          Mass: g  or Solution Volume: mL of Concentration: mol/L
PbSO4          Mass: g
HNO3           Mass: g  or Solution Volume: mL of Concentration: mol/L

Enthalpy of Reaction

[1ΔHf(PbSO4 (s)) + 2ΔHf(HNO3 (aq))] - [1ΔHf(Pb(NO3)2 (aq)) + 1ΔHf(H2SO4 (aq))]
[1(-919.94) + 2(-207.36)] - [1(-416.42) + 1(-909.27)] = -8.97000000000003 kJ
-8.97 kJ     (exothermic)

Entropy Change

[1ΔSf(PbSO4 (s)) + 2ΔSf(HNO3 (aq))] - [1ΔSf(Pb(NO3)2 (aq)) + 1ΔSf(H2SO4 (aq))]
[1(148.57) + 2(146.44)] - [1(303.38) + 1(20.08)] = 117.99 J/K
117.99 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(PbSO4 (s)) + 2ΔGf(HNO3 (aq))] - [1ΔGf(Pb(NO3)2 (aq)) + 1ΔGf(H2SO4 (aq))]
[1(-813.2) + 2(-111.34)] - [1(-247.08) + 1(-744.63)] = -44.1700000000001 kJ
-44.17 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-44.15 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

54787286.0057473
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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