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

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## Reaction Type:

Double Displacement

## 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.

 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 Heat Released: kJ

## 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)

54787286.006
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.