## Pb (s) + 1 CuSO4 (aq) → PbSO4 (s) + Cu (s)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

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 Pb             Mass: g CuSO4          Mass: g or Solution Volume: mL of Concentration: mol/L PbSO4          Mass: g Cu             Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(PbSO4 (s)) + 1ΔHf(Cu (s))] - [1ΔHf(Pb (s)) + 1ΔHf(CuSO4 (aq))]
[1(-919.94) + 1(0)] - [1(0) + 1(-844.5)] = -75.4400000000001 kJ
-75.44 kJ     (exothermic)

## Entropy Change

[1ΔSf(PbSO4 (s)) + 1ΔSf(Cu (s))] - [1ΔSf(Pb (s)) + 1ΔSf(CuSO4 (aq))]
[1(148.57) + 1(33.15)] - [1(64.77) + 1(-79.5)] = 196.45 J/K
196.45 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(PbSO4 (s)) + 1ΔGf(Cu (s))] - [1ΔGf(Pb (s)) + 1ΔGf(CuSO4 (aq))]
[1(-813.2) + 1(0)] - [1(0) + 1(-679.11)] = -134.09 kJ
-134.09 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-134.01 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

3.110704722e+023
This process is favorable at 25°C.