## Pb (s) + 1 PbO2 (s) + 2 H2SO4 (aq) → 2 PbSO4 (s) + 2 H2O (ℓ)

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## Stoichiometry

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 Pb             Mass: g PbO2           Mass: g H2SO4          Mass: g or Solution Volume: mL of Concentration: mol/L PbSO4          Mass: g H2O            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(PbSO4 (s)) + 2ΔHf(H2O (ℓ))] - [1ΔHf(Pb (s)) + 1ΔHf(PbO2 (s)) + 2ΔHf(H2SO4 (aq))]
[2(-919.94) + 2(-285.83)] - [1(0) + 1(-274.47) + 2(-909.27)] = -318.53 kJ
-318.53 kJ     (exothermic)

## Entropy Change

[2ΔSf(PbSO4 (s)) + 2ΔSf(H2O (ℓ))] - [1ΔSf(Pb (s)) + 1ΔSf(PbO2 (s)) + 2ΔSf(H2SO4 (aq))]
[2(148.57) + 2(69.91)] - [1(64.77) + 1(71.8) + 2(20.08)] = 260.23 J/K
260.23 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(PbSO4 (s)) + 2ΔGf(H2O (ℓ))] - [1ΔGf(Pb (s)) + 1ΔGf(PbO2 (s)) + 2ΔGf(H2SO4 (aq))]
[2(-813.2) + 2(-237.18)] - [1(0) + 1(-215.48) + 2(-744.63)] = -396.02 kJ
-396.02 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-396.12 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

2.4185931112e+069
This process is favorable at 25°C.

## Reference(s):

Halka, Monica and Nordstrom, Brian. Metals & Metalloids; Infobase Publishing: New York, NY, 2011; pg. 66.