## Pb (s) + 2 HCl (aq) → PbCl2 (aq) + H2 (g)

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## Stoichiometry

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 Pb             Mass: g HCl            Mass: g or Solution Volume: mL of Concentration: mol/L PbCl2          Mass: g H2             Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(PbCl2 (aq)) + 1ΔHf(H2 (g))] - [1ΔHf(Pb (s)) + 2ΔHf(HCl (aq))]
[1(-336) + 1(0)] - [1(0) + 2(-167.15)] = -1.69999999999999 kJ
-1.70 kJ     (exothermic)

## Entropy Change

[1ΔSf(PbCl2 (aq)) + 1ΔSf(H2 (g))] - [1ΔSf(Pb (s)) + 2ΔSf(HCl (aq))]
[1(123.46) + 1(130.59)] - [1(64.77) + 2(56.48)] = 76.32 J/K
76.32 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(PbCl2 (aq)) + 1ΔGf(H2 (g))] - [1ΔGf(Pb (s)) + 2ΔGf(HCl (aq))]
[1(-286.9) + 1(0)] - [1(0) + 2(-131.25)] = -24.4 kJ
-24.40 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-24.45 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

18833.581424
This process is favorable at 25°C.

## Reference(s):

Halka, Monica and Nordstrom, Brian. Metals & Metalloids; Infobase Publishing: New York, NY, 2011; pg. 61.