## Pb (s) + Mg(NO3)2 (aq) → Pb(NO3)2 (aq) + Mg (s)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

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 Heat Added: kJ Pb             Mass: g Mg(NO3)2       Mass: g or Solution Volume: mL of Concentration: mol/L Pb(NO3)2       Mass: g Mg             Mass: g

## Enthalpy of Reaction

[1ΔHf(Pb(NO3)2 (aq)) + 1ΔHf(Mg (s))] - [1ΔHf(Pb (s)) + 1ΔHf(Mg(NO3)2 (aq))]
[1(-416.42) + 1(0)] - [1(0) + 1(-881.57)] = 465.15 kJ
465.15 kJ     (endothermic)

## Entropy Change

[1ΔSf(Pb(NO3)2 (aq)) + 1ΔSf(Mg (s))] - [1ΔSf(Pb (s)) + 1ΔSf(Mg(NO3)2 (aq))]
[1(303.38) + 1(32.69)] - [1(64.77) + 1(154.81)] = 116.49 J/K
116.49 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Pb(NO3)2 (aq)) + 1ΔGf(Mg (s))] - [1ΔGf(Pb (s)) + 1ΔGf(Mg(NO3)2 (aq))]
[1(-247.08) + 1(0)] - [1(0) + 1(-677.48)] = 430.4 kJ
430.40 kJ     (nonspontaneous)

From ΔG = ΔH - TΔS:
430.42 kJ     (nonspontaneous)

## Equilibrium Constant, K (at 298.15 K)

3.9172981888e-076
This process is not favorable at 25°C.