## 3 Mg (s) + 2 Al(NO3)3 (aq) → 3 Mg(NO3)2 (aq) + 2 Al (s)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

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 Mg             Mass: g Al(NO3)3       Mass: g or Solution Volume: mL of Concentration: mol/L Mg(NO3)2       Mass: g Al             Mass: g Heat Released: kJ

## Enthalpy of Reaction

[3ΔHf(Mg(NO3)2 (aq)) + 2ΔHf(Al (s))] - [3ΔHf(Mg (s)) + 2ΔHf(Al(NO3)3 (aq))]
[3(-881.57) + 2(0)] - [3(0) + 2(-1153.45)] = -337.81 kJ
-337.81 kJ     (exothermic)

## Entropy Change

[3ΔSf(Mg(NO3)2 (aq)) + 2ΔSf(Al (s))] - [3ΔSf(Mg (s)) + 2ΔSf(Al(NO3)3 (aq))]
[3(154.81) + 2(28.33)] - [3(32.69) + 2(117.57)] = 187.88 J/K
187.88 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[3ΔGf(Mg(NO3)2 (aq)) + 2ΔGf(Al (s))] - [3ΔGf(Mg (s)) + 2ΔGf(Al(NO3)3 (aq))]
[3(-677.48) + 2(0)] - [3(0) + 2(-819.36)] = -393.72 kJ
-393.72 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-393.83 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

9.5630807679e+068
This process is favorable at 25°C.