3 Ba (s) + 2 Al(NO3)3 (aq) → 3 Ba(NO3)2 (aq) + 2 Al (s)

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Reaction Type:

Single displacement/Oxidation-reduction

Stoichiometry

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

Enthalpy of Reaction

[3ΔHf(Ba(NO3)2 (aq)) + 2ΔHf(Al (s))] - [3ΔHf(Ba (s)) + 2ΔHf(Al(NO3)3 (aq))]
[3(-952.32) + 2(0)] - [3(0) + 2(-1153.45)] = -550.06 kJ
-550.06 kJ     (exothermic)

Entropy Change

[3ΔSf(Ba(NO3)2 (aq)) + 2ΔSf(Al (s))] - [3ΔSf(Ba (s)) + 2ΔSf(Al(NO3)3 (aq))]
[3(302.48) + 2(28.33)] - [3(62.34) + 2(117.57)] = 541.94 J/K
541.94 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[3ΔGf(Ba(NO3)2 (aq)) + 2ΔGf(Al (s))] - [3ΔGf(Ba (s)) + 2ΔGf(Al(NO3)3 (aq))]
[3(-783.48) + 2(0)] - [3(0) + 2(-819.36)] = -711.72 kJ
-711.72 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-711.64 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

4.9532179789e+124
This process is favorable at 25°C.