2 NaI (aq) + 1 Pb(NO3)2 (aq) → PbI2 (s) + 2 NaNO3 (aq)

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Reaction Type:

Double Displacement

Stoichiometry

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NaI            Mass: g  or Solution Volume: mL of Concentration: mol/L
Pb(NO3)2       Mass: g  or Solution Volume: mL of Concentration: mol/L
PbI2           Mass: g
NaNO3          Mass: g  or Solution Volume: mL of Concentration: mol/L

Enthalpy of Reaction

[1ΔHf(PbI2 (s)) + 2ΔHf(NaNO3 (aq))] - [2ΔHf(NaI (aq)) + 1ΔHf(Pb(NO3)2 (aq))]
[1(-175.39) + 2(-447.46)] - [2(-295.29) + 1(-416.42)] = -63.3099999999999 kJ
-63.31 kJ     (exothermic)

Entropy Change

[1ΔSf(PbI2 (s)) + 2ΔSf(NaNO3 (aq))] - [2ΔSf(NaI (aq)) + 1ΔSf(Pb(NO3)2 (aq))]
[1(174.85) + 2(205.44)] - [2(170.29) + 1(303.38)] = -58.23 J/K
-58.23 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(PbI2 (s)) + 2ΔGf(NaNO3 (aq))] - [2ΔGf(NaI (aq)) + 1ΔGf(Pb(NO3)2 (aq))]
[1(-173.59) + 2(-373.24)] - [2(-313.49) + 1(-247.08)] = -46.01 kJ
-46.01 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-45.95 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

115093759.818946
This process is favorable at 25°C.