## KI (aq) + 1 AgNO3 (aq) → KNO3 (aq) + AgI (s)

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## Stoichiometry

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 KI             Mass: g or Solution Volume: mL of Concentration: mol/L AgNO3          Mass: g or Solution Volume: mL of Concentration: mol/L KNO3           Mass: g AgI            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(KNO3 (aq)) + 1ΔHf(AgI (s))] - [1ΔHf(KI (aq)) + 1ΔHf(AgNO3 (aq))]
[1(-459.76) + 1(-61.84)] - [1(-307.59) + 1(-101.78)] = -112.23 kJ
-112.23 kJ     (exothermic)

## Entropy Change

[1ΔSf(KNO3 (aq)) + 1ΔSf(AgI (s))] - [1ΔSf(KI (aq)) + 1ΔSf(AgNO3 (aq))]
[1(248.94) + 1(115.48)] - [1(213.79) + 1(219.12)] = -68.49 J/K
-68.49 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(KNO3 (aq)) + 1ΔGf(AgI (s))] - [1ΔGf(KI (aq)) + 1ΔGf(AgNO3 (aq))]
[1(-394.64) + 1(-66.19)] - [1(-334.89) + 1(-34.22)] = -91.72 kJ
-91.72 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-91.81 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

1.1736616245e+016
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 139.