## Cd (s gamma) + 2 AgNO3 (aq) → Cd(NO3)2 (aq) + 2 Ag (s)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

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 Cd             Mass: g AgNO3          Mass: g or Solution Volume: mL of Concentration: mol/L Cd(NO3)2       Mass: g Ag             Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(Cd(NO3)2 (aq)) + 2ΔHf(Ag (s))] - [1ΔHf(Cd (s gamma)) + 2ΔHf(AgNO3 (aq))]
[1(-490.62) + 2(0)] - [1(0) + 2(-101.78)] = -287.06 kJ
-287.06 kJ     (exothermic)

## Entropy Change

[1ΔSf(Cd(NO3)2 (aq)) + 2ΔSf(Ag (s))] - [1ΔSf(Cd (s gamma)) + 2ΔSf(AgNO3 (aq))]
[1(219.68) + 2(42.55)] - [1(51.76) + 2(219.12)] = -185.22 J/K
-185.22 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Cd(NO3)2 (aq)) + 2ΔGf(Ag (s))] - [1ΔGf(Cd (s gamma)) + 2ΔGf(AgNO3 (aq))]
[1(-300.28) + 2(0)] - [1(0) + 2(-34.22)] = -231.84 kJ
-231.84 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-231.84 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

4.1578686901e+040
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 97.