AgNO3 (s) → Ag+1 (aq) + NO3-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Ag+1 (aq)) + 1ΔHf(NO3-1 (aq))] - [1ΔHf(AgNO3 (s))]
[1(105.58) + 1(-207.36)] - [1(-124.39)] = 22.61 kJ
22.61 kJ     (endothermic)

Entropy Change

[1ΔSf(Ag+1 (aq)) + 1ΔSf(NO3-1 (aq))] - [1ΔSf(AgNO3 (s))]
[1(72.68) + 1(146.44)] - [1(140.92)] = 78.2 J/K
78.20 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ag+1 (aq)) + 1ΔGf(NO3-1 (aq))] - [1ΔGf(AgNO3 (s))]
[1(77.12) + 1(-111.34)] - [1(-33.47)] = -0.75 kJ
-0.75 kJ     (close to or at equilibrium)

From ΔG = ΔH - TΔS:
-0.71 kJ     (close to or at equilibrium)

Equilibrium Constant, K (at 298.15 K)

1.35332351
This process is close to or at equilibrium at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.35332351) will be used to calculate the equilibrium concentration for all species.

AgNO3 Ag+1 NO3-1
Initial M   0 0
Change -x +x +x
Equilibrium