Reaction Type:
Dissociation of an ionic compound in water
Enthalpy of Reaction
[1ΔHf(Ag+1 (aq)) + 1ΔHf(CN-1 (aq))] - [1ΔHf(AgCN (s))]
[1(105.58) + 1(150.62)] - [1(146.02)] = 110.18 kJ
110.18 kJ (endothermic)
Entropy Change
[1ΔSf(Ag+1 (aq)) + 1ΔSf(CN-1 (aq))] - [1ΔSf(AgCN (s))]
[1(72.68) + 1(94.14)] - [1(107.19)] = 59.63 J/K
59.63 J/K (increase in entropy)
Free Energy of Reaction (at 298.15 K)
From ΔGf° values:
[1ΔGf(Ag+1 (aq)) + 1ΔGf(CN-1 (aq))] - [1ΔGf(AgCN (s))]
[1(77.12) + 1(172.38)] - [1(156.9)] = 92.6 kJ
92.60 kJ (nonspontaneous)
From ΔG = ΔH - TΔS:
92.40 kJ (nonspontaneous)
Equilibrium Constant, K (at 298.15 K)
5.9741921525e-017
This process is not favorable at 25°C.
Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (5.9741921525e-017) will be used to calculate the equilibrium concentration for all species.