NH4Cl (s) → NH4+1 (aq) + Cl-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(NH4+1 (aq)) + 1ΔHf(Cl-1 (aq))] - [1ΔHf(NH4Cl (s))]
[1(-132.51) + 1(-167.15)] - [1(-314.43)] = 14.77 kJ
14.77 kJ     (endothermic)

Entropy Change

[1ΔSf(NH4+1 (aq)) + 1ΔSf(Cl-1 (aq))] - [1ΔSf(NH4Cl (s))]
[1(113.39) + 1(56.48)] - [1(94.56)] = 75.31 J/K
75.31 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(NH4+1 (aq)) + 1ΔGf(Cl-1 (aq))] - [1ΔGf(NH4Cl (s))]
[1(-79.37) + 1(-131.25)] - [1(-202.97)] = -7.65000000000001 kJ
-7.65 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-7.68 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

21.892562077
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (21.892562077) will be used to calculate the equilibrium concentration for all species.

NH4Cl NH4+1 Cl-1
Initial M   0 0
Change -x +x +x
Equilibrium