NH4NO3 (s) → NH4+1 (aq) + NO3-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(NH4+1 (aq)) + 1ΔHf(NO3-1 (aq))] - [1ΔHf(NH4NO3 (s))]
[1(-132.51) + 1(-207.36)] - [1(-365.56)] = 25.69 kJ
25.69 kJ     (endothermic)

Entropy Change

[1ΔSf(NH4+1 (aq)) + 1ΔSf(NO3-1 (aq))] - [1ΔSf(NH4NO3 (s))]
[1(113.39) + 1(146.44)] - [1(151.08)] = 108.75 J/K
108.75 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(NH4+1 (aq)) + 1ΔGf(NO3-1 (aq))] - [1ΔGf(NH4NO3 (s))]
[1(-79.37) + 1(-111.34)] - [1(-184.01)] = -6.70000000000002 kJ
-6.70 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-6.73 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

14.9229447014
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (14.9229447014) will be used to calculate the equilibrium concentration for all species.

NH4NO3 NH4+1 NO3-1
Initial M   0 0
Change -x +x +x
Equilibrium