NaNO3 (s) → Na+1 (aq) + NO3-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Na+1 (aq)) + 1ΔHf(NO3-1 (aq))] - [1ΔHf(NaNO3 (s))]
[1(-240.1) + 1(-207.36)] - [1(-466.68)] = 19.22 kJ
19.22 kJ     (endothermic)

Entropy Change

[1ΔSf(Na+1 (aq)) + 1ΔSf(NO3-1 (aq))] - [1ΔSf(NaNO3 (s))]
[1(59) + 1(146.44)] - [1(116.32)] = 89.12 J/K
89.12 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Na+1 (aq)) + 1ΔGf(NO3-1 (aq))] - [1ΔGf(NaNO3 (s))]
[1(-261.9) + 1(-111.34)] - [1(-365.89)] = -7.35000000000002 kJ
-7.35 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-7.35 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

19.397061343
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (19.397061343) will be used to calculate the equilibrium concentration for all species.

NaNO3 Na+1 NO3-1
Initial M   0 0
Change -x +x +x
Equilibrium

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 223.

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