## Na2SO4 (s) → 2 Na+1 (aq) + SO4-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[2ΔHf(Na+1 (aq)) + 1ΔHf(SO4-2 (aq))] - [1ΔHf(Na2SO4 (s))]
[2(-240.1) + 1(-909.27)] - [1(-1384.49)] = -4.98000000000002 kJ
-4.98 kJ     (exothermic)

## Entropy Change

[2ΔSf(Na+1 (aq)) + 1ΔSf(SO4-2 (aq))] - [1ΔSf(Na2SO4 (s))]
[2(59) + 1(20.08)] - [1(149.49)] = -11.41 J/K
-11.41 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(Na+1 (aq)) + 1ΔGf(SO4-2 (aq))] - [1ΔGf(Na2SO4 (s))]
[2(-261.9) + 1(-744.63)] - [1(-1266.83)] = -1.59999999999991 kJ
-1.60 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-1.58 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

1.9068804655
This process is close to or at equilibrium at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.9068804655) will be used to calculate the equilibrium concentration for all species.

 Na2SO4 Na+1 SO4-2 Initial M 0 0 Change -x +2x +x Equilibrium