## TlCl (s) → Tl+1 (aq) + Cl-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Tl+1 (aq)) + 1ΔHf(Cl-1 (aq))] - [1ΔHf(TlCl (s))]
[1(5.4) + 1(-167.15)] - [1(-204.14)] = 42.39 kJ
42.39 kJ     (endothermic)

## Entropy Change

[1ΔSf(Tl+1 (aq)) + 1ΔSf(Cl-1 (aq))] - [1ΔSf(TlCl (s))]
[1(125.5) + 1(56.48)] - [1(111.25)] = 70.73 J/K
70.73 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Tl+1 (aq)) + 1ΔGf(Cl-1 (aq))] - [1ΔGf(TlCl (s))]
[1(-32.4) + 1(-131.25)] - [1(-184.93)] = 21.28 kJ
21.28 kJ     (nonspontaneous)

From ΔG = ΔH - TΔS:
21.30 kJ     (nonspontaneous)

## Equilibrium Constant, K (at 298.15 K)

0.00018693811195
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (0.00018693811195) will be used to calculate the equilibrium concentration for all species.

 TlCl Tl+1 Cl-1 Initial M 0 0 Change -x +x +x Equilibrium