## SrCl2 (s) → Sr+2 (aq) + 2 Cl-1 (aq)

Back to reactions list

## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Sr+2 (aq)) + 2ΔHf(Cl-1 (aq))] - [1ΔHf(SrCl2 (s))]
[1(-545.8) + 2(-167.15)] - [1(-828.9)] = -51.1999999999999 kJ
-51.20 kJ     (exothermic)

## Entropy Change

[1ΔSf(Sr+2 (aq)) + 2ΔSf(Cl-1 (aq))] - [1ΔSf(SrCl2 (s))]
[1(-32.6) + 2(56.48)] - [1(114.9)] = -34.54 J/K
-34.54 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Sr+2 (aq)) + 2ΔGf(Cl-1 (aq))] - [1ΔGf(SrCl2 (s))]
[1(-559.5) + 2(-131.25)] - [1(-781.1)] = -40.9 kJ
-40.90 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-40.90 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

14647675.022
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (14647675.022) will be used to calculate the equilibrium concentration for all species.

 SrCl2 Sr+2 Cl-1 Initial M 0 0 Change -x +x +2x Equilibrium