## SrBr2 (s) → Sr+2 (aq) + 2 Br-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Sr+2 (aq)) + 2ΔHf(Br-1 (aq))] - [1ΔHf(SrBr2 (s))]
[1(-545.8) + 2(-121.55)] - [1(-717.97)] = -70.9299999999999 kJ
-70.93 kJ     (exothermic)

## Entropy Change

[1ΔSf(Sr+2 (aq)) + 2ΔSf(Br-1 (aq))] - [1ΔSf(SrBr2 (s))]
[1(-32.6) + 2(82.42)] - [1(143.43)] = -11.19 J/K
-11.19 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Sr+2 (aq)) + 2ΔGf(Br-1 (aq))] - [1ΔGf(SrBr2 (s))]
[1(-559.5) + 2(-103.97)] - [1(-699.77)] = -67.6700000000001 kJ
-67.67 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-67.59 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

7.1767984456e+011
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (7.1767984456e+011) will be used to calculate the equilibrium concentration for all species.

 SrBr2 Sr+2 Br-1 Initial M 0 0 Change -x +x +2x Equilibrium