## 2 HBr (aq) + 1 Ba(OH)2 (aq) → 2 H2O (ℓ) + BaBr2 (aq)

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## Stoichiometry

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 HBr            Mass: g or Solution Volume: mL of Concentration: mol/L Ba(OH)2        Mass: g or Solution Volume: mL of Concentration: mol/L H2O            Mass: g BaBr2          Mass: g Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(H2O (ℓ)) + 1ΔHf(BaBr2 (aq))] - [2ΔHf(HBr (aq)) + 1ΔHf(Ba(OH)2 (aq))]
[2(-285.83) + 1(-780.7)] - [2(-121.55) + 1(-997.58)] = -111.68 kJ
-111.68 kJ     (exothermic)

## Entropy Change

[2ΔSf(H2O (ℓ)) + 1ΔSf(BaBr2 (aq))] - [2ΔSf(HBr (aq)) + 1ΔSf(Ba(OH)2 (aq))]
[2(69.91) + 1(174.44)] - [2(82.42) + 1(-11.9)] = 161.32 J/K
161.32 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(H2O (ℓ)) + 1ΔGf(BaBr2 (aq))] - [2ΔGf(HBr (aq)) + 1ΔGf(Ba(OH)2 (aq))]
[2(-237.18) + 1(-768.74)] - [2(-103.97) + 1(-875.36)] = -159.8 kJ
-159.80 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-159.78 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

9.9381727897e+027
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 98.