Ba(OH)2 (aq) + 2 NH4F (s) → BaI2 (aq) + 2 H2O (ℓ) + 2 NH3 (g)

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Reaction Type:

Double Displacement/Decomposition of Ammonium Hydroxide

Stoichiometry

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Ba(OH)2        Mass: g  or Solution Volume: mL of Concentration: mol/L
NH4F           Mass: g
BaI2           Mass: g  or Solution Volume: mL of Concentration: mol/L
H2O            Mass: g
NH3            Mass: g  or Gas Volume: L

Enthalpy of Reaction

[1ΔHf(BaI2 (aq)) + 2ΔHf(H2O (ℓ)) + 2ΔHf(NH3 (g))] - [1ΔHf(Ba(OH)2 (aq)) + 2ΔHf(NH4F (s))]
[1(-647.98) + 2(-285.83) + 2(-46.11)] - [1(-997.58) + 2(-463.96)] = 613.64 kJ
613.64 kJ     (endothermic)

Entropy Change

[1ΔSf(BaI2 (aq)) + 2ΔSf(H2O (ℓ)) + 2ΔSf(NH3 (g))] - [1ΔSf(Ba(OH)2 (aq)) + 2ΔSf(NH4F (s))]
[1(232.18) + 2(69.91) + 2(192.34)] - [1(-11.9) + 2(71.96)] = 624.66 J/K
624.66 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(BaI2 (aq)) + 2ΔGf(H2O (ℓ)) + 2ΔGf(NH3 (g))] - [1ΔGf(Ba(OH)2 (aq)) + 2ΔGf(NH4F (s))]
[1(-663.98) + 2(-237.18) + 2(-16.48)] - [1(-875.36) + 2(-348.78)] = 401.62 kJ
401.62 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

4.3182227813e-071
This process is not favorable at 25°C.