2 HBr (aq) + 1 Ag2SO3 (s) → 2 AgBr (s) + H2O (ℓ) + 1 SO2 (g)

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Reaction Type:

Double Displacement/Decomposition of a Sulfite

Stoichiometry

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HBr            Mass: g  or Solution Volume: mL of Concentration: mol/L
Ag2SO3         Mass: g
AgBr           Mass: g
H2O            Mass: g
SO2            Mass: g  or Gas Volume: L

Enthalpy of Reaction

[2ΔHf(AgBr (s)) + 1ΔHf(H2O (ℓ)) + 1ΔHf(SO2 (g))] - [2ΔHf(HBr (aq)) + 1ΔHf(Ag2SO3 (s))]
[2(-100.37) + 1(-285.83) + 1(-296.83)] - [2(-121.55) + 1(-490.78)] = -49.52 kJ
-49.52 kJ     (exothermic)

Entropy Change

[2ΔSf(AgBr (s)) + 1ΔSf(H2O (ℓ)) + 1ΔSf(SO2 (g))] - [2ΔSf(HBr (aq)) + 1ΔSf(Ag2SO3 (s))]
[2(107.11) + 1(69.91) + 1(248.11)] - [2(82.42) + 1(158.16)] = 209.24 J/K
209.24 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(AgBr (s)) + 1ΔGf(H2O (ℓ)) + 1ΔGf(SO2 (g))] - [2ΔGf(HBr (aq)) + 1ΔGf(Ag2SO3 (s))]
[2(-96.9) + 1(-237.18) + 1(-300.19)] - [2(-103.97) + 1(-411.29)] = -111.94 kJ
-111.94 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-111.90 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

4.0938389511638E+19
This process is favorable at 25°C.