S-2 (aq) + 1 H2O (ℓ) → HS-1 (aq) + OH-1 (aq)

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Stoichiometry

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S-2            Mass: g  or Solution Volume: mL of Concentration: mol/L
H2O            Mass: g
HS-1           Mass: g  or Solution Volume: mL of Concentration: mol/L
OH-1           Mass: g  or Solution Volume: mL of Concentration: mol/L

Enthalpy of Reaction

[1ΔHf(HS-1 (aq)) + 1ΔHf(OH-1 (aq))] - [1ΔHf(S-2 (aq)) + 1ΔHf(H2O (ℓ))]
[1(-17.57) + 1(-229.99)] - [1(33.05) + 1(-285.83)] = 5.21999999999997 kJ
5.22 kJ     (endothermic)

Entropy Change

[1ΔSf(HS-1 (aq)) + 1ΔSf(OH-1 (aq))] - [1ΔSf(S-2 (aq)) + 1ΔSf(H2O (ℓ))]
[1(62.76) + 1(-10.75)] - [1(-14.64) + 1(69.91)] = -3.26 J/K
-3.26 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(HS-1 (aq)) + 1ΔGf(OH-1 (aq))] - [1ΔGf(S-2 (aq)) + 1ΔGf(H2O (ℓ))]
[1(12.05) + 1(-157.28)] - [1(85.77) + 1(-237.18)] = 6.18000000000004 kJ
6.18 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

8.26514730219802E-02
This process is not favorable at 25°C.

Reference(s):

Halka, Monica and Nordstrom, Brian. Metals & Metalloids; Infobase Publishing: New York, NY, 2011; p 14.

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