## Sn+2 (aq) + 1 H2S (g) → SnS (s) + 2 H+1 (aq)

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## Stoichiometry

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 Sn+2           Mass: g or Solution Volume: mL of Concentration: mol/L H2S            Mass: g or Gas Volume: L SnS            Mass: g H+1            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(SnS (s)) + 2ΔHf(H+1 (aq))] - [1ΔHf(Sn+2 (aq)) + 1ΔHf(H2S (g))]
[1(-100.42) + 2(0)] - [1(-8.8) + 1(-20.17)] = -71.45 kJ
-71.45 kJ     (exothermic)

## Entropy Change

[1ΔSf(SnS (s)) + 2ΔSf(H+1 (aq))] - [1ΔSf(Sn+2 (aq)) + 1ΔSf(H2S (g))]
[1(76.99) + 2(0)] - [1(-17) + 1(205.77)] = -111.78 J/K
-111.78 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(SnS (s)) + 2ΔGf(H+1 (aq))] - [1ΔGf(Sn+2 (aq)) + 1ΔGf(H2S (g))]
[1(-98.32) + 2(0)] - [1(-27.2) + 1(-33.05)] = -38.07 kJ
-38.07 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-38.12 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

4676775.8871
This process is favorable at 25°C.

## Reference(s):

Halka, Monica and Nordstrom, Brian. Metals & Metalloids; Infobase Publishing: New York, NY, 2011; pg. 49.