## Cl2 (g) + 1 H2S (aq) → S (s rhombic) + 2 HCl (aq)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

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 Cl2            Mass: g or Gas Volume: L H2S            Mass: g or Solution Volume: mL of Concentration: mol/L S              Mass: g HCl            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(S (s rhombic)) + 2ΔHf(HCl (aq))] - [1ΔHf(Cl2 (g)) + 1ΔHf(H2S (aq))]
[1(0) + 2(-167.15)] - [1(0) + 1(129.03)] = -463.33 kJ
-463.33 kJ     (exothermic)

## Entropy Change

[1ΔSf(S (s rhombic)) + 2ΔSf(HCl (aq))] - [1ΔSf(Cl2 (g)) + 1ΔSf(H2S (aq))]
[1(31.92) + 2(56.48)] - [1(222.97) + 1(228.07)] = -306.16 J/K
-306.16 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(S (s rhombic)) + 2ΔGf(HCl (aq))] - [1ΔGf(Cl2 (g)) + 1ΔGf(H2S (aq))]
[1(0) + 2(-131.25)] - [1(0) + 1(80.08)] = -342.58 kJ
-342.58 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-372.05 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

1.0489599847e+060
This process is favorable at 25°C.