## 2 I2 (s) + 5 Cl2 (g) + 6 H2O (ℓ) → 2 HIO3 (aq) + 10 HCl (aq)

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## Stoichiometry

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 I2             Mass: g Cl2            Mass: g or Gas Volume: L H2O            Mass: g HIO3           Mass: g HCl            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(HIO3 (aq)) + 10ΔHf(HCl (aq))] - [2ΔHf(I2 (s)) + 5ΔHf(Cl2 (g)) + 6ΔHf(H2O (ℓ))]
[2(-221.33) + 10(-167.15)] - [2(0) + 5(0) + 6(-285.83)] = -399.18 kJ
-399.18 kJ     (exothermic)

## Entropy Change

[2ΔSf(HIO3 (aq)) + 10ΔSf(HCl (aq))] - [2ΔSf(I2 (s)) + 5ΔSf(Cl2 (g)) + 6ΔSf(H2O (ℓ))]
[2(118.41) + 10(56.48)] - [2(116.14) + 5(222.97) + 6(69.91)] = -964.97 J/K
-964.97 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(HIO3 (aq)) + 10ΔGf(HCl (aq))] - [2ΔGf(I2 (s)) + 5ΔGf(Cl2 (g)) + 6ΔGf(H2O (ℓ))]
[2(-128.03) + 10(-131.25)] - [2(0) + 5(0) + 6(-237.18)] = -145.48 kJ
-145.48 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-111.47 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

3.0790127612e+025
This process is favorable at 25°C.