5 HClO2 (aq) → 4 ClO2 (g) + HCl (aq) + 2 H2O (ℓ)

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Reaction Type:

Decomposition

Stoichiometry

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Heat Added: kJ
HClO2          Mass: g  or Solution Volume: mL of Concentration: mol/L
ClO2           Mass: g  or Gas Volume: L
HCl            Mass: g
H2O            Mass: g

Enthalpy of Reaction

[4ΔHf(ClO2 (g)) + 1ΔHf(HCl (aq)) + 2ΔHf(H2O (ℓ))] - [5ΔHf(HClO2 (aq))]
[4(102.51) + 1(-167.15) + 2(-285.83)] - [5(-66.53)] = 3.88 kJ
3.88 kJ     (endothermic)

Entropy Change

[4ΔSf(ClO2 (g)) + 1ΔSf(HCl (aq)) + 2ΔSf(H2O (ℓ))] - [5ΔSf(HClO2 (aq))]
[4(256.77) + 1(56.48) + 2(69.91)] - [5(101.25)] = 717.13 J/K
717.13 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[4ΔGf(ClO2 (g)) + 1ΔGf(HCl (aq)) + 2ΔGf(H2O (ℓ))] - [5ΔGf(HClO2 (aq))]
[4(120.33) + 1(-131.25) + 2(-237.18)] - [5(17.15)] = -210.04 kJ
-210.04 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-209.93 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

6.3017837229e+036
This process is favorable at 25°C.

Reference(s):

Swaddle, T.W. Inorganic Chemistry; Academic Press: San Diego, 1997; p 225.

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