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  3. 6HClO 💧⚡→ 3Cl2↑ + 3H2↑ + 2O3↑

6HClO 💧⚡→ 3Cl2↑ + 3H2↑ + 2O3↑

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Electrolysis of aqueous hypochlorous acid without water as reactant
6HClOHypochlorous acid
💧⚡
⟶
3Cl2↑Chlorine + 3H2↑Hydrogen + 2O3↑Ozone

Electrolysis of aqueous hypochlorous acid yields chlorine, hydrogen, and ozone (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

Electrolysis of aqueous hypochlorous acid without water as reactant
6HClOHypochlorous acid
💧⚡
⟶
3Cl2↑Chlorine + 3H2↑Hydrogen + 2O3↑Ozone

General equation

Electrolysis of aqueous solution without water as reactant
Miscible with water/Very soluble in water/Soluble in waterSelf redox agent
💧⚡
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Electrolysis of aqueous hypochlorous acid without water as reactant

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HClOHypochlorous acid6
Self redox agent
Soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cl2Chlorine3
Reduced
–
H2Hydrogen3
Reduced
–
O3Ozone2
Oxidized
–

Thermodynamic changes

Changes in standard condition (1)

Electrolysis of aqueous hypochlorous acid without water as reactant
◆
ΔrG805.8 kJ/mol
K0.68 × 10−141
pK141.17
6HClOUn-ionized aqueous solution
💧⚡
⟶
3Cl2↑Gas + 3H2↑Gas + 2O3↑Gas
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
1010.8805.8687–
per 1 mol of
168.47134.3115–
per 1 mol of
336.93268.6229–
per 1 mol of
336.93268.6229–
per 1 mol of
505.40402.9344–

Changes in standard condition (2)

Electrolysis of aqueous hypochlorous acid without water as reactant
◆
ΔrG827.6 kJ/mol
K0.10 × 10−144
pK144.99
6HClOUn-ionized aqueous solution
💧⚡
⟶
3Cl2↑Gas + 3H2↑Gas + 2O3↑Un-ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
977.2827.6501–
per 1 mol of
162.9137.983.5–
per 1 mol of
325.7275.9167–
per 1 mol of
325.7275.9167–
per 1 mol of
488.6413.8251–

Changes in standard condition (3)

Electrolysis of aqueous hypochlorous acid without water as reactant
◆
ΔrG858.6 kJ/mol
K0.38 × 10−150
pK150.42
6HClOUn-ionized aqueous solution
💧⚡
⟶
3Cl2↑Gas + 3H2↑Un-ionized aqueous solution + 2O3↑Gas
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
998.2858.62026–
per 1 mol of
166.4143.1337.7–
per 1 mol of
332.7286.2675.3–
per 1 mol of
332.7286.2675.3–
per 1 mol of
499.1429.31013–

Changes in standard condition (4)

Electrolysis of aqueous hypochlorous acid without water as reactant
◆
ΔrG880.4 kJ/mol
K0.58 × 10−154
pK154.24
6HClOUn-ionized aqueous solution
💧⚡
⟶
3Cl2↑Gas + 3H2↑Un-ionized aqueous solution + 2O3↑Un-ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
964.6880.41840–
per 1 mol of
160.8146.7306.7–
per 1 mol of
321.5293.5613.3–
per 1 mol of
321.5293.5613.3–
per 1 mol of
482.3440.2920.0–

Changes in standard condition (5)

Electrolysis of aqueous hypochlorous acid without water as reactant
◆
ΔrG826.6 kJ/mol
K0.15 × 10−144
pK144.81
6HClOUn-ionized aqueous solution
💧⚡
⟶
3Cl2↑Un-ionized aqueous solution + 3H2↑Gas + 2O3↑Gas
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
940.6826.6381–
per 1 mol of
156.8137.863.5–
per 1 mol of
313.5275.5127–
per 1 mol of
313.5275.5127–
per 1 mol of
470.3413.3191–

Changes in standard condition (6)

Electrolysis of aqueous hypochlorous acid without water as reactant
◆
ΔrG848.4 kJ/mol
K0.23 × 10−148
pK148.63
6HClOUn-ionized aqueous solution
💧⚡
⟶
3Cl2↑Un-ionized aqueous solution + 3H2↑Gas + 2O3↑Un-ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
907.0848.4195–
per 1 mol of
151.2141.432.5–
per 1 mol of
302.3282.865.0–
per 1 mol of
302.3282.865.0–
per 1 mol of
453.5424.297.5–

Changes in standard condition (7)

Electrolysis of aqueous hypochlorous acid without water as reactant
◆
ΔrG879.4 kJ/mol
K0.86 × 10−154
pK154.06
6HClOUn-ionized aqueous solution
💧⚡
⟶
3Cl2↑Un-ionized aqueous solution + 3H2↑Un-ionized aqueous solution + 2O3↑Gas
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
928.0879.41720–
per 1 mol of
154.7146.6286.7–
per 1 mol of
309.3293.1573.3–
per 1 mol of
309.3293.1573.3–
per 1 mol of
464.0439.7860.0–

Changes in standard condition (8)

Electrolysis of aqueous hypochlorous acid without water as reactant
◆
ΔrG901.2 kJ/mol
K0.13 × 10−157
pK157.88
6HClOUn-ionized aqueous solution
💧⚡
⟶
3Cl2↑Un-ionized aqueous solution + 3H2↑Un-ionized aqueous solution + 2O3↑Un-ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
894.4901.21534–
per 1 mol of
149.1150.2255.7–
per 1 mol of
298.1300.4511.3–
per 1 mol of
298.1300.4511.3–
per 1 mol of
447.2450.6767.0–

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
HClO (g)-78.7[1]-66.1[1]236.67[1]37.15[1]
HClO (ao)-120.9[1]-79.9[1]142[1]–
* (g):Gas, (ao):Un-ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]–
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
O3 (g)142.7[1]163.2[1]238.93[1]39.20[1]
O3 (ao)125.9[1]174.1[1]146[1]–
* (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)