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4KClO + 2H2O 💧⚡→ 4KOH + 2Cl2↑ + O2↑

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Electrolysis of aqueous potassium hypochlorite with water as non-redox agent
4KClOPotassium hypochlorite + 2H2OWater
💧⚡
⟶
4KOHPotassium hydroxide + 2Cl2↑Chlorine + O2↑Oxygen

Electrolysis of aqueous potassium hypochlorite yields potassium hydroxide, chlorine, and oxygen (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 potassium hypochlorite with water as non-redox agent
4KClOPotassium hypochlorite + 2H2OWater
💧⚡
⟶
4KOHPotassium hydroxide + 2Cl2↑Chlorine + O2↑Oxygen

General equation

Electrolysis of aqueous solution with water as non redox agent
Miscible with water/Very soluble in water/Soluble in waterSelf redox agent + H2ONon-redox agent
💧⚡
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Electrolysis of aqueous potassium hypochlorite with water as non-redox agent

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KClOPotassium hypochlorite4
Oxidizing
Soluble in water
H2OWater2
–
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
KOHPotassium hydroxide4
–
–
Cl2Chlorine2
Reduced
–
O2Oxygen1
–
–

Thermodynamic changes

Changes in aqueous solution (1)

Electrolysis of aqueous potassium hypochlorite with water as non-redox agent
◆
ΔrG−7.7 kJ/mol
K2.23 × 101
pK−1.35
4KClOIonized aqueous solution + 2H2OLiquid
💧⚡
⟶
4KOHIonized aqueous solution + 2Cl2↑Gas + O2↑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
79.8−7.7294–
19.9−1.973.5–
per 1 mol of
39.9−3.9147–
19.9−1.973.5–
per 1 mol of
39.9−3.9147–
per 1 mol of
79.8−7.7294–

Changes in aqueous solution (2)

Electrolysis of aqueous potassium hypochlorite with water as non-redox agent
◆
ΔrG8.7 kJ/mol
K0.30 × 10−1
pK1.52
4KClOIonized aqueous solution + 2H2OLiquid
💧⚡
⟶
4KOHIonized aqueous solution + 2Cl2↑Gas + O2↑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
68.18.7200–
17.02.250.0–
per 1 mol of
34.04.3100–
17.02.250.0–
per 1 mol of
34.04.3100–
per 1 mol of
68.18.7200–

Changes in aqueous solution (3)

Electrolysis of aqueous potassium hypochlorite with water as non-redox agent
◆
ΔrG6.1 kJ/mol
K0.85 × 10−1
pK1.07
4KClOIonized aqueous solution + 2H2OLiquid
💧⚡
⟶
4KOHIonized aqueous solution + 2Cl2↑Un-ionized aqueous solution + O2↑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
33.06.190–
8.251.523–
per 1 mol of
16.53.045–
8.251.523–
per 1 mol of
16.53.045–
per 1 mol of
33.06.190–

Changes in aqueous solution (4)

Electrolysis of aqueous potassium hypochlorite with water as non-redox agent
◆
ΔrG22.5 kJ/mol
K0.11 × 10−3
pK3.94
4KClOIonized aqueous solution + 2H2OLiquid
💧⚡
⟶
4KOHIonized aqueous solution + 2Cl2↑Un-ionized aqueous solution + O2↑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
21.322.5−5–
5.335.63−1–
per 1 mol of
10.711.3−3–
5.335.63−1–
per 1 mol of
10.711.3−3–
per 1 mol of
21.322.5−5–

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
KClO (ai)-359.4[1]-320.0[1]146[1]–
H2O (cr)––––
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (l):Liquid, (g):Gas

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
KOH (cr)-424.764[1]-379.08[1]78.9[1]64.9[1]
KOH (g)-231.0[1]-232.6[1]238.3[1]49.20[1]
KOH (ai)-482.37[1]-440.50[1]91.6[1]-126.8[1]
KOH (cr)
1 hydrate
-748.9[1]-645.1[1]117.2[1]–
KOH (cr)
2 hydrate
-1051.0[1]-887.3[1]150.6[1]–
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]–
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[1]–
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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)