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2KClO + H2O 🔥→ K2O + Cl2↑ + H2O2

The reaction of potassium hypochlorite and water yields potassium oxide, chlorine, and hydrogen peroxide (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

General equation

Reaction of self redoxing species and water
Self-redoxing speciesSelf redox agent + H2ONon-redox agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KClOPotassium hypochlorite2
Self redox agent
Self redoxing
H2OWater1
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2OPotassium oxide1
Cl2Chlorine1
Reduced
H2O2Hydrogen peroxide1
Oxidized

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of potassium hypochlorite and water
ΔrG421.0 kJ/mol
K0.18 × 10−73
pK73.76
2KClOIonized aqueous solution + H2OLiquid
🔥
K2OCrystalline solid + Cl2Gas + H2O2Un-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
452.0421.099
226.0210.550
per 1 mol of
452.0421.099
per 1 mol of
452.0421.099
per 1 mol of
452.0421.099
per 1 mol of
452.0421.099

Changes in aqueous solution (2)

Reaction of potassium hypochlorite and water
ΔrG427.9 kJ/mol
K0.11 × 10−74
pK74.96
2KClOIonized aqueous solution + H2OLiquid
🔥
K2OCrystalline solid + Cl2Un-ionized aqueous solution + H2O2Un-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
428.6427.9−3
214.3213.9−2
per 1 mol of
428.6427.9−3
per 1 mol of
428.6427.9−3
per 1 mol of
428.6427.9−3
per 1 mol of
428.6427.9−3

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
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]
H2O2 (l)-187.78[1]-120.35[1]109.6[1]89.1[1]
H2O2 (g)-136.31[1]-105.57[1]232.7[1]43.1[1]
H2O2 (ao)-191.17[1]-134.03[1]143.9[1]
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid

References

List of references

  1. 1
  2. 2
    James G. Speight (2017)
    Lange's Handbook of Chemistry, 17th edition
    McGraw Hill Education