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8KClO + 4H2SO4 → 4K2SO4 + 2ClO2↑ + 3Cl2↑ + 4H2O

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Reaction of potassium hypochlorite and sulfuric acid
8KClOPotassium hypochlorite + 4H2SO4Sulfuric acid
⟶
4K2SO4Potassium sulfate + 2ClO2↑Chlorine dioxide + 3Cl2↑Chlorine + 4H2OWater

The reaction of potassium hypochlorite and sulfuric acid yields potassium sulfate, chlorine dioxide, chlorine, and water (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

Reaction of potassium hypochlorite and sulfuric acid
8KClOPotassium hypochlorite + 4H2SO4Sulfuric acid
⟶
4K2SO4Potassium sulfate + 2ClO2↑Chlorine dioxide + 3Cl2↑Chlorine + 4H2OWater

General equation

Reaction of self redoxing species and acid
Self-redoxing speciesSelf redox agent + AcidNon-redox agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of potassium hypochlorite and sulfuric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KClOPotassium hypochlorite8
–
Self redoxing
H2SO4Sulfuric acid4
–
Acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2SO4Potassium sulfate4
–
–
ClO2Chlorine dioxide2
Oxidized
–
Cl2Chlorine3
Reduced
–
H2OWater4
–
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of potassium hypochlorite and sulfuric acid
◆
ΔrG−413.7 kJ/mol
K3.00 × 1072
pK−72.48
8KClOIonized aqueous solution + 4H2SO4Ionized aqueous solution
⟶
4K2SO4Ionized aqueous solution + 2ClO2↑Gas + 3Cl2↑Gas + 4H2OLiquid
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
−82.1−413.71115–
−10.3−51.71139.4–
per 1 mol of
−20.5−103.4278.8–
per 1 mol of
−20.5−103.4278.8–
per 1 mol of
−41.0−206.8557.5–
per 1 mol of
−27.4−137.9371.7–
per 1 mol of
−20.5−103.4278.8–

Changes in aqueous solution (2)

Reaction of potassium hypochlorite and sulfuric acid
◆
ΔrG−392.9 kJ/mol
K6.81 × 1068
pK−68.83
8KClOIonized aqueous solution + 4H2SO4Ionized aqueous solution
⟶
4K2SO4Ionized aqueous solution + 2ClO2↑Gas + 3Cl2↑Un-ionized aqueous solution + 4H2OLiquid
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
−152.3−392.9808–
−19.04−49.11101–
per 1 mol of
−38.08−98.22202–
per 1 mol of
−38.08−98.22202–
per 1 mol of
−76.15−196.4404–
per 1 mol of
−50.77−131.0269–
per 1 mol of
−38.08−98.22202–

Changes in aqueous solution (3)

Reaction of potassium hypochlorite and sulfuric acid
◆
ΔrG−414.5 kJ/mol
K4.14 × 1072
pK−72.62
8KClOIonized aqueous solution + 4H2SO4Ionized aqueous solution
⟶
4K2SO4Ionized aqueous solution + 2ClO2↑Un-ionized aqueous solution + 3Cl2↑Gas + 4H2OLiquid
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
−137.3−414.5930–
−17.16−51.81116–
per 1 mol of
−34.33−103.6233–
per 1 mol of
−34.33−103.6233–
per 1 mol of
−68.65−207.3465–
per 1 mol of
−45.77−138.2310–
per 1 mol of
−34.33−103.6233–

Changes in aqueous solution (4)

Reaction of potassium hypochlorite and sulfuric acid
◆
ΔrG−393.7 kJ/mol
K9.40 × 1068
pK−68.97
8KClOIonized aqueous solution + 4H2SO4Ionized aqueous solution
⟶
4K2SO4Ionized aqueous solution + 2ClO2↑Un-ionized aqueous solution + 3Cl2↑Un-ionized aqueous solution + 4H2OLiquid
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
−207.5−393.7624–
−25.94−49.2178.0–
per 1 mol of
−51.88−98.42156–
per 1 mol of
−51.88−98.42156–
per 1 mol of
−103.8−196.8312–
per 1 mol of
−69.17−131.2208–
per 1 mol of
−51.88−98.42156–

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]–
H2SO4 (cr)––––
H2SO4 (l)-813.989[1]-690.003[1]156.904[1]138.91[1]
H2SO4 (ai)-909.27[1]-744.53[1]20.1[1]-293[1]
H2SO4 (l)
1 hydrate
-1127.621[1]-950.383[1]211.54[1]214.85[1]
H2SO4 (l)
2 hydrate
-1427.100[1]-1199.650[1]276.40[1]260.83[1]
H2SO4 (l)
3 hydrate
-1720.402[1]-1443.980[1]345.39[1]318.95[1]
H2SO4 (l)
4 hydrate
-2011.199[1]-1685.863[1]414.59[1]382.21[1]
H2SO4 (l)
6.5 hydrate
-2733.256[1]-2285.734[1]587.89[1]570.28[1]
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (l):Liquid

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
K2SO4 (cr)-1437.79[1]-1321.37[1]175.56[1]131.46[1]
K2SO4 (g)-1096[1]-1033[1]364[1]108.8[1]
K2SO4 (ai)-1414.02[1]-1311.07[1]225.1[1]-251[1]
ClO2 (g)102.5[1]120.5[1]256.84[1]41.97[1]
ClO2 (ao)74.9[1]120.1[1]164.8[1]–
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[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]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid

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)