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H2S + 2KClO2 → K2SO3 + Cl2 + H2O

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Reaction of hydrogen sulfide and potassium chlorite
H2SHydrogen sulfide + 2KClO2Potassium chlorite
⟶
K2SO3Potassium sulfite + Cl2Chlorine + H2OWater

The reaction of hydrogen sulfide and potassium chlorite yields potassium sulfite, 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 hydrogen sulfide and potassium chlorite
H2SHydrogen sulfide + 2KClO2Potassium chlorite
⟶
K2SO3Potassium sulfite + Cl2Chlorine + H2OWater

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of hydrogen sulfide and potassium chlorite

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide1
Reducing
Reducing
KClO2Potassium chlorite2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2SO3Potassium sulfite1
Oxidized
–
Cl2Chlorine1
Reduced
–
H2OWater1
–
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and potassium chlorite
◆
ΔrG−730.2 kJ/mol
K8.42 × 10127
pK−127.93
H2SUn-ionized aqueous solution + 2KClO2Ionized aqueous solution
⟶
K2SO3Ionized aqueous solution + Cl2Gas + H2OLiquid
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
−748.6−730.2−60–
per 1 mol of
−748.6−730.2−60–
per 1 mol of
−374.3−365.1−30–
per 1 mol of
−748.6−730.2−60–
per 1 mol of
−748.6−730.2−60–
per 1 mol of
−748.6−730.2−60–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and potassium chlorite
◆
ΔrG−723.3 kJ/mol
K5.21 × 10126
pK−126.72
H2SUn-ionized aqueous solution + 2KClO2Ionized aqueous solution
⟶
K2SO3Ionized aqueous solution + Cl2Un-ionized aqueous solution + H2OLiquid
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
−772.0−723.3−162–
per 1 mol of
−772.0−723.3−162–
per 1 mol of
−386.0−361.6−81.0–
per 1 mol of
−772.0−723.3−162–
per 1 mol of
−772.0−723.3−162–
per 1 mol of
−772.0−723.3−162–

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
H2S (g)-20.63[1]-33.56[1]205.79[1]34.23[1]
H2S (ao)-39.7[1]-27.83[1]121[1]–
KClO2 (ai)-318.8[1]-266.1[1]203.8[1]–
* (g):Gas, (ao):Un-ionized aqueous solution, (ai):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
K2SO3 (cr)-1125.5[1]–––
K2SO3 (ai)-1140.1[1]-1053.1[1]176[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, (ai):Ionized aqueous solution, (g):Gas, (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)