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H2S + 3KClO2 → SO2 + 3KClO + H2O

The reaction of hydrogen sulfide and potassium chlorite yields sulfur dioxide, potassium hypochlorite, 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

General equation

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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide1
Reducing
Reducing
KClO2Potassium chlorite3
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide1
Oxidized
KClOPotassium hypochlorite3
Reduced
H2OWater1

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and potassium chlorite
ΔrG−671.2 kJ/mol
K3.88 × 10117
pK−117.59
H2SUn-ionized aqueous solution + 3KClO2Ionized aqueous solution
SO2Gas + 3KClOIonized 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
−664.8−671.224
per 1 mol of
−664.8−671.224
per 1 mol of
−221.6−223.78.0
per 1 mol of
−664.8−671.224
−221.6−223.78.0
per 1 mol of
−664.8−671.224

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and potassium chlorite
ΔrG−671.7 kJ/mol
K4.75 × 10117
pK−117.68
H2SUn-ionized aqueous solution + 3KClO2Ionized aqueous solution
SO2Un-ionized aqueous solution + 3KClOIonized 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
−690.9−671.7−63
per 1 mol of
−690.9−671.7−63
per 1 mol of
−230.3−223.9−21
per 1 mol of
−690.9−671.7−63
−230.3−223.9−21
per 1 mol of
−690.9−671.7−63

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
SO2 (l)-320.5[1]
SO2 (g)-296.830[1]-300.194[1]248.22[1]39.87[1]
SO2 (ao)-322.980[1]-300.676[1]161.9[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]
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (ai):Ionized aqueous solution, (cr):Crystalline solid

References

List of references

  1. 1