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H2S + 4HClO2 → SO3 + 4HClO + H2O

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Reaction of hydrogen sulfide and chlorous acid
H2SHydrogen sulfide + 4HClO2Chlorous acid
⟶
SO3Sulfur trioxide + 4HClOHypochlorous acid + H2OWater

The reaction of hydrogen sulfide and chlorous acid yields sulfur trioxide, hypochlorous acid, 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 chlorous acid
H2SHydrogen sulfide + 4HClO2Chlorous acid
⟶
SO3Sulfur trioxide + 4HClOHypochlorous acid + 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 chlorous acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide1
Reducing
Reducing
HClO2Chlorous acid4
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO3Sulfur trioxide1
Oxidized
–
HClOHypochlorous acid4
Reduced
–
H2OWater1
–
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and chlorous acid
◆
ΔrG−926.7 kJ/mol
K2.24 × 10162
pK−162.35
H2SUn-ionized aqueous solution + 4HClO2Un-ionized aqueous solution
⟶
SO3Crystalline solidβ + 4HClOUn-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
−976.6−926.7−166–
per 1 mol of
−976.6−926.7−166–
per 1 mol of
−244.2−231.7−41.5–
per 1 mol of
−976.6−926.7−166–
per 1 mol of
−244.2−231.7−41.5–
per 1 mol of
−976.6−926.7−166–

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]–
HClO2 (ao)-51.9[1]5.9[1]188.3[1]–
* (g):Gas, (ao):Un-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
SO3 (cr)
β
-454.51[1]-374.21[1]70.7[1]–
SO3 (l)-441.04[1]-373.75[1]113.8[1]–
SO3 (g)-395.72[1]-371.06[1]256.76[1]50.67[1]
HClO (g)-78.7[1]-66.1[1]236.67[1]37.15[1]
HClO (ao)-120.9[1]-79.9[1]142[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, (l):Liquid, (g):Gas, (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)