You-iggy
  1. Home
  2. Chemical reactions
  3. H2S + 4KClO3 → K2SO4 + 2KClO2 + 2HClO2

H2S + 4KClO3 → K2SO4 + 2KClO2 + 2HClO2

Last updated:
Reaction of hydrogen sulfide and potassium chlorate
H2SHydrogen sulfide + 4KClO3Potassium chlorate
⟶
K2SO4Potassium sulfate + 2KClO2Potassium chlorite + 2HClO2Chlorous acid

The reaction of hydrogen sulfide and potassium chlorate yields potassium sulfate, potassium chlorite, and chlorous acid (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 chlorate
H2SHydrogen sulfide + 4KClO3Potassium chlorate
⟶
K2SO4Potassium sulfate + 2KClO2Potassium chlorite + 2HClO2Chlorous acid

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 chlorate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide1
Reducing
Reducing
KClO3Potassium chlorate4
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2SO4Potassium sulfate1
Oxidized
–
KClO2Potassium chlorite2
Reduced
–
HClO2Chlorous acid2
Reduced
–

Thermodynamic changes

Changes in aqueous solution

Reaction of hydrogen sulfide and potassium chlorate
◆
ΔrG−638.8 kJ/mol
K8.18 × 10111
pK−111.91
H2SUn-ionized aqueous solution + 4KClO3Ionized aqueous solution
⟶
K2SO4Ionized aqueous solution + 2KClO2Ionized aqueous solution + 2HClO2Un-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
−690.3−638.8−171–
per 1 mol of
−690.3−638.8−171–
per 1 mol of
−172.6−159.7−42.8–
per 1 mol of
−690.3−638.8−171–
per 1 mol of
−345.1−319.4−85.5–
per 1 mol of
−345.1−319.4−85.5–

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]–
KClO3 (cr)-397.73[1]-296.25[1]143.1[1]100.25[1]
KClO3 (ai)-356.35[1]-291.22[1]264.8[1]–
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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
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]
KClO2 (ai)-318.8[1]-266.1[1]203.8[1]–
HClO2 (ao)-51.9[1]5.9[1]188.3[1]–
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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)