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11H2S + 6KClO3 → 5SO2 + 3Cl2 + 6KHS + 8H2O

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Reaction of hydrogen sulfide and potassium chlorate
11H2SHydrogen sulfide + 6KClO3Potassium chlorate
⟶
5SO2Sulfur dioxide + 3Cl2Chlorine + 6KHSPotassium hydrogensulfide + 8H2OWater

The reaction of hydrogen sulfide and potassium chlorate yields sulfur dioxide, chlorine, potassium hydrogensulfide, 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 chlorate
11H2SHydrogen sulfide + 6KClO3Potassium chlorate
⟶
5SO2Sulfur dioxide + 3Cl2Chlorine + 6KHSPotassium hydrogensulfide + 8H2OWater

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 sulfide11
Reducing
Reducing
KClO3Potassium chlorate6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide5
Oxidized
–
Cl2Chlorine3
Reduced
–
KHSPotassium hydrogensulfide6
–
–
H2OWater8
–
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and potassium chlorate
11H2SGas + 6KClO3Crystalline solid
⟶
5SO2Gas + 3Cl2Gas + 6KHSCrystalline solid + 8H2OLiquid
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
−2748.08––377.23
per 1 mol of
−249.825––34.294
per 1 mol of
−458.013––62.872
per 1 mol of
−549.616––75.446
per 1 mol of
−916.027––125.74
−458.013––62.872
per 1 mol of
−343.510––47.154

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and potassium chlorate
◆
ΔrG−2971.69 kJ/mol
K4.15 × 10520
pK−520.62
11H2SUn-ionized aqueous solution + 6KClO3Ionized aqueous solution
⟶
5SO2Gas + 3Cl2Gas + 6KHSIonized aqueous solution + 8H2OLiquid
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
−2815.4−2971.69542–
per 1 mol of
−255.95−270.15449.3–
per 1 mol of
−469.23−495.28290.3–
per 1 mol of
−563.08−594.338108–
per 1 mol of
−938.47−990.563181–
−469.23−495.28290.3–
per 1 mol of
−351.93−371.46167.8–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and potassium chlorate
◆
ΔrG−2950.87 kJ/mol
K9.33 × 10516
pK−516.97
11H2SUn-ionized aqueous solution + 6KClO3Ionized aqueous solution
⟶
5SO2Gas + 3Cl2Un-ionized aqueous solution + 6KHSIonized aqueous solution + 8H2OLiquid
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
−2885.6−2950.87235–
per 1 mol of
−262.33−268.26121.4–
per 1 mol of
−480.93−491.81239.2–
per 1 mol of
−577.12−590.17447.0–
per 1 mol of
−961.87−983.62378.3–
−480.93−491.81239.2–
per 1 mol of
−360.70−368.85929.4–

Changes in aqueous solution (3)

Reaction of hydrogen sulfide and potassium chlorate
◆
ΔrG−2974.10 kJ/mol
K1.10 × 10521
pK−521.04
11H2SUn-ionized aqueous solution + 6KClO3Ionized aqueous solution
⟶
5SO2Un-ionized aqueous solution + 3Cl2Gas + 6KHSIonized aqueous solution + 8H2OLiquid
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
−2946.1−2974.10110–
per 1 mol of
−267.83−270.37310.0–
per 1 mol of
−491.02−495.68318.3–
per 1 mol of
−589.22−594.82022.0–
per 1 mol of
−982.03−991.36736.7–
−491.02−495.68318.3–
per 1 mol of
−368.26−371.76213.8–

Changes in aqueous solution (4)

Reaction of hydrogen sulfide and potassium chlorate
◆
ΔrG−2953.28 kJ/mol
K2.47 × 10517
pK−517.39
11H2SUn-ionized aqueous solution + 6KClO3Ionized aqueous solution
⟶
5SO2Un-ionized aqueous solution + 3Cl2Un-ionized aqueous solution + 6KHSIonized aqueous solution + 8H2OLiquid
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
−3016.3−2953.28−196–
per 1 mol of
−274.21−268.480−17.8–
per 1 mol of
−502.72−492.213−32.7–
per 1 mol of
−603.26−590.656−39.2–
per 1 mol of
−1005.4−984.427−65.3–
−502.72−492.213−32.7–
per 1 mol of
−377.04−369.160−24.5–

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
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]–
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]–
KHS (cr)-265.10[1]––75.31[1]
KHS (ai)-269.9[1]-271.19[1]165.3[1]–
KHS (cr)
0.25 hydrate
-337.2[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, (cr):Crystalline solid, (ai):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)