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2H2S + 2KClO4 → SO2 + 2ClO2 + K2S + 2H2O

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Reaction of hydrogen sulfide and potassium perchlorate
2H2SHydrogen sulfide + 2KClO4Potassium perchlorate
⟶
SO2Sulfur dioxide + 2ClO2Chlorine dioxide + K2SPotassium sulfide + 2H2OWater

The reaction of hydrogen sulfide and potassium perchlorate yields sulfur dioxide, chlorine dioxide, potassium sulfide, 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 perchlorate
2H2SHydrogen sulfide + 2KClO4Potassium perchlorate
⟶
SO2Sulfur dioxide + 2ClO2Chlorine dioxide + K2SPotassium sulfide + 2H2OWater

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 perchlorate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide2
Reducing
Reducing
KClO4Potassium perchlorate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide1
Oxidized
–
ClO2Chlorine dioxide2
Reduced
–
K2SPotassium sulfide1
–
–
H2OWater2
–
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and potassium perchlorate
◆
ΔrG−224.2 kJ/mol
K1.90 × 1039
pK−39.28
2H2SGas + 2KClO4Crystalline solid
⟶
SO2Gas + 2ClO2Gas + K2SCrystalline solid + 2H2OLiquid
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
−137.4−224.2293–
per 1 mol of
−68.70−112.1147–
−68.70−112.1147–
per 1 mol of
−137.4−224.2293–
per 1 mol of
−68.70−112.1147–
per 1 mol of
−137.4−224.2293–
per 1 mol of
−68.70−112.1147–

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and potassium perchlorate
◆
ΔrG−374.9 kJ/mol
K4.78 × 1065
pK−65.68
2H2SUn-ionized aqueous solution + 2KClO4Ionized aqueous solution
⟶
SO2Gas + 2ClO2Gas + K2SIonized aqueous solution + 2H2OLiquid
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
−292.2−374.9281–
per 1 mol of
−146.1−187.4141–
−146.1−187.4141–
per 1 mol of
−292.2−374.9281–
per 1 mol of
−146.1−187.4141–
per 1 mol of
−292.2−374.9281–
per 1 mol of
−146.1−187.4141–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and potassium perchlorate
◆
ΔrG−375.7 kJ/mol
K6.60 × 1065
pK−65.82
2H2SUn-ionized aqueous solution + 2KClO4Ionized aqueous solution
⟶
SO2Gas + 2ClO2Un-ionized aqueous solution + K2SIonized aqueous solution + 2H2OLiquid
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
−347.4−375.797–
per 1 mol of
−173.7−187.849–
−173.7−187.849–
per 1 mol of
−347.4−375.797–
per 1 mol of
−173.7−187.849–
per 1 mol of
−347.4−375.797–
per 1 mol of
−173.7−187.849–

Changes in aqueous solution (3)

Reaction of hydrogen sulfide and potassium perchlorate
◆
ΔrG−375.4 kJ/mol
K5.85 × 1065
pK−65.77
2H2SUn-ionized aqueous solution + 2KClO4Ionized aqueous solution
⟶
SO2Un-ionized aqueous solution + 2ClO2Gas + K2SIonized aqueous solution + 2H2OLiquid
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
−318.3−375.4195–
per 1 mol of
−159.2−187.797.5–
−159.2−187.797.5–
per 1 mol of
−318.3−375.4195–
per 1 mol of
−159.2−187.797.5–
per 1 mol of
−318.3−375.4195–
per 1 mol of
−159.2−187.797.5–

Changes in aqueous solution (4)

Reaction of hydrogen sulfide and potassium perchlorate
◆
ΔrG−376.2 kJ/mol
K8.08 × 1065
pK−65.91
2H2SUn-ionized aqueous solution + 2KClO4Ionized aqueous solution
⟶
SO2Un-ionized aqueous solution + 2ClO2Un-ionized aqueous solution + K2SIonized aqueous solution + 2H2OLiquid
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
−373.5−376.211–
per 1 mol of
−186.8−188.15.5–
−186.8−188.15.5–
per 1 mol of
−373.5−376.211–
per 1 mol of
−186.8−188.15.5–
per 1 mol of
−373.5−376.211–
per 1 mol of
−186.8−188.15.5–

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]–
KClO4 (cr)-432.75[1]-303.09[1]151.0[1]112.38[1]
KClO4 (ai)-381.71[1]-291.79[1]284.5[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]–
ClO2 (g)102.5[1]120.5[1]256.84[1]41.97[1]
ClO2 (ao)74.9[1]120.1[1]164.8[1]–
K2S (cr)-380.7[1]-364.0[1]105[1]–
K2S (ai)-471.5[1]-480.7[1]190.4[1]–
K2S (cr)
2 hydrate
-975.3[1]–––
K2S (cr)
5 hydrate
-1871.5[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)