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10H2S + 6KClO4 → 7SO2 + 3Cl2 + 3K2S + 10H2O

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Reaction of hydrogen sulfide and potassium perchlorate
10H2SHydrogen sulfide + 6KClO4Potassium perchlorate
⟶
7SO2Sulfur dioxide + 3Cl2Chlorine + 3K2SPotassium sulfide + 10H2OWater

The reaction of hydrogen sulfide and potassium perchlorate yields sulfur dioxide, chlorine, 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
10H2SHydrogen sulfide + 6KClO4Potassium perchlorate
⟶
7SO2Sulfur dioxide + 3Cl2Chlorine + 3K2SPotassium sulfide + 10H2OWater

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 sulfide10
Reducing
Reducing
KClO4Potassium perchlorate6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide7
Oxidized
–
Cl2Chlorine3
Reduced
–
K2SPotassium sulfide3
–
–
H2OWater10
–
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and potassium perchlorate
◆
ΔrG−3410.5 kJ/mol
K3.12 × 10597
pK−597.49
10H2SGas + 6KClO4Crystalline solid
⟶
7SO2Gas + 3Cl2Gas + 3K2SCrystalline solid + 10H2OLiquid
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
−3275.4−3410.5457–
per 1 mol of
−327.54−341.0545.7–
−545.90−568.4276.2–
per 1 mol of
−467.91−487.2165.3–
per 1 mol of
−1091.8−1136.8152–
per 1 mol of
−1091.8−1136.8152–
per 1 mol of
−327.54−341.0545.7–

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and potassium perchlorate
◆
ΔrG−3885.7 kJ/mol
K5.56 × 10680
pK−680.75
10H2SUn-ionized aqueous solution + 6KClO4Ionized aqueous solution
⟶
7SO2Gas + 3Cl2Gas + 3K2SIonized aqueous solution + 10H2OLiquid
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
−3663.4−3885.7760–
per 1 mol of
−366.34−388.5776.0–
−610.57−647.62127–
per 1 mol of
−523.34−555.10109–
per 1 mol of
−1221.1−1295.2253–
per 1 mol of
−1221.1−1295.2253–
per 1 mol of
−366.34−388.5776.0–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and potassium perchlorate
◆
ΔrG−3864.9 kJ/mol
K1.26 × 10677
pK−677.10
10H2SUn-ionized aqueous solution + 6KClO4Ionized aqueous solution
⟶
7SO2Gas + 3Cl2Un-ionized aqueous solution + 3K2SIonized aqueous solution + 10H2OLiquid
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
−3733.6−3864.9454–
per 1 mol of
−373.36−386.4945.4–
−622.27−644.1575.7–
per 1 mol of
−533.37−552.1364.9–
per 1 mol of
−1244.5−1288.3151–
per 1 mol of
−1244.5−1288.3151–
per 1 mol of
−373.36−386.4945.4–

Changes in aqueous solution (3)

Reaction of hydrogen sulfide and potassium perchlorate
◆
ΔrG−3889.1 kJ/mol
K2.19 × 10681
pK−681.34
10H2SUn-ionized aqueous solution + 6KClO4Ionized aqueous solution
⟶
7SO2Un-ionized aqueous solution + 3Cl2Gas + 3K2SIonized aqueous solution + 10H2OLiquid
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
−3846.4−3889.1156–
per 1 mol of
−384.64−388.9115.6–
−641.07−648.1826.0–
per 1 mol of
−549.49−555.5922.3–
per 1 mol of
−1282.1−1296.452.0–
per 1 mol of
−1282.1−1296.452.0–
per 1 mol of
−384.64−388.9115.6–

Changes in aqueous solution (4)

Reaction of hydrogen sulfide and potassium perchlorate
◆
ΔrG−3868.3 kJ/mol
K4.98 × 10677
pK−677.70
10H2SUn-ionized aqueous solution + 6KClO4Ionized aqueous solution
⟶
7SO2Un-ionized aqueous solution + 3Cl2Un-ionized aqueous solution + 3K2SIonized aqueous solution + 10H2OLiquid
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
−3916.6−3868.3−150–
per 1 mol of
−391.66−386.83−15.0–
−652.77−644.72−25.0–
per 1 mol of
−559.51−552.61−21.4–
per 1 mol of
−1305.5−1289.4−50.0–
per 1 mol of
−1305.5−1289.4−50.0–
per 1 mol of
−391.66−386.83−15.0–

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]–
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[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)