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2H2S + 3PbO2 → 2SO2 + 3Pb + 2H2O

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Reaction of hydrogen sulfide and lead(IV) oxide
2H2SHydrogen sulfide + 3PbO2Lead(IV) oxide
⟶
2SO2Sulfur dioxide + 3PbLead + 2H2OWater

The reaction of hydrogen sulfide and lead(IV) oxide yields sulfur dioxide, lead, 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 lead(IV) oxide
2H2SHydrogen sulfide + 3PbO2Lead(IV) oxide
⟶
2SO2Sulfur dioxide + 3PbLead + 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 lead(IV) oxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide2
Reducing
Reducing
PbO2Lead(IV) oxide3
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide2
Oxidized
–
PbLead3
Reduced
–
H2OWater2
–
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and lead(IV) oxide
◆
ΔrG−355.54 kJ/mol
K1.94 × 1062
pK−62.29
2H2SGas + 3PbO2Crystalline solid
⟶
2SO2Gas + 3PbCrystalline 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
−291.9−355.54213.347.26
per 1 mol of
−145.9−177.77106.723.63
per 1 mol of
−97.30−118.5171.1015.75
per 1 mol of
−145.9−177.77106.723.63
per 1 mol of
−97.30−118.5171.1015.75
per 1 mol of
−145.9−177.77106.723.63

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and lead(IV) oxide
◆
ΔrG−367.00 kJ/mol
K1.98 × 1064
pK−64.30
2H2SUn-ionized aqueous solution + 3PbO2Crystalline solid
⟶
2SO2Gas + 3PbCrystalline 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
−253.7−367.00383–
per 1 mol of
−126.8−183.50192–
per 1 mol of
−84.57−122.33128–
per 1 mol of
−126.8−183.50192–
per 1 mol of
−84.57−122.33128–
per 1 mol of
−126.8−183.50192–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and lead(IV) oxide
◆
ΔrG−367.96 kJ/mol
K2.91 × 1064
pK−64.46
2H2SUn-ionized aqueous solution + 3PbO2Crystalline solid
⟶
2SO2Un-ionized aqueous solution + 3PbCrystalline 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
−306.0−367.96210–
per 1 mol of
−153.0−183.98105–
per 1 mol of
−102.0−122.6570.0–
per 1 mol of
−153.0−183.98105–
per 1 mol of
−102.0−122.6570.0–
per 1 mol of
−153.0−183.98105–

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]–
PbO2 (cr)-277.4[1]-217.33[1]68.6[1]64.64[1]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid

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]–
Pb (cr)0[1]0[1]64.81[1]26.44[1]
Pb (g)195.0[1]161.9[1]175.373[1]20.786[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

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)