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3H2 + PbSO4 → S + PbO + 3H2O

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Reaction of hydrogen and lead(II) sulfate
3H2Hydrogen + PbSO4Lead(II) sulfate
⟶
SSulfur + PbOLead(II) oxide + 3H2OWater

The reaction of hydrogen and lead(II) sulfate yields sulfur, lead(II) oxide, 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 and lead(II) sulfate
3H2Hydrogen + PbSO4Lead(II) sulfate
⟶
SSulfur + PbOLead(II) oxide + 3H2OWater

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of hydrogen and lead(II) sulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2Hydrogen3
Reducing
Reducing
PbSO4Lead(II) sulfate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
SSulfur1
Reduced
–
PbOLead(II) oxide1
–
–
H2OWater3
Oxidized
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen and lead(II) sulfate
◆
ΔrG−86.14 kJ/mol
K1.23 × 1015
pK−15.09
3H2Gas + PbSO4Crystalline solid
⟶
SCrystalline solidrhombic + PbOCrystalline solidmassicot, yellow + 3H2OLiquid
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
−154.87−86.14−230.39104.60
per 1 mol of
−51.623−28.71−76.79734.867
per 1 mol of
−154.87−86.14−230.39104.60
per 1 mol of
−154.87−86.14−230.39104.60
per 1 mol of
−154.87−86.14−230.39104.60
per 1 mol of
−51.623−28.71−76.79734.867

Changes in standard condition (2)

Reaction of hydrogen and lead(II) sulfate
◆
ΔrG−87.18 kJ/mol
K1.88 × 1015
pK−15.27
3H2Gas + PbSO4Crystalline solid
⟶
SCrystalline solidrhombic + PbOCrystalline solidlitharge, red + 3H2OLiquid
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
−156.54−87.18−232.6104.64
per 1 mol of
−52.180−29.06−77.5334.880
per 1 mol of
−156.54−87.18−232.6104.64
per 1 mol of
−156.54−87.18−232.6104.64
per 1 mol of
−156.54−87.18−232.6104.64
per 1 mol of
−52.180−29.06−77.5334.880

Changes in standard condition (3)

Reaction of hydrogen and lead(II) sulfate
3H2Gas + PbSO4Crystalline solid
⟶
SCrystalline solidmonoclinic + PbOCrystalline solidmassicot, yellow + 3H2OLiquid
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
−154.54–––
per 1 mol of
−51.513–––
per 1 mol of
−154.54–––
per 1 mol of
−154.54–––
per 1 mol of
−154.54–––
per 1 mol of
−51.513–––

Changes in standard condition (4)

Reaction of hydrogen and lead(II) sulfate
3H2Gas + PbSO4Crystalline solid
⟶
SCrystalline solidmonoclinic + PbOCrystalline solidlitharge, red + 3H2OLiquid
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
−156.21–––
per 1 mol of
−52.070–––
per 1 mol of
−156.21–––
per 1 mol of
−156.21–––
per 1 mol of
−156.21–––
per 1 mol of
−52.070–––

Changes in aqueous solution

Reaction of hydrogen and lead(II) sulfate
◆
ΔrG−138.9 kJ/mol
K2.16 × 1024
pK−24.33
3H2Un-ionized aqueous solution + PbSO4Crystalline solid
⟶
SCrystalline solidrhombic + PbOCrystalline solidmassicot, yellow + 3H2OLiquid
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
−142.3−138.9−1569–
per 1 mol of
−47.43−46.30−523.0–
per 1 mol of
−142.3−138.9−1569–
per 1 mol of
−142.3−138.9−1569–
per 1 mol of
−142.3−138.9−1569–
per 1 mol of
−47.43−46.30−523.0–

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
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
PbSO4 (cr)-919.94[1]-813.14[1]148.57[1]103.207[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
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]–––
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
PbO (cr)
massicot, yellow
-217.32[1]-187.89[1]68.70[1]45.77[1]
PbO (cr)
litharge, red
-218.99[1]-188.93[1]66.5[1]45.81[1]
PbO (cr)
1/3 hydrate
–-266.5[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]
* (cr):Crystalline solid, (g):Gas, (l):Liquid

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)