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H2S + 5Pb(OH)2 🔥→ PbSO4 + 4Pb + 6H2O

The reaction of hydrogen sulfide and lead(II) hydroxide yields lead(II) sulfate, 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

General equation

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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide1
Reducing
Reducing
Pb(OH)2Lead(II) hydroxide5
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbSO4Lead(II) sulfate1
Oxidized
PbLead4
Reduced
H2OWater6

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and lead(II) hydroxide
ΔrG58.6 kJ/mol
K0.54 × 10−10
pK10.27
H2SGas + 5Pb(OH)2Crystalline solid
🔥
PbSO4Crystalline solid + 4PbCrystalline solid + 6H2OLiquid
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
58.6
per 1 mol of
58.6
per 1 mol of
11.7
per 1 mol of
58.6
per 1 mol of
14.7
per 1 mol of
9.77

Changes in standard condition (2)

Reaction of hydrogen sulfide and lead(II) hydroxide
H2SGas + 5Pb(OH)2Crystalline solidprecipitated
🔥
PbSO4Crystalline solid + 4PbCrystalline solid + 6H2OLiquid
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
−34.8
per 1 mol of
−34.8
per 1 mol of
−6.96
per 1 mol of
−34.8
per 1 mol of
−8.70
per 1 mol of
−5.80

Changes in aqueous solution

Reaction of hydrogen sulfide and lead(II) hydroxide
ΔrG52.9 kJ/mol
K0.54 × 10−9
pK9.27
H2SUn-ionized aqueous solution + 5Pb(OH)2Crystalline solid
🔥
PbSO4Crystalline solid + 4PbCrystalline solid + 6H2OLiquid
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
52.9
per 1 mol of
52.9
per 1 mol of
10.6
per 1 mol of
52.9
per 1 mol of
13.2
per 1 mol of
8.82

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]
Pb(OH)2 (cr)-452.2[1]
Pb(OH)2 (cr)
precipitated
-515.9[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
PbSO4 (cr)-919.94[1]-813.14[1]148.57[1]103.207[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]
* (cr):Crystalline solid, (g):Gas, (l):Liquid

References

List of references

  1. 1