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  3. 2PbI2 + O2 + 2H2O 🔥→ 2PbO2 + 4HI

2PbI2 + O2 + 2H2O 🔥→ 2PbO2 + 4HI

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Reaction of lead(II) iodide and oxygen under neutral condition
2PbI2Lead(II) iodide + O2Oxygen + 2H2OWater
🔥
⟶
2PbO2Lead(IV) oxide + 4HIHydrogen iodide

The reaction of lead(II) iodide, oxygen, and water yields lead(IV) oxide and hydrogen iodide (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 lead(II) iodide and oxygen under neutral condition
2PbI2Lead(II) iodide + O2Oxygen + 2H2OWater
🔥
⟶
2PbO2Lead(IV) oxide + 4HIHydrogen iodide

General equation

Reaction of oxidizable species and oxidizing species under neutral condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of lead(II) iodide and oxygen under neutral condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
PbI2Lead(II) iodide2
Reducing
Oxidizable
O2Oxygen1
Oxidizing
Oxidizing
H2OWater2
–
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbO2Lead(IV) oxide2
Redoxed product
–
HIHydrogen iodide4
–
–

Thermodynamic changes

Changes in standard condition

Reaction of lead(II) iodide and oxygen under neutral condition
◆
ΔrG393.68 kJ/mol
K0.11 × 10−68
pK68.97
2PbI2Crystalline solid + O2Gas + 2H2OLiquid
🔥
⟶
2PbO2Crystalline solid + 4HIGas
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
473.7393.68268.9−88.75
per 1 mol of
236.8196.84134.4−44.38
per 1 mol of
473.7393.68268.9−88.75
per 1 mol of
236.8196.84134.4−44.38
per 1 mol of
236.8196.84134.4−44.38
per 1 mol of
118.498.42067.22−22.19

Changes in aqueous solution (1)

Reaction of lead(II) iodide and oxygen under neutral condition
◆
ΔrG285.1 kJ/mol
K0.11 × 10−49
pK49.95
2PbI2Ionized aqueous solution + O2Un-ionized aqueous solution + 2H2OLiquid
🔥
⟶
2PbO2Crystalline solid + 4HIGas
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
358.7285.1246.9–
per 1 mol of
179.3142.6123.5–
per 1 mol of
358.7285.1246.9–
per 1 mol of
179.3142.6123.5–
per 1 mol of
179.3142.6123.5–
per 1 mol of
89.6771.2861.73–

Changes in aqueous solution (2)

Reaction of lead(II) iodide and oxygen under neutral condition
◆
ΔrG72.1 kJ/mol
K0.23 × 10−12
pK12.63
2PbI2Ionized aqueous solution + O2Un-ionized aqueous solution + 2H2OLiquid
🔥
⟶
2PbO2Crystalline solid + 4HIIonized aqueous solution
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
32.072.1−134.3–
per 1 mol of
16.036.0−67.15–
per 1 mol of
32.072.1−134.3–
per 1 mol of
16.036.0−67.15–
per 1 mol of
16.036.0−67.15–
per 1 mol of
8.0018.0−33.58–

Changes in aqueous solution (3)

Reaction of lead(II) iodide and oxygen under neutral condition
◆
ΔrG317.0 kJ/mol
K0.29 × 10−55
pK55.54
2PbI2Un-ionized aqueous solution + O2Un-ionized aqueous solution + 2H2OLiquid
🔥
⟶
2PbO2Crystalline solid + 4HIGas
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
–317.0––
per 1 mol of
–158.5––
per 1 mol of
–317.0––
per 1 mol of
–158.5––
per 1 mol of
–158.5––
per 1 mol of
–79.25––

Changes in aqueous solution (4)

Reaction of lead(II) iodide and oxygen under neutral condition
◆
ΔrG103.9 kJ/mol
K0.63 × 10−18
pK18.20
2PbI2Un-ionized aqueous solution + O2Un-ionized aqueous solution + 2H2OLiquid
🔥
⟶
2PbO2Crystalline solid + 4HIIonized aqueous solution
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
–103.9––
per 1 mol of
–51.95––
per 1 mol of
–103.9––
per 1 mol of
–51.95––
per 1 mol of
–51.95––
per 1 mol of
–25.98––

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
PbI2 (cr)-175.48[1]-173.64[1]174.85[1]77.36[1]
PbI2 (ai)-112.1[1]-127.57[1]233.0[1]–
PbI2 (ao)–-143.5[1]––
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[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, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas, (l):Liquid

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
PbO2 (cr)-277.4[1]-217.33[1]68.6[1]64.64[1]
HI (g)26.48[1]1.70[1]206.594[1]29.158[1]
HI (ai)-55.19[1]-51.57[1]111.3[1]-142.3[1]
* (cr):Crystalline solid, (g):Gas, (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)