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  3. 11PbI2 + 14KMnO4 + 28H^+ → 11PbO2 + 8HIO3 + 14Mn^2+ + 14KI + 10H2O

11PbI2 + 14KMnO4 + 28H+ → 11PbO2 + 8HIO3 + 14Mn2+ + 14KI + 10H2O

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Reaction of lead(II) iodide and potassium permanganate under acidic condition
11PbI2Lead(II) iodide + 14KMnO4Potassium permanganate + 28H+Hydrogen ion
⟶
11PbO2Lead(IV) oxide + 8HIO3Iodic acid + 14Mn2+Manganese(II) ion + 14KIPotassium iodide + 10H2OWater

The reaction of lead(II) iodide, potassium permanganate, and hydrogen ion yields lead(IV) oxide, iodic acid, manganese(II) ion, potassium iodide, 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 lead(II) iodide and potassium permanganate under acidic condition
11PbI2Lead(II) iodide + 14KMnO4Potassium permanganate + 28H+Hydrogen ion
⟶
11PbO2Lead(IV) oxide + 8HIO3Iodic acid + 14Mn2+Manganese(II) ion + 14KIPotassium iodide + 10H2OWater

General equation

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

Oxidation state of each atom

Reaction of lead(II) iodide and potassium permanganate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
PbI2Lead(II) iodide11
Reducing
Oxidizable
KMnO4Potassium permanganate14
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion28
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbO2Lead(IV) oxide11
Oxidized
–
HIO3Iodic acid8
Oxidized
–
Mn2+Manganese(II) ion14
Reduced
–
KIPotassium iodide14
–
–
H2OWater10
–
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of lead(II) iodide and potassium permanganate under acidic condition
◆
ΔrG−2073.8 kJ/mol
K2.06 × 10363
pK−363.31
11PbI2Ionized aqueous solution + 14KMnO4Ionized aqueous solution + 28H+Un-ionized aqueous solution
⟶
11PbO2Crystalline solid + 8HIO3Un-ionized aqueous solution + 14Mn2+Un-ionized aqueous solution + 14KIIonized 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
−2650.3−2073.8−1923.1–
per 1 mol of
−240.94−188.53−174.83–
−189.31−148.13−137.36–
per 1 mol of
Hydrogen ion
−94.654−74.064−68.682–
per 1 mol of
−240.94−188.53−174.83–
per 1 mol of
−331.29−259.23−240.39–
per 1 mol of
Manganese(II) ion
−189.31−148.13−137.36–
per 1 mol of
−189.31−148.13−137.36–
per 1 mol of
−265.03−207.38−192.31–

Changes in standard condition (2)

Reaction of lead(II) iodide and potassium permanganate under acidic condition
◆
ΔrG−1898.5 kJ/mol
K4.01 × 10332
pK−332.60
11PbI2Un-ionized aqueous solution + 14KMnO4Ionized aqueous solution + 28H+Un-ionized aqueous solution
⟶
11PbO2Crystalline solid + 8HIO3Un-ionized aqueous solution + 14Mn2+Un-ionized aqueous solution + 14KIIonized 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
–−1898.5––
per 1 mol of
–−172.59––
–−135.61––
per 1 mol of
Hydrogen ion
–−67.804––
per 1 mol of
–−172.59––
per 1 mol of
–−237.31––
per 1 mol of
Manganese(II) ion
–−135.61––
per 1 mol of
–−135.61––
per 1 mol of
–−189.85––

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]––
KMnO4 (cr)-837.2[1]-737.6[1]171.71[1]117.57[1]
KMnO4 (ai)-793.8[1]-730.5[1]293.7[1]-60.2[1]
H+ (g)1536.202[1]–––
H+ (ao)0[1]0[1]0[1]0[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas

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]
HIO3 (cr)-230.1[1]–––
HIO3 (ao)-211.3[1]-132.6[1]166.9[1]–
Mn2+ (g)2519.69[1]–––
Mn2+ (ao)-220.75[1]-228.1[1]-73.6[1]50[1]
KI (cr)-327.900[1]-324.892[1]106.32[1]52.93[1]
KI (g)-125.5[1]-166.1[1]258.3[1]37.11[1]
KI (ai)-307.57[1]-334.85[1]213.8[1]-120.5[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, (ao):Un-ionized aqueous solution, (g):Gas, (ai):Ionized aqueous solution, (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)