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  3. 23PbCl2 + 14KMnO4 + 2H2O → 23PbO2 + 4HClO3 + 14MnCl2 + 14KCl

23PbCl2 + 14KMnO4 + 2H2O → 23PbO2 + 4HClO3 + 14MnCl2 + 14KCl

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Reaction of lead(II) chloride and potassium permanganate under neutral condition
23PbCl2Lead(II) chloride + 14KMnO4Potassium permanganate + 2H2OWater
⟶
23PbO2Lead(IV) oxide + 4HClO3Chloric acid + 14MnCl2Manganese(II) chloride + 14KClPotassium chloride

The reaction of lead(II) chloride, potassium permanganate, and water yields lead(IV) oxide, chloric acid, manganese(II) chloride, and potassium chloride (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) chloride and potassium permanganate under neutral condition
23PbCl2Lead(II) chloride + 14KMnO4Potassium permanganate + 2H2OWater
⟶
23PbO2Lead(IV) oxide + 4HClO3Chloric acid + 14MnCl2Manganese(II) chloride + 14KClPotassium chloride

General equation

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

Oxidation state of each atom

Reaction of lead(II) chloride and potassium permanganate under neutral condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
PbCl2Lead(II) chloride23
Reducing
Hardly oxidizable
KMnO4Potassium permanganate14
Oxidizing
Oxidizing
H2OWater2
–
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbO2Lead(IV) oxide23
Oxidized
–
HClO3Chloric acid4
Oxidized
–
MnCl2Manganese(II) chloride14
Reduced
–
KClPotassium chloride14
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of lead(II) chloride and potassium permanganate under neutral condition
◆
ΔrG−405.4 kJ/mol
K1.05 × 1071
pK−71.02
23PbCl2Ionized aqueous solution + 14KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
23PbO2Crystalline solid + 4HClO3Ionized aqueous solution + 14MnCl2Ionized aqueous solution + 14KClIonized 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
−1027.3−405.4−2092.2–
per 1 mol of
−44.665−17.63−90.965–
−73.379−28.96−149.44–
per 1 mol of
−513.65−202.7−1046.1–
per 1 mol of
−44.665−17.63−90.965–
per 1 mol of
−256.82−101.3−523.05–
−73.379−28.96−149.44–
per 1 mol of
−73.379−28.96−149.44–

Changes in standard condition (2)

Reaction of lead(II) chloride and potassium permanganate under neutral condition
◆
ΔrG−422.2 kJ/mol
K9.25 × 1073
pK−73.97
23PbCl2Ionized aqueous solution + 14KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
23PbO2Crystalline solid + 4HClO3Ionized aqueous solution + 14MnCl2Un-ionized aqueous solution + 14KClIonized 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
–−422.2––
per 1 mol of
–−18.36––
–−30.16––
per 1 mol of
–−211.1––
per 1 mol of
–−18.36––
per 1 mol of
–−105.5––
–−30.16––
per 1 mol of
–−30.16––

Changes in standard condition (3)

Reaction of lead(II) chloride and potassium permanganate under neutral condition
◆
ΔrG−168.5 kJ/mol
K3.31 × 1029
pK−29.52
23PbCl2Un-ionized aqueous solution + 14KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
23PbO2Crystalline solid + 4HClO3Ionized aqueous solution + 14MnCl2Ionized aqueous solution + 14KClIonized 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
–−168.5––
per 1 mol of
–−7.326––
–−12.04––
per 1 mol of
–−84.25––
per 1 mol of
–−7.326––
per 1 mol of
–−42.13––
–−12.04––
per 1 mol of
–−12.04––

Changes in standard condition (4)

Reaction of lead(II) chloride and potassium permanganate under neutral condition
◆
ΔrG−185.3 kJ/mol
K2.91 × 1032
pK−32.46
23PbCl2Un-ionized aqueous solution + 14KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
23PbO2Crystalline solid + 4HClO3Ionized aqueous solution + 14MnCl2Un-ionized aqueous solution + 14KClIonized 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
–−185.3––
per 1 mol of
–−8.057––
–−13.24––
per 1 mol of
–−92.65––
per 1 mol of
–−8.057––
per 1 mol of
–−46.33––
–−13.24––
per 1 mol of
–−13.24––

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
PbCl2 (cr)-359.41[1]-314.10[1]136.0[1]–
PbCl2 (ai)-336.0[1]-286.86[1]123.4[1]–
PbCl2 (ao)–-297.16[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]
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, (l):Liquid, (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]
HClO3 (ai)-103.97[1]-7.95[1]162.3[1]–
MnCl2 (cr)-481.29[1]-440.50[1]118.24[1]72.93[1]
MnCl2 (g)-263.6[1]–––
MnCl2 (ai)-555.05[1]-490.8[1]38.9[1]-222[1]
MnCl2 (ao)–-492.0[1]––
MnCl2 (cr)
1 hydrate
-789.9[1]-696.1[1]174.1[1]–
MnCl2 (cr)
2 hydrate
-1092.0[1]-942.1[1]218.8[1]–
MnCl2 (cr)
4 hydrate
-1687.4[1]-1423.6[1]303.3[1]–
KCl (cr)-436.747[1]-409.14[1]82.59[1]51.30[1]
KCl (g)-214.14[1]-233.0[1]239.10[1]36.48[1]
KCl (ai)-419.53[1]-414.49[1]159.0[1]-114.6[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-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)