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5PbCl2 + 6KMnO4 → 5PbO2 + 2Cl2O↑ + 6MnO2 + 6KCl

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Reaction of lead(II) chloride and potassium permanganate
5PbCl2Lead(II) chloride + 6KMnO4Potassium permanganate
⟶
5PbO2Lead(IV) oxide + 2Cl2O↑Dichlorine monoxide + 6MnO2Manganese(IV) oxide + 6KClPotassium chloride

The reaction of lead(II) chloride and potassium permanganate yields lead(IV) oxide, dichlorine monoxide, manganese(IV) oxide, 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
5PbCl2Lead(II) chloride + 6KMnO4Potassium permanganate
⟶
5PbO2Lead(IV) oxide + 2Cl2O↑Dichlorine monoxide + 6MnO2Manganese(IV) oxide + 6KClPotassium chloride

General equation

Reaction of hardly oxidizable species and oxidizing species
Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of lead(II) chloride and potassium permanganate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
PbCl2Lead(II) chloride5
Reducing
Hardly oxidizable
KMnO4Potassium permanganate6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbO2Lead(IV) oxide5
Oxidized
–
Cl2ODichlorine monoxide2
Oxidized
–
MnO2Manganese(IV) oxide6
Reduced
–
KClPotassium chloride6
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of lead(II) chloride and potassium permanganate
◆
ΔrG−140.4 kJ/mol
K3.95 × 1024
pK−24.60
5PbCl2Crystalline solid + 6KMnO4Crystalline solid
⟶
5PbO2Crystalline solid + 2Cl2O↑Gas + 6MnO2Crystalline solid + 6KClCrystalline solid
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
−146.8−140.4−21.0–
per 1 mol of
−29.36−28.08−4.20–
−24.47−23.40−3.50–
per 1 mol of
−29.36−28.08−4.20–
−73.40−70.20−10.5–
−24.47−23.40−3.50–
per 1 mol of
−24.47−23.40−3.50–

Changes in standard condition (2)

Reaction of lead(II) chloride and potassium permanganate
5PbCl2Crystalline solid + 6KMnO4Crystalline solid
⟶
5PbO2Crystalline solid + 2Cl2O↑Gas + 6MnO2Amorphous solidprecipitated + 6KClCrystalline solid
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
−41.6–––
per 1 mol of
−8.32–––
−6.93–––
per 1 mol of
−8.32–––
−20.8–––
−6.93–––
per 1 mol of
−6.93–––

Changes in aqueous solution (1)

Reaction of lead(II) chloride and potassium permanganate
◆
ΔrG−351.3 kJ/mol
K3.51 × 1061
pK−61.55
5PbCl2Ionized aqueous solution + 6KMnO4Ionized aqueous solution
⟶
5PbO2Crystalline solid + 2Cl2O↑Gas + 6MnO2Crystalline solid + 6KClIonized 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
−421.0−351.3−231.5–
per 1 mol of
−84.20−70.26−46.30–
−70.17−58.55−38.58–
per 1 mol of
−84.20−70.26−46.30–
−210.5−175.7−115.8–
−70.17−58.55−38.58–
per 1 mol of
−70.17−58.55−38.58–

Changes in aqueous solution (2)

Reaction of lead(II) chloride and potassium permanganate
◆
ΔrG−299.8 kJ/mol
K3.33 × 1052
pK−52.52
5PbCl2Un-ionized aqueous solution + 6KMnO4Ionized aqueous solution
⟶
5PbO2Crystalline solid + 2Cl2O↑Gas + 6MnO2Crystalline solid + 6KClIonized 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
–−299.8––
per 1 mol of
–−59.96––
–−49.97––
per 1 mol of
–−59.96––
–−149.9––
–−49.97––
per 1 mol of
–−49.97––

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]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

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]
Cl2O (g)80.3[1]97.9[1]266.21[1]45.40[1]
MnO2 (cr)-520.03[1]-465.14[1]53.05[1]54.14[1]
MnO2 (am)
precipitated
-502.5[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, (g):Gas, (am):Amorphous solid, (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)