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4PbCl2 + 2KMnO4 → 4PbO2 + Cl2↑ + 2MnCl2 + 2KCl

The reaction of lead(II) chloride and potassium permanganate yields lead(IV) oxide, chlorine, 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

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

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
PbCl2Lead(II) chloride4
Reducing
Hardly oxidizable
KMnO4Potassium permanganate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbO2Lead(IV) oxide4
Oxidized
Cl2Chlorine1
Oxidized
MnCl2Manganese(II) chloride2
Reduced
KClPotassium chloride2

Thermodynamic changes

Changes in standard condition

Reaction of lead(II) chloride and potassium permanganate
ΔrG163.0 kJ/mol
K0.28 × 10−28
pK28.56
4PbCl2Crystalline solid + 2KMnO4Crystalline solid
4PbO2Crystalline solid + Cl2Gas + 2MnCl2Crystalline solid + 2KClCrystalline 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
166.4163.011.7
per 1 mol of
41.6040.752.92
83.2081.505.85
per 1 mol of
41.6040.752.92
per 1 mol of
166.4163.011.7
83.2081.505.85
per 1 mol of
83.2081.505.85

Changes in aqueous solution (1)

Reaction of lead(II) chloride and potassium permanganate
ΔrG−71.5 kJ/mol
K3.36 × 1012
pK−12.53
4PbCl2Ionized aqueous solution + 2KMnO4Ionized aqueous solution
4PbO2Crystalline solid + Cl2Gas + 2MnCl2Ionized aqueous solution + 2KClIonized 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
−127.2−71.5−187.7
per 1 mol of
−31.80−17.9−46.92
−63.60−35.8−93.85
per 1 mol of
−31.80−17.9−46.92
per 1 mol of
−127.2−71.5−187.7
−63.60−35.8−93.85
per 1 mol of
−63.60−35.8−93.85

Changes in aqueous solution (2)

Reaction of lead(II) chloride and potassium permanganate
ΔrG−73.9 kJ/mol
K8.85 × 1012
pK−12.95
4PbCl2Ionized aqueous solution + 2KMnO4Ionized aqueous solution
4PbO2Crystalline solid + Cl2Gas + 2MnCl2Un-ionized aqueous solution + 2KClIonized 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
−73.9
per 1 mol of
−18.5
−37.0
per 1 mol of
−18.5
per 1 mol of
−73.9
−37.0
per 1 mol of
−37.0

Changes in aqueous solution (3)

Reaction of lead(II) chloride and potassium permanganate
ΔrG−64.5 kJ/mol
K1.99 × 1011
pK−11.30
4PbCl2Ionized aqueous solution + 2KMnO4Ionized aqueous solution
4PbO2Crystalline solid + Cl2Un-ionized aqueous solution + 2MnCl2Ionized aqueous solution + 2KClIonized 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
−150.6−64.5−290
per 1 mol of
−37.65−16.1−72.5
−75.30−32.3−145
per 1 mol of
−37.65−16.1−72.5
per 1 mol of
−150.6−64.5−290
−75.30−32.3−145
per 1 mol of
−75.30−32.3−145

Changes in aqueous solution (4)

Reaction of lead(II) chloride and potassium permanganate
ΔrG−66.9 kJ/mol
K5.25 × 1011
pK−11.72
4PbCl2Ionized aqueous solution + 2KMnO4Ionized aqueous solution
4PbO2Crystalline solid + Cl2Un-ionized aqueous solution + 2MnCl2Un-ionized aqueous solution + 2KClIonized 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
−66.9
per 1 mol of
−16.7
−33.5
per 1 mol of
−16.7
per 1 mol of
−66.9
−33.5
per 1 mol of
−33.5

Changes in aqueous solution (5)

Reaction of lead(II) chloride and potassium permanganate
ΔrG−30.3 kJ/mol
K2.03 × 105
pK−5.31
4PbCl2Un-ionized aqueous solution + 2KMnO4Ionized aqueous solution
4PbO2Crystalline solid + Cl2Gas + 2MnCl2Ionized aqueous solution + 2KClIonized 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
−30.3
per 1 mol of
−7.58
−15.2
per 1 mol of
−7.58
per 1 mol of
−30.3
−15.2
per 1 mol of
−15.2

Changes in aqueous solution (6)

Reaction of lead(II) chloride and potassium permanganate
ΔrG−32.7 kJ/mol
K5.36 × 105
pK−5.73
4PbCl2Un-ionized aqueous solution + 2KMnO4Ionized aqueous solution
4PbO2Crystalline solid + Cl2Gas + 2MnCl2Un-ionized aqueous solution + 2KClIonized 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
−32.7
per 1 mol of
−8.18
−16.4
per 1 mol of
−8.18
per 1 mol of
−32.7
−16.4
per 1 mol of
−16.4

Changes in aqueous solution (7)

Reaction of lead(II) chloride and potassium permanganate
ΔrG−23.3 kJ/mol
K1.21 × 104
pK−4.08
4PbCl2Un-ionized aqueous solution + 2KMnO4Ionized aqueous solution
4PbO2Crystalline solid + Cl2Un-ionized aqueous solution + 2MnCl2Ionized aqueous solution + 2KClIonized 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
−23.3
per 1 mol of
−5.83
−11.7
per 1 mol of
−5.83
per 1 mol of
−23.3
−11.7
per 1 mol of
−11.7

Changes in aqueous solution (8)

Reaction of lead(II) chloride and potassium permanganate
ΔrG−25.7 kJ/mol
K3.18 × 104
pK−4.50
4PbCl2Un-ionized aqueous solution + 2KMnO4Ionized aqueous solution
4PbO2Crystalline solid + Cl2Un-ionized aqueous solution + 2MnCl2Un-ionized aqueous solution + 2KClIonized 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
−25.7
per 1 mol of
−6.42
−12.8
per 1 mol of
−6.42
per 1 mol of
−25.7
−12.8
per 1 mol of
−12.8

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]
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[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, (g):Gas, (ao):Un-ionized aqueous solution, (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)