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4Pb(CH3COO)2 + 6H2O 💧⚡→ 4PbO2 + 7CO2↑ + 9CH4↑

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Electrolysis of aqueous lead(II) acetate with water as non-redox agent
4Pb(CH3COO)2Lead(II) acetate + 6H2OWater
💧⚡
⟶
4PbO2Lead(IV) oxide + 7CO2↑Carbon dioxide + 9CH4↑Methane

Electrolysis of aqueous lead(II) acetate yields lead(IV) oxide, carbon dioxide, and methane (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

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
4Pb(CH3COO)2Lead(II) acetate + 6H2OWater
💧⚡
⟶
4PbO2Lead(IV) oxide + 7CO2↑Carbon dioxide + 9CH4↑Methane

General equation

Electrolysis of aqueous solution with water as non redox agent
Miscible with water/Very soluble in water/Soluble in waterSelf redox agent + H2ONon-redox agent
💧⚡
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Electrolysis of aqueous lead(II) acetate with water as non-redox agent

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Pb(CH3COO)2Lead(II) acetate4
Self redox agent
Very soluble in water
H2OWater6
–
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbO2Lead(IV) oxide4
Oxidized
–
CO2Carbon dioxide7
Oxidized
–
CH4Methane9
Reduced
–

Thermodynamic changes

Changes in standard condition

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
4Pb(CH3COO)2Crystalline solid + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CO2↑Gas + 9CH4↑Gas
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
1032.8–––
per 1 mol of
258.20–––
per 1 mol of
172.13–––
per 1 mol of
258.20–––
per 1 mol of
147.54–––
per 1 mol of
114.76–––

Changes in aqueous solution (1)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG388.62 kJ/mol
K0.83 × 10−68
pK68.08
4Pb(CH3COO)2Ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CO2↑Gas + 9CH4↑Gas
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
1071.9388.622296.3–
per 1 mol of
267.9897.155574.08–
per 1 mol of
178.6564.770382.72–
per 1 mol of
267.9897.155574.08–
per 1 mol of
153.1355.517328.04–
per 1 mol of
119.1043.180255.14–

Changes in aqueous solution (2)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG536.13 kJ/mol
K0.12 × 10−93
pK93.93
4Pb(CH3COO)2Ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CO2↑Gas + 9CH4↑Un-ionized 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
943.9536.131373.2–
per 1 mol of
236.0134.03343.30–
per 1 mol of
157.389.355228.87–
per 1 mol of
236.0134.03343.30–
per 1 mol of
134.876.590196.17–
per 1 mol of
104.959.570152.58–

Changes in aqueous solution (3)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG447.27 kJ/mol
K0.44 × 10−78
pK78.36
4Pb(CH3COO)2Ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CO2↑Un-ionized aqueous solution + 9CH4↑Gas
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
929.9447.271623.3–
per 1 mol of
232.5111.82405.82–
per 1 mol of
155.074.545270.55–
per 1 mol of
232.5111.82405.82–
per 1 mol of
132.863.896231.90–
per 1 mol of
103.349.697180.37–

Changes in aqueous solution (4)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG594.78 kJ/mol
K0.63 × 10−104
pK104.20
4Pb(CH3COO)2Ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CO2↑Un-ionized aqueous solution + 9CH4↑Un-ionized 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
801.8594.78700.2–
per 1 mol of
200.4148.69175.1–
per 1 mol of
133.699.130116.7–
per 1 mol of
200.4148.69175.1–
per 1 mol of
114.584.969100.0–
per 1 mol of
89.0966.08777.80–

Changes in aqueous solution (5)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG455.3 kJ/mol
K0.17 × 10−79
pK79.77
4Pb(CH3COO)2Un-ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CO2↑Gas + 9CH4↑Gas
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
–455.3––
per 1 mol of
–113.8––
per 1 mol of
–75.88––
per 1 mol of
–113.8––
per 1 mol of
–65.04––
per 1 mol of
–50.59––

Changes in aqueous solution (6)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG602.8 kJ/mol
K0.25 × 10−105
pK105.61
4Pb(CH3COO)2Un-ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CO2↑Gas + 9CH4↑Un-ionized 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
–602.8––
per 1 mol of
–150.7––
per 1 mol of
–100.5––
per 1 mol of
–150.7––
per 1 mol of
–86.11––
per 1 mol of
–66.98––

Changes in aqueous solution (7)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG513.9 kJ/mol
K0.93 × 10−90
pK90.03
4Pb(CH3COO)2Un-ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CO2↑Un-ionized aqueous solution + 9CH4↑Gas
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
–513.9––
per 1 mol of
–128.5––
per 1 mol of
–85.65––
per 1 mol of
–128.5––
per 1 mol of
–73.41––
per 1 mol of
–57.10––

Changes in aqueous solution (8)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG661.4 kJ/mol
K0.13 × 10−115
pK115.87
4Pb(CH3COO)2Un-ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CO2↑Un-ionized aqueous solution + 9CH4↑Un-ionized 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
–661.4––
per 1 mol of
–165.3––
per 1 mol of
–110.2––
per 1 mol of
–165.3––
per 1 mol of
–94.49––
per 1 mol of
–73.49––

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
Pb(CH3COO)2 (cr)-963.83[1]–––
Pb(CH3COO)2 (ai)-973.6[1]-763.04[1]182.8[1]–
Pb(CH3COO)2 (ao)–-779.7[1]––
Pb(CH3COO)2 (cr)
3 hydrate
-1851.50[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]
CO2 (g)-393.509[1]-394.359[1]213.74[1]37.11[1]
CO2 (ao)-413.80[1]-385.98[1]117.6[1]–
CH4 (g)-74.81[1]-50.72[1]186.264[1]35.309[1]
CH4 (ao)-89.04[1]-34.33[1]83.7[1]–
* (cr):Crystalline solid, (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)