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  3. 4Pb(CH3COO)2 + 6H2O 💧⚡→ 4PbO2 + 7CH3COOH + 2CH4↑

4Pb(CH3COO)2 + 6H2O 💧⚡→ 4PbO2 + 7CH3COOH + 2CH4↑

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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 + 7CH3COOHAcetic acid + 2CH4↑Methane

Electrolysis of aqueous lead(II) acetate yields lead(IV) oxide, acetic acid, 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 + 7CH3COOHAcetic acid + 2CH4↑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
–
CH3COOHAcetic acid7
Reduced
–
CH4Methane2
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 + 7CH3COOHLiquid + 2CH4↑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
919.6–––
per 1 mol of
229.9–––
per 1 mol of
153.3–––
per 1 mol of
229.9–––
per 1 mol of
131.4–––
per 1 mol of
459.8–––

Changes in aqueous solution (1)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG919.00 kJ/mol
K1.00 × 10−161
pK161.00
4Pb(CH3COO)2Ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CH3COOHIonized aqueous solution + 2CH4↑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
948.1919.00102.5–
per 1 mol of
237.0229.7525.63–
per 1 mol of
158.0153.1717.08–
per 1 mol of
237.0229.7525.63–
per 1 mol of
135.4131.2914.64–
per 1 mol of
474.1459.5051.25–

Changes in aqueous solution (2)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG951.78 kJ/mol
K0.18 × 10−166
pK166.74
4Pb(CH3COO)2Ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CH3COOHIonized aqueous solution + 2CH4↑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
919.6951.78−102.7–
per 1 mol of
229.9237.94−25.68–
per 1 mol of
153.3158.63−17.12–
per 1 mol of
229.9237.94−25.68–
per 1 mol of
131.4135.97−14.67–
per 1 mol of
459.8475.89−51.35–

Changes in aqueous solution (3)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG728.95 kJ/mol
K0.20 × 10−127
pK127.71
4Pb(CH3COO)2Ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CH3COOHUn-ionized aqueous solution + 2CH4↑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
949.8728.95747.2–
per 1 mol of
237.4182.24186.8–
per 1 mol of
158.3121.49124.5–
per 1 mol of
237.4182.24186.8–
per 1 mol of
135.7104.14106.7–
per 1 mol of
474.9364.48373.6–

Changes in aqueous solution (4)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG761.73 kJ/mol
K0.36 × 10−133
pK133.45
4Pb(CH3COO)2Ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CH3COOHUn-ionized aqueous solution + 2CH4↑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
921.4761.73542.0–
per 1 mol of
230.3190.43135.5–
per 1 mol of
153.6126.9590.33–
per 1 mol of
230.3190.43135.5–
per 1 mol of
131.6108.8277.43–
per 1 mol of
460.7380.87271.0–

Changes in aqueous solution (5)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG985.6 kJ/mol
K0.21 × 10−172
pK172.67
4Pb(CH3COO)2Un-ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CH3COOHIonized aqueous solution + 2CH4↑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
–985.6––
per 1 mol of
–246.4––
per 1 mol of
–164.3––
per 1 mol of
–246.4––
per 1 mol of
–140.8––
per 1 mol of
–492.8––

Changes in aqueous solution (6)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG1018.4 kJ/mol
K0.38 × 10−178
pK178.42
4Pb(CH3COO)2Un-ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CH3COOHIonized aqueous solution + 2CH4↑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
–1018.4––
per 1 mol of
–254.60––
per 1 mol of
–169.73––
per 1 mol of
–254.60––
per 1 mol of
–145.49––
per 1 mol of
–509.20––

Changes in aqueous solution (7)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG795.6 kJ/mol
K0.41 × 10−139
pK139.38
4Pb(CH3COO)2Un-ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CH3COOHUn-ionized aqueous solution + 2CH4↑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
–795.6––
per 1 mol of
–198.9––
per 1 mol of
–132.6––
per 1 mol of
–198.9––
per 1 mol of
–113.7––
per 1 mol of
–397.8––

Changes in aqueous solution (8)

Electrolysis of aqueous lead(II) acetate with water as non-redox agent
◆
ΔrG828.4 kJ/mol
K0.74 × 10−145
pK145.13
4Pb(CH3COO)2Un-ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
4PbO2Crystalline solid + 7CH3COOHUn-ionized aqueous solution + 2CH4↑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
–828.4––
per 1 mol of
–207.1––
per 1 mol of
–138.1––
per 1 mol of
–207.1––
per 1 mol of
–118.3––
per 1 mol of
–414.2––

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]
CH3COOH (l)-484.5[1]-389.9[1]159.8[1]124.3[1]
CH3COOH (g)-432.25[1]-374.0[1]282.5[1]66.5[1]
CH3COOH (ai)-486.01[1]-369.31[1]86.6[1]-6.3[1]
CH3COOH (ao)-485.76[1]-396.46[1]178.7[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, (l):Liquid, (g):Gas, (ai):Ionized aqueous solution, (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)