You-iggy
  1. Home
  2. Chemical reactions
  3. 9H2 + Pb(CH3COO)2 → Pb + 4H2O + 4CH4

9H2 + Pb(CH3COO)2 → Pb + 4H2O + 4CH4

Last updated:
Reaction of hydrogen and lead(II) acetate
9H2Hydrogen + Pb(CH3COO)2Lead(II) acetate
⟶
PbLead + 4H2OWater + 4CH4Methane

The reaction of hydrogen and lead(II) acetate yields lead, water, 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

Reaction of hydrogen and lead(II) acetate
9H2Hydrogen + Pb(CH3COO)2Lead(II) acetate
⟶
PbLead + 4H2OWater + 4CH4Methane

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of hydrogen and lead(II) acetate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2Hydrogen9
Reducing
Reducing
Pb(CH3COO)2Lead(II) acetate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbLead1
Reduced
–
H2OWater4
Oxidized
–
CH4Methane4
Redoxed product
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen and lead(II) acetate
9H2Gas + Pb(CH3COO)2Crystalline solid
⟶
PbCrystalline solid + 4H2OLiquid + 4CH4Gas
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
−478.73–––
per 1 mol of
−53.192–––
per 1 mol of
−478.73–––
per 1 mol of
−478.73–––
per 1 mol of
−119.68–––
per 1 mol of
−119.68–––

Changes in aqueous solution (1)

Reaction of hydrogen and lead(II) acetate
◆
ΔrG−546.8 kJ/mol
K6.24 × 1095
pK−95.80
9H2Un-ionized aqueous solution + Pb(CH3COO)2Ionized aqueous solution
⟶
PbCrystalline solid + 4H2OLiquid + 4CH4Gas
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
−431.2−546.8−4286–
per 1 mol of
−47.91−60.76−476.2–
per 1 mol of
−431.2−546.8−4286–
per 1 mol of
−431.2−546.8−4286–
per 1 mol of
−107.8−136.7−1072–
per 1 mol of
−107.8−136.7−1072–

Changes in aqueous solution (2)

Reaction of hydrogen and lead(II) acetate
◆
ΔrG−481.2 kJ/mol
K2.01 × 1084
pK−84.30
9H2Un-ionized aqueous solution + Pb(CH3COO)2Ionized aqueous solution
⟶
PbCrystalline solid + 4H2OLiquid + 4CH4Un-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
−488.1−481.2−4697–
per 1 mol of
−54.23−53.47−521.9–
per 1 mol of
−488.1−481.2−4697–
per 1 mol of
−488.1−481.2−4697–
per 1 mol of
−122.0−120.3−1174–
per 1 mol of
−122.0−120.3−1174–

Changes in aqueous solution (3)

Reaction of hydrogen and lead(II) acetate
◆
ΔrG−530.1 kJ/mol
K7.40 × 1092
pK−92.87
9H2Un-ionized aqueous solution + Pb(CH3COO)2Un-ionized aqueous solution
⟶
PbCrystalline solid + 4H2OLiquid + 4CH4Gas
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
–−530.1––
per 1 mol of
–−58.90––
per 1 mol of
–−530.1––
per 1 mol of
–−530.1––
per 1 mol of
–−132.5––
per 1 mol of
–−132.5––

Changes in aqueous solution (4)

Reaction of hydrogen and lead(II) acetate
◆
ΔrG−464.5 kJ/mol
K2.38 × 1081
pK−81.38
9H2Un-ionized aqueous solution + Pb(CH3COO)2Un-ionized aqueous solution
⟶
PbCrystalline solid + 4H2OLiquid + 4CH4Un-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
–−464.5––
per 1 mol of
–−51.61––
per 1 mol of
–−464.5––
per 1 mol of
–−464.5––
per 1 mol of
–−116.1––
per 1 mol of
–−116.1––

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
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[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]–––
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):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
Pb (cr)0[1]0[1]64.81[1]26.44[1]
Pb (g)195.0[1]161.9[1]175.373[1]20.786[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]
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, (l):Liquid, (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)