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Pb(CH3COO)2 + 6HNO3 → PbO2 + 6NO↑ + 4CO2↑ + 6H2O

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Reaction of lead(II) acetate and nitric acid
Pb(CH3COO)2Lead(II) acetate + 6HNO3Nitric acid
⟶
PbO2Lead(IV) oxide + 6NO↑Nitrogen monoxide + 4CO2↑Carbon dioxide + 6H2OWater

The reaction of lead(II) acetate and nitric acid yields lead(IV) oxide, nitrogen monoxide, carbon dioxide, and water (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) acetate and nitric acid
Pb(CH3COO)2Lead(II) acetate + 6HNO3Nitric acid
⟶
PbO2Lead(IV) oxide + 6NO↑Nitrogen monoxide + 4CO2↑Carbon dioxide + 6H2OWater

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of lead(II) acetate and nitric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Pb(CH3COO)2Lead(II) acetate1
Reducing
Reducing
HNO3Nitric acid6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbO2Lead(IV) oxide1
Oxidized
–
NONitrogen monoxide6
Reduced
–
CO2Carbon dioxide4
Oxidized
–
H2OWater6
–
–

Thermodynamic changes

Changes in standard condition

Reaction of lead(II) acetate and nitric acid
Pb(CH3COO)2Crystalline solid + 6HNO3Liquid
⟶
PbO2Crystalline solid + 6NO↑Gas + 4CO2↑Gas + 6H2OLiquid
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
−1016.5–––
per 1 mol of
−1016.5–––
per 1 mol of
−169.42–––
per 1 mol of
−1016.5–––
per 1 mol of
−169.42–––
per 1 mol of
−254.13–––
per 1 mol of
−169.42–––

Changes in aqueous solution (1)

Reaction of lead(II) acetate and nitric acid
◆
ΔrG−1267.70 kJ/mol
K1.23 × 10222
pK−222.09
Pb(CH3COO)2Ionized aqueous solution + 6HNO3Ionized aqueous solution
⟶
PbO2Crystalline solid + 6NO↑Gas + 4CO2↑Gas + 6H2OLiquid
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
−807.2−1267.701546.4–
per 1 mol of
−807.2−1267.701546.4–
per 1 mol of
−134.5−211.283257.73–
per 1 mol of
−807.2−1267.701546.4–
per 1 mol of
−134.5−211.283257.73–
per 1 mol of
−201.8−316.925386.60–
per 1 mol of
−134.5−211.283257.73–

Changes in aqueous solution (2)

Reaction of lead(II) acetate and nitric acid
◆
ΔrG−1234.18 kJ/mol
K1.66 × 10216
pK−216.22
Pb(CH3COO)2Ionized aqueous solution + 6HNO3Ionized aqueous solution
⟶
PbO2Crystalline solid + 6NO↑Gas + 4CO2↑Un-ionized aqueous solution + 6H2OLiquid
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
−888.3−1234.181161.8–
per 1 mol of
−888.3−1234.181161.8–
per 1 mol of
−148.0−205.697193.63–
per 1 mol of
−888.3−1234.181161.8–
per 1 mol of
−148.0−205.697193.63–
per 1 mol of
−222.1−308.545290.45–
per 1 mol of
−148.0−205.697193.63–

Changes in aqueous solution (3)

Reaction of lead(II) acetate and nitric acid
◆
ΔrG−1251.0 kJ/mol
K1.46 × 10219
pK−219.17
Pb(CH3COO)2Un-ionized aqueous solution + 6HNO3Ionized aqueous solution
⟶
PbO2Crystalline solid + 6NO↑Gas + 4CO2↑Gas + 6H2OLiquid
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
–−1251.0––
per 1 mol of
–−1251.0––
per 1 mol of
–−208.50––
per 1 mol of
–−1251.0––
per 1 mol of
–−208.50––
per 1 mol of
–−312.75––
per 1 mol of
–−208.50––

Changes in aqueous solution (4)

Reaction of lead(II) acetate and nitric acid
◆
ΔrG−1217.5 kJ/mol
K1.98 × 10213
pK−213.30
Pb(CH3COO)2Un-ionized aqueous solution + 6HNO3Ionized aqueous solution
⟶
PbO2Crystalline solid + 6NO↑Gas + 4CO2↑Un-ionized aqueous solution + 6H2OLiquid
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
–−1217.5––
per 1 mol of
–−1217.5––
per 1 mol of
–−202.92––
per 1 mol of
–−1217.5––
per 1 mol of
–−202.92––
per 1 mol of
–−304.38––
per 1 mol of
–−202.92––

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]–––
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[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]
NO (g)90.25[1]86.55[1]210.761[1]29.844[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]–
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, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid

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)