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PbSO4 + 2HNO3 🔥→ PbO2 + 2NO2↑ + H2SO4

The reaction of lead(II) sulfate and nitric acid yields lead(IV) oxide, nitrogen dioxide, and sulfuric acid (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
PbSO4Lead(II) sulfate1
Reducing
Hardly oxidizable
HNO3Nitric acid2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbO2Lead(IV) oxide1
Oxidized
NO2Nitrogen dioxide2
Reduced
H2SO4Sulfuric acid1

Thermodynamic changes

Changes in standard condition

Reaction of lead(II) sulfate and nitric acid
ΔrG169.85 kJ/mol
K0.18 × 10−29
pK29.76
PbSO4Crystalline solid + 2HNO3Liquid
🔥
PbO2Crystalline solid + 2NO2Gas + H2SO4Liquid
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
243.1169.85245.9−45.00
per 1 mol of
243.1169.85245.9−45.00
per 1 mol of
121.584.925123.0−22.50
per 1 mol of
243.1169.85245.9−45.00
per 1 mol of
121.584.925123.0−22.50
per 1 mol of
243.1169.85245.9−45.00

Changes in aqueous solution

Reaction of lead(II) sulfate and nitric acid
ΔrG176.40 kJ/mol
K0.12 × 10−30
pK30.90
PbSO4Crystalline solid + 2HNO3Ionized aqueous solution
🔥
PbO2Crystalline solid + 2NO2Gas + H2SO4Ionized 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
214.4176.40127.5−84
per 1 mol of
214.4176.40127.5−84
per 1 mol of
107.288.20063.75−42
per 1 mol of
214.4176.40127.5−84
per 1 mol of
107.288.20063.75−42
per 1 mol of
214.4176.40127.5−84

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
PbSO4 (cr)-919.94[1]-813.14[1]148.57[1]103.207[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, (l):Liquid, (g):Gas, (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
PbO2 (cr)-277.4[1]-217.33[1]68.6[1]64.64[1]
NO2 (g)33.18[1]51.31[1]240.06[1]37.20[1]
H2SO4 (cr)
H2SO4 (l)-813.989[1]-690.003[1]156.904[1]138.91[1]
H2SO4 (ai)-909.27[1]-744.53[1]20.1[1]-293[1]
H2SO4 (l)
1 hydrate
-1127.621[1]-950.383[1]211.54[1]214.85[1]
H2SO4 (l)
2 hydrate
-1427.100[1]-1199.650[1]276.40[1]260.83[1]
H2SO4 (l)
3 hydrate
-1720.402[1]-1443.980[1]345.39[1]318.95[1]
H2SO4 (l)
4 hydrate
-2011.199[1]-1685.863[1]414.59[1]382.21[1]
H2SO4 (l)
6.5 hydrate
-2733.256[1]-2285.734[1]587.89[1]570.28[1]
* (cr):Crystalline solid, (g):Gas, (l):Liquid, (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)