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2Pb + H2SO4 🔥→ 2PbO2 + S + H2

The reaction of lead and sulfuric acid yields lead(IV) oxide, sulfur, and hydrogen (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 reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of lead and sulfuric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
PbLead2
Reducing
Reducing
H2SO4Sulfuric acid1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbO2Lead(IV) oxide2
Oxidized
SSulfur1
Reduced
H2Hydrogen1
Reduced

Thermodynamic changes

Changes in standard condition (1)

Reaction of lead and sulfuric acid
ΔrG255.34 kJ/mol
K0.18 × 10−44
pK44.73
2PbCrystalline solid + H2SO4Liquid
🔥
2PbO2Crystalline solid + SCrystalline solidrhombic + H2Gas
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
259.2255.3413.2−11.05
per 1 mol of
129.6127.676.60−5.525
per 1 mol of
259.2255.3413.2−11.05
per 1 mol of
129.6127.676.60−5.525
per 1 mol of
259.2255.3413.2−11.05
per 1 mol of
259.2255.3413.2−11.05

Changes in standard condition (2)

Reaction of lead and sulfuric acid
2PbCrystalline solid + H2SO4Liquid
🔥
2PbO2Crystalline solid + SCrystalline solidmonoclinic + H2Gas
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
259.5
per 1 mol of
129.8
per 1 mol of
259.5
per 1 mol of
129.8
per 1 mol of
259.5
per 1 mol of
259.5

Changes in aqueous solution (1)

Reaction of lead and sulfuric acid
ΔrG309.87 kJ/mol
K0.52 × 10−54
pK54.29
2PbCrystalline solid + H2SO4Ionized aqueous solution
🔥
2PbO2Crystalline solid + SCrystalline solidrhombic + H2Gas
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
354.5309.87150.0421
per 1 mol of
177.3154.9475.00211
per 1 mol of
354.5309.87150.0421
per 1 mol of
177.3154.9475.00211
per 1 mol of
354.5309.87150.0421
per 1 mol of
354.5309.87150.0421

Changes in aqueous solution (2)

Reaction of lead and sulfuric acid
ΔrG327.5 kJ/mol
K0.42 × 10−57
pK57.38
2PbCrystalline solid + H2SO4Ionized aqueous solution
🔥
2PbO2Crystalline solid + SCrystalline solidrhombic + H2Un-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
350.3327.5596
per 1 mol of
175.2163.8298
per 1 mol of
350.3327.5596
per 1 mol of
175.2163.8298
per 1 mol of
350.3327.5596
per 1 mol of
350.3327.5596

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 (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]
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

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]
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[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)