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  3. 3PbCl2 + 2HNO3 🔥→ 3PbO2 + 2Cl2↑ + N2↑ + 2HCl↑

3PbCl2 + 2HNO3 🔥→ 3PbO2 + 2Cl2↑ + N2↑ + 2HCl↑

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Reaction of lead(II) chloride and nitric acid
3PbCl2Lead(II) chloride + 2HNO3Nitric acid
🔥
⟶
3PbO2Lead(IV) oxide + 2Cl2↑Chlorine + N2↑Nitrogen + 2HCl↑Hydrogen chloride

The reaction of lead(II) chloride and nitric acid yields lead(IV) oxide, chlorine, nitrogen, and hydrogen chloride (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) chloride and nitric acid
3PbCl2Lead(II) chloride + 2HNO3Nitric acid
🔥
⟶
3PbO2Lead(IV) oxide + 2Cl2↑Chlorine + N2↑Nitrogen + 2HCl↑Hydrogen chloride

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

Reaction of lead(II) chloride and nitric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
PbCl2Lead(II) chloride3
Reducing
Hardly oxidizable
HNO3Nitric acid2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbO2Lead(IV) oxide3
Oxidized
–
Cl2Chlorine2
Oxidized
–
N2Nitrogen1
Reduced
–
HClHydrogen chloride2
–
–

Thermodynamic changes

Changes in standard condition

Reaction of lead(II) chloride and nitric acid
◆
ΔrG261.13 kJ/mol
K0.18 × 10−45
pK45.75
3PbCl2Crystalline solid + 2HNO3Liquid
🔥
⟶
3PbO2Crystalline solid + 2Cl2↑Gas + N2↑Gas + 2HCl↑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
409.6261.13498.2–
per 1 mol of
136.587.043166.1–
per 1 mol of
204.8130.56249.1–
per 1 mol of
136.587.043166.1–
per 1 mol of
204.8130.56249.1–
per 1 mol of
409.6261.13498.2–
per 1 mol of
204.8130.56249.1–

Changes in aqueous solution (1)

Reaction of lead(II) chloride and nitric acid
◆
ΔrG240.49 kJ/mol
K0.74 × 10−42
pK42.13
3PbCl2Ionized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3PbO2Crystalline solid + 2Cl2↑Gas + N2↑Gas + 2HCl↑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
405.9240.49554.4–
per 1 mol of
135.380.163184.8–
per 1 mol of
202.9120.25277.2–
per 1 mol of
135.380.163184.8–
per 1 mol of
202.9120.25277.2–
per 1 mol of
405.9240.49554.4–
per 1 mol of
202.9120.25277.2–

Changes in aqueous solution (2)

Reaction of lead(II) chloride and nitric acid
◆
ΔrG168.63 kJ/mol
K0.29 × 10−29
pK29.54
3PbCl2Ionized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3PbO2Crystalline solid + 2Cl2↑Gas + N2↑Gas + 2HCl↑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
256.2168.63293.5–
per 1 mol of
85.4056.21097.83–
per 1 mol of
128.184.315146.8–
per 1 mol of
85.4056.21097.83–
per 1 mol of
128.184.315146.8–
per 1 mol of
256.2168.63293.5–
per 1 mol of
128.184.315146.8–

Changes in aqueous solution (3)

Reaction of lead(II) chloride and nitric acid
◆
ΔrG254.37 kJ/mol
K0.27 × 10−44
pK44.56
3PbCl2Ionized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3PbO2Crystalline solid + 2Cl2↑Un-ionized aqueous solution + N2↑Gas + 2HCl↑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
359.1254.37350–
per 1 mol of
119.784.790117–
per 1 mol of
179.6127.19175–
per 1 mol of
119.784.790117–
per 1 mol of
179.6127.19175–
per 1 mol of
359.1254.37350–
per 1 mol of
179.6127.19175–

Changes in aqueous solution (4)

Reaction of lead(II) chloride and nitric acid
◆
ΔrG182.51 kJ/mol
K0.11 × 10−31
pK31.97
3PbCl2Ionized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3PbO2Crystalline solid + 2Cl2↑Un-ionized aqueous solution + N2↑Gas + 2HCl↑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
209.4182.5189–
per 1 mol of
69.8060.83730–
per 1 mol of
104.791.25545–
per 1 mol of
69.8060.83730–
per 1 mol of
104.791.25545–
per 1 mol of
209.4182.5189–
per 1 mol of
104.791.25545–

Changes in aqueous solution (5)

Reaction of lead(II) chloride and nitric acid
◆
ΔrG271.39 kJ/mol
K0.28 × 10−47
pK47.55
3PbCl2Un-ionized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3PbO2Crystalline solid + 2Cl2↑Gas + N2↑Gas + 2HCl↑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
–271.39––
per 1 mol of
–90.463––
per 1 mol of
–135.69––
per 1 mol of
–90.463––
per 1 mol of
–135.69––
per 1 mol of
–271.39––
per 1 mol of
–135.69––

Changes in aqueous solution (6)

Reaction of lead(II) chloride and nitric acid
◆
ΔrG199.53 kJ/mol
K0.11 × 10−34
pK34.96
3PbCl2Un-ionized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3PbO2Crystalline solid + 2Cl2↑Gas + N2↑Gas + 2HCl↑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
–199.53––
per 1 mol of
–66.510––
per 1 mol of
–99.765––
per 1 mol of
–66.510––
per 1 mol of
–99.765––
per 1 mol of
–199.53––
per 1 mol of
–99.765––

Changes in aqueous solution (7)

Reaction of lead(II) chloride and nitric acid
◆
ΔrG285.27 kJ/mol
K0.11 × 10−49
pK49.98
3PbCl2Un-ionized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3PbO2Crystalline solid + 2Cl2↑Un-ionized aqueous solution + N2↑Gas + 2HCl↑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
–285.27––
per 1 mol of
–95.090––
per 1 mol of
–142.63––
per 1 mol of
–95.090––
per 1 mol of
–142.63––
per 1 mol of
–285.27––
per 1 mol of
–142.63––

Changes in aqueous solution (8)

Reaction of lead(II) chloride and nitric acid
◆
ΔrG213.41 kJ/mol
K0.41 × 10−37
pK37.39
3PbCl2Un-ionized aqueous solution + 2HNO3Ionized aqueous solution
🔥
⟶
3PbO2Crystalline solid + 2Cl2↑Un-ionized aqueous solution + N2↑Gas + 2HCl↑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
–213.41––
per 1 mol of
–71.137––
per 1 mol of
–106.70––
per 1 mol of
–71.137––
per 1 mol of
–106.70––
per 1 mol of
–213.41––
per 1 mol of
–106.70––

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
PbCl2 (cr)-359.41[1]-314.10[1]136.0[1]–
PbCl2 (ai)-336.0[1]-286.86[1]123.4[1]–
PbCl2 (ao)–-297.16[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]
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]–
N2 (g)0[1]0[1]191.61[1]29.125[1]
HCl (g)-92.307[1]-95.299[1]186.908[1]29.12[1]
HCl (ai)-167.159[1]-131.228[1]56.5[1]-136.4[1]
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (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)