3PbCl2 + 6HNO3 🔥→ 3PbO2 + 2HClO3 + 6NO↑ + 4HCl↑
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- Reaction of lead(II) chloride and nitric acid
The reaction of lead(II) chloride and nitric acid yields lead(IV) oxide, chloric acid, nitrogen monoxide, and hydrogen chloride (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of lead(II) chloride and nitric acid
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 formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbCl2 | Lead(II) chloride | 3 | Reducing | Hardly oxidizable |
| HNO3 | Nitric acid | 6 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbO2 | Lead(IV) oxide | 3 | Oxidized | – |
| HClO3 | Chloric acid | 2 | Oxidized | – |
| NO | Nitrogen monoxide | 6 | Reduced | – |
| HCl | Hydrogen chloride | 4 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 998.29 kJ/mol K 0.13 × 10−174 pK 174.89
| 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 | 1384.3 | 998.29 | 1294.0 | – |
per 1 mol of | 461.43 | 332.76 | 431.33 | – |
per 1 mol of | 230.72 | 166.38 | 215.67 | – |
per 1 mol of | 461.43 | 332.76 | 431.33 | – |
per 1 mol of | 692.15 | 499.14 | 647.00 | – |
per 1 mol of | 230.72 | 166.38 | 215.67 | – |
per 1 mol of | 346.07 | 249.57 | 323.50 | – |
Changes in standard condition (2)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 854.58 kJ/mol K 0.19 × 10−149 pK 149.72
| 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 | 1084.9 | 854.58 | 772.4 | – |
per 1 mol of | 361.63 | 284.86 | 257.5 | – |
per 1 mol of | 180.82 | 142.43 | 128.7 | – |
per 1 mol of | 361.63 | 284.86 | 257.5 | – |
per 1 mol of | 542.45 | 427.29 | 386.2 | – |
per 1 mol of | 180.82 | 142.43 | 128.7 | – |
per 1 mol of | 271.23 | 213.65 | 193.1 | – |
Changes in standard condition (3)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 1029.19 kJ/mol K 0.49 × 10−180 pK 180.31
| 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 | – | 1029.19 | – | – |
per 1 mol of | – | 343.063 | – | – |
per 1 mol of | – | 171.532 | – | – |
per 1 mol of | – | 343.063 | – | – |
per 1 mol of | – | 514.595 | – | – |
per 1 mol of | – | 171.532 | – | – |
per 1 mol of | – | 257.298 | – | – |
Changes in standard condition (4)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 885.48 kJ/mol K 0.74 × 10−155 pK 155.13
| 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 | – | 885.48 | – | – |
per 1 mol of | – | 295.16 | – | – |
per 1 mol of | – | 147.58 | – | – |
per 1 mol of | – | 295.16 | – | – |
per 1 mol of | – | 442.74 | – | – |
per 1 mol of | – | 147.58 | – | – |
per 1 mol of | – | 221.37 | – | – |
Thermodynamic data of reactants
| Chemical formula | Standard 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 formula | Standard 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] |
| HClO3 (ai) | -103.97[1] | -7.95[1] | 162.3[1] | – |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[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, (ai):Ionized aqueous solution, (g):Gas
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -359.41 kJ · mol−1
- ^ ΔfG°, -314.10 kJ · mol−1
- ^ S°, 136.0 J · K−1 · mol−1
- ^ ΔfH°, -336.0 kJ · mol−1
- ^ ΔfG°, -286.86 kJ · mol−1
- ^ S°, 123.4 J · K−1 · mol−1
- ^ ΔfG°, -297.16 kJ · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1
- ^ ΔfH°, -277.4 kJ · mol−1
- ^ ΔfG°, -217.33 kJ · mol−1
- ^ S°, 68.6 J · K−1 · mol−1
- ^ Cp°, 64.64 J · K−1 · mol−1
- ^ ΔfH°, -103.97 kJ · mol−1
- ^ ΔfG°, -7.95 kJ · mol−1
- ^ S°, 162.3 J · K−1 · mol−1
- ^ ΔfH°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 J · K−1 · mol−1
- ^ ΔfH°, -92.307 kJ · mol−1
- ^ ΔfG°, -95.299 kJ · mol−1
- ^ S°, 186.908 J · K−1 · mol−1
- ^ Cp°, 29.12 J · K−1 · mol−1
- ^ ΔfH°, -167.159 kJ · mol−1
- ^ ΔfG°, -131.228 kJ · mol−1
- ^ S°, 56.5 J · K−1 · mol−1
- ^ Cp°, -136.4 J · K−1 · mol−1