4PbCl2 + 8HNO3 🔥→ 4PbO2 + HClO4 + 4N2O3↑ + 7HCl↑
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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, perchloric acid, dinitrogen trioxide, 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 | 4 | Reducing | Hardly oxidizable |
| HNO3 | Nitric acid | 8 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbO2 | Lead(IV) oxide | 4 | Oxidized | – |
| HClO4 | Perchloric acid | 1 | Oxidized | – |
| N2O3 | Dinitrogen trioxide | 4 | Reduced | – |
| HCl | Hydrogen chloride | 7 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of lead(II) chloride and nitric acid
| 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 | 1369.0 | – | – | – |
per 1 mol of | 342.25 | – | – | – |
per 1 mol of | 171.13 | – | – | – |
per 1 mol of | 342.25 | – | – | – |
per 1 mol of | 1369.0 | – | – | – |
per 1 mol of | 342.25 | – | – | – |
per 1 mol of | 195.57 | – | – | – |
Changes in aqueous solution (1)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 1050.35 kJ/mol K 0.97 × 10−184 pK 184.01
| 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 | 1452.7 | 1050.35 | 1349.1 | – |
per 1 mol of | 363.18 | 262.587 | 337.27 | – |
per 1 mol of | 181.59 | 131.294 | 168.64 | – |
per 1 mol of | 363.18 | 262.587 | 337.27 | – |
per 1 mol of | 1452.7 | 1050.35 | 1349.1 | – |
per 1 mol of | 363.18 | 262.587 | 337.27 | – |
per 1 mol of | 207.53 | 150.050 | 192.73 | – |
Changes in aqueous solution (2)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 798.84 kJ/mol K 0.11 × 10−139 pK 139.95
| 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 | 928.7 | 798.84 | 436.2 | – |
per 1 mol of | 232.2 | 199.71 | 109.0 | – |
per 1 mol of | 116.1 | 99.855 | 54.52 | – |
per 1 mol of | 232.2 | 199.71 | 109.0 | – |
per 1 mol of | 928.7 | 798.84 | 436.2 | – |
per 1 mol of | 232.2 | 199.71 | 109.0 | – |
per 1 mol of | 132.7 | 114.12 | 62.31 | – |
Changes in aqueous solution (3)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 1091.55 kJ/mol K 0.59 × 10−191 pK 191.23
| 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 | – | 1091.55 | – | – |
per 1 mol of | – | 272.887 | – | – |
per 1 mol of | – | 136.444 | – | – |
per 1 mol of | – | 272.887 | – | – |
per 1 mol of | – | 1091.55 | – | – |
per 1 mol of | – | 272.887 | – | – |
per 1 mol of | – | 155.936 | – | – |
Changes in aqueous solution (4)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 840.04 kJ/mol K 0.68 × 10−147 pK 147.17
| 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 | – | 840.04 | – | – |
per 1 mol of | – | 210.01 | – | – |
per 1 mol of | – | 105.00 | – | – |
per 1 mol of | – | 210.01 | – | – |
per 1 mol of | – | 840.04 | – | – |
per 1 mol of | – | 210.01 | – | – |
per 1 mol of | – | 120.01 | – | – |
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] |
| HClO4 (l) | -40.58[1] | – | – | – |
| HClO4 (ai) | -129.33[1] | -8.52[1] | 182.0[1] | – |
| HClO4 (cr) 1 hydrate | -382.21[1] | – | – | – |
| HClO4 (l) 2 hydrate | -677.98[1] | – | – | – |
| N2O3 (l) | 50.29[1] | – | – | – |
| N2O3 (g) | 83.72[1] | 139.46[1] | 312.28[1] | 65.61[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, (l):Liquid, (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°, -40.58 kJ · mol−1
- ^ ΔfH°, -129.33 kJ · mol−1
- ^ ΔfG°, -8.52 kJ · mol−1
- ^ S°, 182.0 J · K−1 · mol−1
- ^ ΔfH°, -382.21 kJ · mol−1
- ^ ΔfH°, -677.98 kJ · mol−1
- ^ ΔfH°, 50.29 kJ · mol−1
- ^ ΔfH°, 83.72 kJ · mol−1
- ^ ΔfG°, 139.46 kJ · mol−1
- ^ S°, 312.28 J · K−1 · mol−1
- ^ Cp°, 65.61 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