3PbCl2 + 2HNO3 🔥→ 3PbO2 + 2Cl2↑ + N2↑ + 2HCl↑
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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, , , 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 | 2 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
PbO2 | Lead(IV) oxide | 3 | Oxidized | – |
2 | Oxidized | – | ||
1 | Reduced | – | ||
HCl | Hydrogen chloride | 2 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 261.13 kJ/mol K 0.18 × 10−45 pK 45.75
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 | 409.6 | 261.13 | 498.2 | – |
per 1 mol of | 136.5 | 87.043 | 166.1 | – |
per 1 mol of | 204.8 | 130.56 | 249.1 | – |
per 1 mol of | 136.5 | 87.043 | 166.1 | – |
204.8 | 130.56 | 249.1 | – | |
409.6 | 261.13 | 498.2 | – | |
per 1 mol of | 204.8 | 130.56 | 249.1 | – |
Changes in aqueous solution (1)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 240.49 kJ/mol K 0.74 × 10−42 pK 42.13
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 | 405.9 | 240.49 | 554.4 | – |
per 1 mol of | 135.3 | 80.163 | 184.8 | – |
per 1 mol of | 202.9 | 120.25 | 277.2 | – |
per 1 mol of | 135.3 | 80.163 | 184.8 | – |
202.9 | 120.25 | 277.2 | – | |
405.9 | 240.49 | 554.4 | – | |
per 1 mol of | 202.9 | 120.25 | 277.2 | – |
Changes in aqueous solution (2)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 168.63 kJ/mol K 0.29 × 10−29 pK 29.54
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 | 256.2 | 168.63 | 293.5 | – |
per 1 mol of | 85.40 | 56.210 | 97.83 | – |
per 1 mol of | 128.1 | 84.315 | 146.8 | – |
per 1 mol of | 85.40 | 56.210 | 97.83 | – |
128.1 | 84.315 | 146.8 | – | |
256.2 | 168.63 | 293.5 | – | |
per 1 mol of | 128.1 | 84.315 | 146.8 | – |
Changes in aqueous solution (3)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 254.37 kJ/mol K 0.27 × 10−44 pK 44.56
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 | 359.1 | 254.37 | 350 | – |
per 1 mol of | 119.7 | 84.790 | 117 | – |
per 1 mol of | 179.6 | 127.19 | 175 | – |
per 1 mol of | 119.7 | 84.790 | 117 | – |
179.6 | 127.19 | 175 | – | |
359.1 | 254.37 | 350 | – | |
per 1 mol of | 179.6 | 127.19 | 175 | – |
Changes in aqueous solution (4)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 182.51 kJ/mol K 0.11 × 10−31 pK 31.97
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 | 209.4 | 182.51 | 89 | – |
per 1 mol of | 69.80 | 60.837 | 30 | – |
per 1 mol of | 104.7 | 91.255 | 45 | – |
per 1 mol of | 69.80 | 60.837 | 30 | – |
104.7 | 91.255 | 45 | – | |
209.4 | 182.51 | 89 | – | |
per 1 mol of | 104.7 | 91.255 | 45 | – |
Changes in aqueous solution (5)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 271.39 kJ/mol K 0.28 × 10−47 pK 47.55
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 | – | – |
– | 135.69 | – | – | |
– | 271.39 | – | – | |
per 1 mol of | – | 135.69 | – | – |
Changes in aqueous solution (6)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 199.53 kJ/mol K 0.11 × 10−34 pK 34.96
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 | – | – |
– | 99.765 | – | – | |
– | 199.53 | – | – | |
per 1 mol of | – | 99.765 | – | – |
Changes in aqueous solution (7)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 285.27 kJ/mol K 0.11 × 10−49 pK 49.98
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 | – | – |
– | 142.63 | – | – | |
– | 285.27 | – | – | |
per 1 mol of | – | 142.63 | – | – |
Changes in aqueous solution (8)
- Reaction of lead(II) chloride and nitric acid◆
ΔrG 213.41 kJ/mol K 0.41 × 10−37 pK 37.39
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 | – | – |
– | 106.70 | – | – | |
– | 213.41 | – | – | |
per 1 mol of | – | 106.70 | – | – |
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] |
(g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
(ao) | -23.4[1] | 6.94[1] | 121[1] | – |
(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
- 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 191.61 J · K−1 · mol−1
- ^ Cp°, 29.125 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