2PbI2 + 2HNO3 🔥→ 2PbO2 + I2 + 2NO↑ + 2HI↑
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- Reaction of lead(II) iodide and nitric acid
The reaction of lead(II) iodide and nitric acid yields lead(IV) oxide, , nitrogen monoxide, and hydrogen iodide (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) iodide and nitric acid
General equation
- Reaction of oxidizable species and oxidizing species
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of lead(II) iodide and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbI2 | Lead(II) iodide | 2 | Reducing | Oxidizable |
| HNO3 | Nitric acid | 2 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbO2 | Lead(IV) oxide | 2 | Oxidized | – |
| 1 | Oxidized | – | ||
| NO | Nitrogen monoxide | 2 | Reduced | – |
| HI | Hydrogen iodide | 2 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of lead(II) iodide and nitric acid◆
ΔrG 250.54 kJ/mol K 0.13 × 10−43 pK 43.89
| 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 | 377.8 | 250.54 | 427.1 | −72.74 |
per 1 mol of | 188.9 | 125.27 | 213.6 | −36.37 |
per 1 mol of | 188.9 | 125.27 | 213.6 | −36.37 |
per 1 mol of | 188.9 | 125.27 | 213.6 | −36.37 |
| 377.8 | 250.54 | 427.1 | −72.74 | |
per 1 mol of | 188.9 | 125.27 | 213.6 | −36.37 |
per 1 mol of | 188.9 | 125.27 | 213.6 | −36.37 |
Changes in aqueous solution (1)
- Reaction of lead(II) iodide and nitric acid◆
ΔrG 235.88 kJ/mol K 0.47 × 10−41 pK 41.32
| 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 | 340.2 | 235.88 | 350.3 | – |
per 1 mol of | 170.1 | 117.94 | 175.2 | – |
per 1 mol of | 170.1 | 117.94 | 175.2 | – |
per 1 mol of | 170.1 | 117.94 | 175.2 | – |
| 340.2 | 235.88 | 350.3 | – | |
per 1 mol of | 170.1 | 117.94 | 175.2 | – |
per 1 mol of | 170.1 | 117.94 | 175.2 | – |
Changes in aqueous solution (2)
- Reaction of lead(II) iodide and nitric acid◆
ΔrG 129.34 kJ/mol K 0.22 × 10−22 pK 22.66
| 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 | 176.8 | 129.34 | 159.7 | – |
per 1 mol of | 88.40 | 64.670 | 79.85 | – |
per 1 mol of | 88.40 | 64.670 | 79.85 | – |
per 1 mol of | 88.40 | 64.670 | 79.85 | – |
| 176.8 | 129.34 | 159.7 | – | |
per 1 mol of | 88.40 | 64.670 | 79.85 | – |
per 1 mol of | 88.40 | 64.670 | 79.85 | – |
Changes in aqueous solution (3)
- Reaction of lead(II) iodide and nitric acid◆
ΔrG 267.7 kJ/mol K 0.13 × 10−46 pK 46.90
| 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 | – | 267.7 | – | – |
per 1 mol of | – | 133.8 | – | – |
per 1 mol of | – | 133.8 | – | – |
per 1 mol of | – | 133.8 | – | – |
| – | 267.7 | – | – | |
per 1 mol of | – | 133.8 | – | – |
per 1 mol of | – | 133.8 | – | – |
Changes in aqueous solution (4)
- Reaction of lead(II) iodide and nitric acid◆
ΔrG 161.2 kJ/mol K 0.57 × 10−28 pK 28.24
| 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 | – | 161.2 | – | – |
per 1 mol of | – | 80.60 | – | – |
per 1 mol of | – | 80.60 | – | – |
per 1 mol of | – | 80.60 | – | – |
| – | 161.2 | – | – | |
per 1 mol of | – | 80.60 | – | – |
per 1 mol of | – | 80.60 | – | – |
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 |
|---|---|---|---|---|
| PbI2 (cr) | -175.48[1] | -173.64[1] | 174.85[1] | 77.36[1] |
| PbI2 (ai) | -112.1[1] | -127.57[1] | 233.0[1] | – |
| PbI2 (ao) | – | -143.5[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] |
| (cr) | 0[1] | 0[1] | 116.135[1] | 54.438[1] |
| (g) | 62.438[1] | 19.327[1] | 260.69[1] | 36.90[1] |
| (ao) | 22.6[1] | 16.40[1] | 137.2[1] | – |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| HI (g) | 26.48[1] | 1.70[1] | 206.594[1] | 29.158[1] |
| HI (ai) | -55.19[1] | -51.57[1] | 111.3[1] | -142.3[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°, -175.48 kJ · mol−1
- ^ ΔfG°, -173.64 kJ · mol−1
- ^ S°, 174.85 J · K−1 · mol−1
- ^ Cp°, 77.36 J · K−1 · mol−1
- ^ ΔfH°, -112.1 kJ · mol−1
- ^ ΔfG°, -127.57 kJ · mol−1
- ^ S°, 233.0 J · K−1 · mol−1
- ^ ΔfG°, -143.5 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°, 116.135 J · K−1 · mol−1
- ^ Cp°, 54.438 J · K−1 · mol−1
- ^ ΔfH°, 62.438 kJ · mol−1
- ^ ΔfG°, 19.327 kJ · mol−1
- ^ S°, 260.69 J · K−1 · mol−1
- ^ Cp°, 36.90 J · K−1 · mol−1
- ^ ΔfH°, 22.6 kJ · mol−1
- ^ ΔfG°, 16.40 kJ · mol−1
- ^ S°, 137.2 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°, 26.48 kJ · mol−1
- ^ ΔfG°, 1.70 kJ · mol−1
- ^ S°, 206.594 J · K−1 · mol−1
- ^ Cp°, 29.158 J · K−1 · mol−1
- ^ ΔfH°, -55.19 kJ · mol−1
- ^ ΔfG°, -51.57 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ Cp°, -142.3 J · K−1 · mol−1