2PbI2 + 7O2 + 2H2O → 2PbO2 + 4HIO3
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- Reaction of lead(II) iodide and under neutral condition
The reaction of lead(II) iodide, , and water yields lead(IV) oxide and iodic acid (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 under neutral condition
General equation
- Reaction of oxidizable species and oxidizing species under neutral condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of lead(II) iodide and under neutral condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbI2 | Lead(II) iodide | 2 | Reducing | Oxidizable |
| 7 | Oxidizing | Oxidizing | ||
| H2O | Water | 2 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbO2 | Lead(IV) oxide | 2 | Redoxed product | – |
| HIO3 | Iodic acid | 4 | Redoxed product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of lead(II) iodide and under neutral condition
| 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 | −552.6 | – | – | – |
per 1 mol of | −276.3 | – | – | – |
| −78.94 | – | – | – | |
per 1 mol of | −276.3 | – | – | – |
per 1 mol of | −276.3 | – | – | – |
per 1 mol of | −138.2 | – | – | – |
Changes in aqueous solution (1)
- Reaction of lead(II) iodide and under neutral condition◆
ΔrG −350.5 kJ/mol K 2.54 × 1061 pK −61.40
| 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 | −522.2 | −350.5 | −577.3 | – |
per 1 mol of | −261.1 | −175.3 | −288.6 | – |
| −74.60 | −50.07 | −82.47 | – | |
per 1 mol of | −261.1 | −175.3 | −288.6 | – |
per 1 mol of | −261.1 | −175.3 | −288.6 | – |
per 1 mol of | −130.6 | −87.63 | −144.3 | – |
Changes in aqueous solution (2)
- Reaction of lead(II) iodide and under neutral condition◆
ΔrG −318.6 kJ/mol K 6.55 × 1055 pK −55.82
| 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 | – | −318.6 | – | – |
per 1 mol of | – | −159.3 | – | – |
| – | −45.51 | – | – | |
per 1 mol of | – | −159.3 | – | – |
per 1 mol of | – | −159.3 | – | – |
per 1 mol of | – | −79.65 | – | – |
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] | – | – |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas, (l):Liquid
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] |
| HIO3 (cr) | -230.1[1] | – | – | – |
| HIO3 (ao) | -211.3[1] | -132.6[1] | 166.9[1] | – |
* (cr):Crystalline solid, (ao):Un-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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 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°, -230.1 kJ · mol−1
- ^ ΔfH°, -211.3 kJ · mol−1
- ^ ΔfG°, -132.6 kJ · mol−1
- ^ S°, 166.9 J · K−1 · mol−1