20KI + 3Zn3(AsO4)2 🔥→ 2KIO3 + 9K2O + 6AsI3 + 9ZnO
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- Reaction of potassium iodide and zinc arsenate
The reaction of potassium iodide and zinc arsenate yields potassium iodate, potassium oxide, , and zinc oxide (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 potassium iodide and zinc arsenate
General equation
- Reaction of oxidizable species and reducible species
- Oxidizable speciesReducing agent + Reducible speciesOxidizing agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of potassium iodide and zinc arsenate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KI | Potassium iodide | 20 | Reducing | Oxidizable |
| Zn3(AsO4)2 | Zinc arsenate | 3 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KIO3 | Potassium iodate | 2 | Oxidized | – |
| K2O | Potassium oxide | 9 | – | – |
| 6 | Reduced | – | ||
| ZnO | Zinc oxide | 9 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium iodide and zinc arsenate◆
ΔrG 5226 kJ/mol K 0.28 × 10−915 pK 915.56 - 20KICrystalline solid + 3Zn3(AsO4)2Crystalline solid2KIO3Crystalline solid + 9K2OCrystalline solid + 6Crystalline solid + 9ZnOCrystalline solid🔥⟶
| 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 | – | 5226 | – | – |
per 1 mol of | – | 261.3 | – | – |
per 1 mol of | – | 1742 | – | – |
per 1 mol of | – | 2613 | – | – |
per 1 mol of | – | 580.7 | – | – |
| – | 871.0 | – | – | |
per 1 mol of | – | 580.7 | – | – |
Changes in aqueous solution
- Reaction of potassium iodide and zinc arsenate◆
ΔrG 5440 kJ/mol K 0.90 × 10−953 pK 953.05 - 20KIIonized aqueous solution + 3Zn3(AsO4)2Crystalline solid2KIO3Ionized aqueous solution + 9K2OCrystalline solid + 6Crystalline solid + 9ZnOCrystalline solid🔥⟶
| 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 | – | 5440 | – | – |
per 1 mol of | – | 272.0 | – | – |
per 1 mol of | – | 1813 | – | – |
per 1 mol of | – | 2720 | – | – |
per 1 mol of | – | 604.4 | – | – |
| – | 906.7 | – | – | |
per 1 mol of | – | 604.4 | – | – |
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 |
|---|---|---|---|---|
| KI (cr) | -327.900[1] | -324.892[1] | 106.32[1] | 52.93[1] |
| KI (g) | -125.5[1] | -166.1[1] | 258.3[1] | 37.11[1] |
| KI (ai) | -307.57[1] | -334.85[1] | 213.8[1] | -120.5[1] |
| Zn3(AsO4)2 (cr) | – | -1895[1] | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution
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 |
|---|---|---|---|---|
| KIO3 (cr) | -501.37[1] | -418.35[1] | 151.46[1] | 106.48[1] |
| KIO3 (ai) | -473.6[1] | -411.2[1] | 220.9[1] | – |
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[1] | – | – | – |
| (cr) | -58.2[1] | -59.4[1] | 213.05[1] | 105.77[1] |
| (g) | – | – | 388.34[1] | 80.63[1] |
| ZnO (cr) | -348.28[1] | -318.30[1] | 43.64[1] | 40.25[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°, -327.900 kJ · mol−1
- ^ ΔfG°, -324.892 kJ · mol−1
- ^ S°, 106.32 J · K−1 · mol−1
- ^ Cp°, 52.93 J · K−1 · mol−1
- ^ ΔfH°, -125.5 kJ · mol−1
- ^ ΔfG°, -166.1 kJ · mol−1
- ^ S°, 258.3 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -307.57 kJ · mol−1
- ^ ΔfG°, -334.85 kJ · mol−1
- ^ S°, 213.8 J · K−1 · mol−1
- ^ Cp°, -120.5 J · K−1 · mol−1
- ^ ΔfG°, -1895. kJ · mol−1
- ^ ΔfH°, -501.37 kJ · mol−1
- ^ ΔfG°, -418.35 kJ · mol−1
- ^ S°, 151.46 J · K−1 · mol−1
- ^ Cp°, 106.48 J · K−1 · mol−1
- ^ ΔfH°, -473.6 kJ · mol−1
- ^ ΔfG°, -411.2 kJ · mol−1
- ^ S°, 220.9 J · K−1 · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · mol−1
- ^ ΔfH°, -58.2 kJ · mol−1
- ^ ΔfG°, -59.4 kJ · mol−1
- ^ S°, 213.05 J · K−1 · mol−1
- ^ Cp°, 105.77 J · K−1 · mol−1
- ^ S°, 388.34 J · K−1 · mol−1
- ^ Cp°, 80.63 J · K−1 · mol−1
- ^ ΔfH°, -348.28 kJ · mol−1
- ^ ΔfG°, -318.30 kJ · mol−1
- ^ S°, 43.64 J · K−1 · mol−1
- ^ Cp°, 40.25 J · K−1 · mol−1
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfG°, -322.1 kJ · mol−1 - p.280
- ^ S°, 94.1 J · K−1 · mol−1 - p.280
- ^ Cp°, 83.7 J · K−1 · mol−1 - p.280