7KI + 3Ag2O2 🔥→ KIO3 + 3K2O + 6AgI
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The reaction of potassium iodide and silver(I,III) oxide yields potassium iodate, potassium oxide, and silver(I) 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 potassium iodide and silver(I,III) oxide
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 potassium iodide and silver(I,III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KI | Potassium iodide | 7 | Reducing | Oxidizable |
| Ag2O2 | Silver(I,III) oxide | 3 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KIO3 | Potassium iodate | 1 | Oxidized | – |
| K2O | Potassium oxide | 3 | – | – |
| AgI | Silver(I) iodide | 6 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium iodide and silver(I,III) oxide◆
ΔrG 409.7 kJ/mol K 0.17 × 10−71 pK 71.78
| 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 | 411.3 | 409.7 | 32 | 64 |
per 1 mol of | 58.76 | 58.53 | 4.6 | 9.1 |
per 1 mol of | 137.1 | 136.6 | 11 | 21 |
per 1 mol of | 411.3 | 409.7 | 32 | 64 |
per 1 mol of | 137.1 | 136.6 | 11 | 21 |
per 1 mol of | 68.55 | 68.28 | 5.3 | 11 |
Changes in aqueous solution (1)
- Reaction of potassium iodide and silver(I,III) oxide◆
ΔrG 1036.8 kJ/mol K 0.23 × 10−181 pK 181.64
| 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 | 970.1 | 1036.8 | −240 | – |
per 1 mol of | 138.6 | 148.11 | −34.3 | – |
per 1 mol of | 323.4 | 345.60 | −80.0 | – |
per 1 mol of | 970.1 | 1036.8 | −240 | – |
per 1 mol of | 323.4 | 345.60 | −80.0 | – |
per 1 mol of | 161.7 | 172.80 | −40.0 | – |
Changes in aqueous solution (2)
- Reaction of potassium iodide and silver(I,III) oxide◆
ΔrG 811.1 kJ/mol K 0.80 × 10−142 pK 142.10
| 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 | – | 811.1 | – | – |
per 1 mol of | – | 115.9 | – | – |
per 1 mol of | – | 270.4 | – | – |
per 1 mol of | – | 811.1 | – | – |
per 1 mol of | – | 270.4 | – | – |
per 1 mol of | – | 135.2 | – | – |
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] |
| Ag2O2 (cr) | -24.3[1] | 27.6[1] | 117[1] | 88[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] | – | – | – |
| AgI (cr) | -61.84[1] | -66.19[1] | 115.5[1] | 56.82[1] |
| AgI (ai) | 50.38[1] | 25.52[1] | 184.1[1] | -120.5[1] |
| AgI (ao) | – | -12.1[1] | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (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°, -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
- ^ ΔfH°, -24.3 kJ · mol−1
- ^ ΔfG°, 27.6 kJ · mol−1
- ^ S°, 117. J · K−1 · mol−1
- ^ Cp°, 88. J · K−1 · 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°, -61.84 kJ · mol−1
- ^ ΔfG°, -66.19 kJ · mol−1
- ^ S°, 115.5 J · K−1 · mol−1
- ^ Cp°, 56.82 J · K−1 · mol−1
- ^ ΔfH°, 50.38 kJ · mol−1
- ^ ΔfG°, 25.52 kJ · mol−1
- ^ S°, 184.1 J · K−1 · mol−1
- ^ Cp°, -120.5 J · K−1 · mol−1
- ^ ΔfG°, -12.1 kJ · 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