8AgI + 14KMnO4 → 4Ag2O2 + 8KIO3 + 7Mn2O3 + 3K2O
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The reaction of silver(I) iodide and potassium permanganate yields silver(I,III) oxide, potassium iodate, manganese(III) oxide, and potassium 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 silver(I) iodide and potassium permanganate
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 silver(I) iodide and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| AgI | Silver(I) iodide | 8 | Reducing | Oxidizable |
| KMnO4 | Potassium permanganate | 14 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ag2O2 | Silver(I,III) oxide | 4 | Oxidized | – |
| KIO3 | Potassium iodate | 8 | Oxidized | – |
| Mn2O3 | Manganese(III) oxide | 7 | Reduced | – |
| K2O | Potassium oxide | 3 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of silver(I) iodide and potassium permanganate◆
ΔrG 485.5 kJ/mol K 0.88 × 10−85 pK 85.06
| 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 | 309.9 | 485.5 | −592 | 108 |
per 1 mol of | 38.74 | 60.69 | −74.0 | 13.5 |
per 1 mol of | 22.14 | 34.68 | −42.3 | 7.71 |
per 1 mol of | 77.47 | 121.4 | −148 | 27.0 |
per 1 mol of | 38.74 | 60.69 | −74.0 | 13.5 |
per 1 mol of | 44.27 | 69.36 | −84.6 | 15.4 |
per 1 mol of | 103.3 | 161.8 | −197 | 36.0 |
Changes in aqueous solution (1)
- Reaction of silver(I) iodide and potassium permanganate◆
ΔrG −290.4 kJ/mol K 7.51 × 1050 pK −50.88
| 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 | −973.3 | −290.4 | −2294 | – |
per 1 mol of | −121.7 | −36.30 | −286.8 | – |
per 1 mol of | −69.52 | −20.74 | −163.9 | – |
per 1 mol of | −243.3 | −72.60 | −573.5 | – |
per 1 mol of | −121.7 | −36.30 | −286.8 | – |
per 1 mol of | −139.0 | −41.49 | −327.7 | – |
per 1 mol of | −324.4 | −96.80 | −764.7 | – |
Changes in aqueous solution (2)
- Reaction of silver(I) iodide and potassium permanganate◆
ΔrG 10.6 kJ/mol K 0.14 × 10−1 pK 1.86
| 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 | – | 10.6 | – | – |
per 1 mol of | – | 1.32 | – | – |
per 1 mol of | – | 0.757 | – | – |
per 1 mol of | – | 2.65 | – | – |
per 1 mol of | – | 1.32 | – | – |
per 1 mol of | – | 1.51 | – | – |
per 1 mol of | – | 3.53 | – | – |
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 |
|---|---|---|---|---|
| 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] | – | – |
| KMnO4 (cr) | -837.2[1] | -737.6[1] | 171.71[1] | 117.57[1] |
| KMnO4 (ai) | -793.8[1] | -730.5[1] | 293.7[1] | -60.2[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-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 |
|---|---|---|---|---|
| Ag2O2 (cr) | -24.3[1] | 27.6[1] | 117[1] | 88[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] | – |
| Mn2O3 (cr) | -959.0[1] | -881.1[1] | 110.5[1] | 107.65[1] |
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[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°, -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
- ^ ΔfH°, -837.2 kJ · mol−1
- ^ ΔfG°, -737.6 kJ · mol−1
- ^ S°, 171.71 J · K−1 · mol−1
- ^ Cp°, 117.57 J · K−1 · mol−1
- ^ ΔfH°, -793.8 kJ · mol−1
- ^ ΔfG°, -730.5 kJ · mol−1
- ^ S°, 293.7 J · K−1 · mol−1
- ^ Cp°, -60.2 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°, -959.0 kJ · mol−1
- ^ ΔfG°, -881.1 kJ · mol−1
- ^ S°, 110.5 J · K−1 · mol−1
- ^ Cp°, 107.65 J · K−1 · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. 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