6KMnO4 + 5e− → 3K2O + MnO + 5MnO4−
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- Reduction of potassium permanganate
- 6KMnO4Potassium permanganate + 5e−Electron3K2OPotassium oxide + MnOManganese(II) oxide + 5MnO4−Permanganate ion⟶
Reduction of potassium permanganate yields potassium oxide, manganese(II) oxide, and permanganate ion (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reduction of potassium permanganate
- 6KMnO4Potassium permanganate + 5e−Electron3K2OPotassium oxide + MnOManganese(II) oxide + 5MnO4−Permanganate ion⟶
General equation
- Reduction of reducible species
- ReactantOxidizing agent + e− ⟶ ProductReduction product
Oxidation state of each atom
- Reduction of potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KMnO4 | Potassium permanganate | 6 | Oxidizing | – |
| e− | Electron | 5 | – | Electron |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2O | Potassium oxide | 3 | – | – |
| MnO | Manganese(II) oxide | 1 | Reduced | – |
| MnO4− | Permanganate ion | 5 | – | – |
Thermodynamic changes
Changes in standard condition
- Reduction of potassium permanganate◆
ΔrG 817.8 kJ/mol K 0.53 × 10−143 pK 143.27
| 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 | 586.1 | 817.8 | −464.2 | 247.7 |
per 1 mol of | 97.68 | 136.3 | −77.37 | 41.28 |
per 1 mol of Electron | 117.2 | 163.6 | −92.84 | 49.54 |
per 1 mol of | 195.4 | 272.6 | −154.7 | 82.57 |
per 1 mol of | 586.1 | 817.8 | −464.2 | 247.7 |
per 1 mol of Permanganate ion | 117.2 | 163.6 | −92.84 | 49.54 |
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 |
|---|---|---|---|---|
| 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] |
| e− | – | – | – | – |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[1] | – | – | – |
| MnO (cr) | -385.22[1] | -362.90[1] | 59.71[1] | 45.44[1] |
| MnO (g) | 124.22[1] | – | – | – |
| MnO4− (ao) | -541.4[1] | -447.2[1] | 191.2[1] | -82.0[1] |
* (cr):Crystalline solid, (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°, -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°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · mol−1
- ^ ΔfH°, -385.22 kJ · mol−1
- ^ ΔfG°, -362.90 kJ · mol−1
- ^ S°, 59.71 J · K−1 · mol−1
- ^ Cp°, 45.44 J · K−1 · mol−1
- ^ ΔfH°, 124.22 kJ · mol−1
- ^ ΔfH°, -541.4 kJ · mol−1
- ^ ΔfG°, -447.2 kJ · mol−1
- ^ S°, 191.2 J · K−1 · mol−1
- ^ Cp°, -82.0 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