9Fe(OH)2 + 2KMnO4 → 3Fe3O4 + 2MnO2 + K2O + 9H2O
Last updated:
The reaction of iron(II) hydroxide and potassium permanganate yields iron(II,III) oxide, manganese(IV) oxide, potassium oxide, and water (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 iron(II) hydroxide 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 iron(II) hydroxide and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe(OH)2 | Iron(II) hydroxide | 9 | Reducing | Oxidizable |
| KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe3O4 | Iron(II,III) oxide | 3 | Oxidized | – |
| MnO2 | Manganese(IV) oxide | 2 | Reduced | – |
| K2O | Potassium oxide | 1 | – | – |
| H2O | Water | 9 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(II) hydroxide and potassium permanganate◆
ΔrG −579.0 kJ/mol K 2.73 × 10101 pK −101.44
| 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 | −533.8 | −579.0 | 133 | – |
per 1 mol of | −59.31 | −64.33 | 14.8 | – |
per 1 mol of | −266.9 | −289.5 | 66.5 | – |
per 1 mol of | −177.9 | −193.0 | 44.3 | – |
per 1 mol of | −266.9 | −289.5 | 66.5 | – |
per 1 mol of | −533.8 | −579.0 | 133 | – |
per 1 mol of | −59.31 | −64.33 | 14.8 | – |
Changes in standard condition (2)
- Reaction of iron(II) hydroxide and potassium permanganate
| 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 | −498.8 | – | – | – |
per 1 mol of | −55.42 | – | – | – |
per 1 mol of | −249.4 | – | – | – |
per 1 mol of | −166.3 | – | – | – |
per 1 mol of | −249.4 | – | – | – |
per 1 mol of | −498.8 | – | – | – |
per 1 mol of | −55.42 | – | – | – |
Changes in aqueous solution
- Reaction of iron(II) hydroxide and potassium permanganate◆
ΔrG −593.2 kJ/mol K 8.40 × 10103 pK −103.92
| 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 | −620.6 | −593.2 | −111 | – |
per 1 mol of | −68.96 | −65.91 | −12.3 | – |
per 1 mol of | −310.3 | −296.6 | −55.5 | – |
per 1 mol of | −206.9 | −197.7 | −37.0 | – |
per 1 mol of | −310.3 | −296.6 | −55.5 | – |
per 1 mol of | −620.6 | −593.2 | −111 | – |
per 1 mol of | −68.96 | −65.91 | −12.3 | – |
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 |
|---|---|---|---|---|
| Fe(OH)2 (cr) precipitated | -569.0[1] | -486.5[1] | 88[1] | – |
| Fe(OH)2 (g) | -372[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, (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 |
|---|---|---|---|---|
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
| MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
| MnO2 (am) precipitated | -502.5[1] | – | – | – |
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[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, (am):Amorphous solid, (g):Gas, (l):Liquid
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°, -569.0 kJ · mol−1
- ^ ΔfG°, -486.5 kJ · mol−1
- ^ S°, 88. J · K−1 · mol−1
- ^ ΔfH°, -372. 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°, -1118.4 kJ · mol−1
- ^ ΔfG°, -1015.4 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, 143.43 J · K−1 · mol−1
- ^ ΔfH°, -520.03 kJ · mol−1
- ^ ΔfG°, -465.14 kJ · mol−1
- ^ S°, 53.05 J · K−1 · mol−1
- ^ Cp°, 54.14 J · K−1 · mol−1
- ^ ΔfH°, -502.5 kJ · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · 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
- 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