15K4[Fe(CN)6] + 128KMnO4 → 90K2CO3 + 4K2O + 5Fe3O4 + 90NO↑ + 128MnO
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The reaction of potassium hexacyanidoferrate(II) and potassium permanganate yields potassium carbonate, potassium oxide, iron(II,III) oxide, nitrogen monoxide, and manganese(II) 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 hexacyanidoferrate(II) and potassium permanganate
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of potassium hexacyanidoferrate(II) and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K4[Fe(CN)6] | Potassium hexacyanidoferrate(II) | 15 | Reducing | Reducing |
| KMnO4 | Potassium permanganate | 128 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2CO3 | Potassium carbonate | 90 | Oxidized | – |
| K2O | Potassium oxide | 4 | – | – |
| Fe3O4 | Iron(II,III) oxide | 5 | Oxidized | – |
| NO | Nitrogen monoxide | 90 | Oxidized | – |
| MnO | Manganese(II) oxide | 128 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium hexacyanidoferrate(II) and potassium permanganate◆
ΔrG −39534.3 kJ/mol K 1.29 × 106926 pK −6926.11
| 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 | −35742.4 | −39534.3 | 13455.7 | −179.2 |
per 1 mol of | −2382.83 | −2635.62 | 897.047 | −11.95 |
per 1 mol of | −279.238 | −308.862 | 105.123 | −1.400 |
per 1 mol of | −397.138 | −439.270 | 149.508 | −1.991 |
per 1 mol of | −8935.60 | −9883.58 | 3363.93 | −44.80 |
per 1 mol of | −7148.48 | −7906.86 | 2691.14 | −35.84 |
per 1 mol of | −397.138 | −439.270 | 149.508 | −1.991 |
per 1 mol of | −279.238 | −308.862 | 105.123 | −1.400 |
Changes in aqueous solution
- Reaction of potassium hexacyanidoferrate(II) and potassium permanganate◆
ΔrG −43445.4 kJ/mol K 2.02 × 107611 pK −7611.30
| 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 | −44678.3 | −43445.4 | −4119.8 | – |
per 1 mol of | −2978.55 | −2896.36 | −274.65 | – |
per 1 mol of | −349.049 | −339.417 | −32.186 | – |
per 1 mol of | −496.426 | −482.727 | −45.776 | – |
per 1 mol of | −11169.6 | −10861.4 | −1030.0 | – |
per 1 mol of | −8935.66 | −8689.08 | −823.96 | – |
per 1 mol of | −496.426 | −482.727 | −45.776 | – |
per 1 mol of | −349.049 | −339.417 | −32.186 | – |
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 |
|---|---|---|---|---|
| K4[Fe(CN)6] (cr) | -594.1[1] | -453.0[1] | 418.8[1] | 332.21[1] |
| K4[Fe(CN)6] (ai) | -554.0[1] | -438.01[1] | 505.0[1] | – |
| K4[Fe(CN)6] (cr) 3 hydrate | -1466.5[1] | -1168.8[1] | 593.7[1] | 482.42[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
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 |
|---|---|---|---|---|
| K2CO3 (cr) | -1151.02[1] | -1063.5[1] | 155.52[1] | 114.43[1] |
| K2CO3 (ai) | -1181.90[1] | -1094.36[1] | 148.1[1] | – |
| K2CO3 (cr) 1.5 hydrate | -1609.2[1] | -1432.5[1] | 203.3[1] | – |
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[1] | – | – | – |
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| MnO (cr) | -385.22[1] | -362.90[1] | 59.71[1] | 45.44[1] |
| MnO (g) | 124.22[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°, -594.1 kJ · mol−1
- ^ ΔfG°, -453.0 kJ · mol−1
- ^ S°, 418.8 J · K−1 · mol−1
- ^ Cp°, 332.21 J · K−1 · mol−1
- ^ ΔfH°, -554.0 kJ · mol−1
- ^ ΔfG°, -438.01 kJ · mol−1
- ^ S°, 505.0 J · K−1 · mol−1
- ^ ΔfH°, -1466.5 kJ · mol−1
- ^ ΔfG°, -1168.8 kJ · mol−1
- ^ S°, 593.7 J · K−1 · mol−1
- ^ Cp°, 482.42 J · K−1 · 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°, -1151.02 kJ · mol−1
- ^ ΔfG°, -1063.5 kJ · mol−1
- ^ S°, 155.52 J · K−1 · mol−1
- ^ Cp°, 114.43 J · K−1 · mol−1
- ^ ΔfH°, -1181.90 kJ · mol−1
- ^ ΔfG°, -1094.36 kJ · mol−1
- ^ S°, 148.1 J · K−1 · mol−1
- ^ ΔfH°, -1609.2 kJ · mol−1
- ^ ΔfG°, -1432.5 kJ · mol−1
- ^ S°, 203.3 J · K−1 · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · 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°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 J · K−1 · 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
- 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