13Na4[Fe(CN)6] + 4KMnO4 🔥→ 12Na3[Fe(CN)6] + 8Na2O + 4MnO2 + K4[Fe(CN)6]
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The reaction of sodium hexacyanidoferrate(II) and potassium permanganate yields sodium hexacyanidoferrate(III), sodium oxide, manganese(IV) oxide, and potassium hexacyanidoferrate(II) (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 sodium 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 sodium hexacyanidoferrate(II) and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na4[Fe(CN)6] | Sodium hexacyanidoferrate(II) | 13 | Reducing | Reducing |
| KMnO4 | Potassium permanganate | 4 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na3[Fe(CN)6] | Sodium hexacyanidoferrate(III) | 12 | Oxidized | – |
| Na2O | Sodium oxide | 8 | – | – |
| MnO2 | Manganese(IV) oxide | 4 | Reduced | – |
| K4[Fe(CN)6] | Potassium hexacyanidoferrate(II) | 1 | – | – |
Thermodynamic changes
Changes in aqueous solution
- Reaction of sodium hexacyanidoferrate(II) and potassium permanganate◆
ΔrG 1525.8 kJ/mol K 0.49 × 10−267 pK 267.31 - 13Na4[Fe(CN)6]Ionized aqueous solution + 4KMnO4Ionized aqueous solution12Na3[Fe(CN)6]Ionized aqueous solution + 8Na2OCrystalline solid + 4MnO2Crystalline solid + K4[Fe(CN)6]Ionized aqueous solution🔥⟶
| 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 | 1889.1 | 1525.8 | 1207.5 | – |
per 1 mol of | 145.32 | 117.37 | 92.885 | – |
per 1 mol of | 472.27 | 381.45 | 301.88 | – |
per 1 mol of | 157.42 | 127.15 | 100.63 | – |
per 1 mol of | 236.14 | 190.72 | 150.94 | – |
per 1 mol of | 472.27 | 381.45 | 301.88 | – |
per 1 mol of | 1889.1 | 1525.8 | 1207.5 | – |
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 |
|---|---|---|---|---|
| Na4[Fe(CN)6] (ai) | -505.0[1] | -352.53[1] | 331.0[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] |
* (ai):Ionized aqueous solution, (cr):Crystalline solid
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 |
|---|---|---|---|---|
| Na3[Fe(CN)6] (ai) | -158.6[1] | -56.4[1] | 447.3[1] | – |
| Na2O (cr) | -414.22[1] | -375.46[1] | 75.06[1] | 69.12[1] |
| Na2O (g) | -35.6[1] | -52.3[1] | 261.2[1] | 55.2[1] |
| MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
| MnO2 (am) precipitated | -502.5[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] |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (g):Gas, (am):Amorphous solid
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°, -505.0 kJ · mol−1
- ^ ΔfG°, -352.53 kJ · mol−1
- ^ S°, 331.0 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°, -158.6 kJ · mol−1
- ^ ΔfG°, -56.4 kJ · mol−1
- ^ S°, 447.3 J · K−1 · mol−1
- ^ ΔfH°, -414.22 kJ · mol−1
- ^ ΔfG°, -375.46 kJ · mol−1
- ^ S°, 75.06 J · K−1 · mol−1
- ^ Cp°, 69.12 J · K−1 · mol−1
- ^ ΔfH°, -35.6 kJ · mol−1
- ^ ΔfG°, -52.3 kJ · mol−1
- ^ S°, 261.2 J · K−1 · mol−1
- ^ Cp°, 55.2 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°, -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