9Na4[Fe(CN)6] + 3KMnO4 🔥→ 4Na3[Fe(CN)6] + 24NaCN + K3[Fe(CN)6] + 2Fe2O3 + 3MnO2
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- Reaction of sodium hexacyanidoferrate(II) and potassium permanganate
The reaction of sodium hexacyanidoferrate(II) and potassium permanganate yields sodium hexacyanidoferrate(III), sodium cyanide, potassium hexacyanidoferrate(III), iron(III) oxide, and manganese(IV) 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 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) | 9 | Reducing | Reducing |
KMnO4 | Potassium permanganate | 3 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na3[Fe(CN)6] | Sodium hexacyanidoferrate(III) | 4 | Oxidized | – |
NaCN | Sodium cyanide | 24 | – | – |
K3[Fe(CN)6] | Potassium hexacyanidoferrate(III) | 1 | Oxidized | – |
Fe2O3 | Iron(III) oxide | 2 | Oxidized | – |
MnO2 | Manganese(IV) oxide | 3 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution
- Reaction of sodium hexacyanidoferrate(II) and potassium permanganate◆
ΔrG −9.6 kJ/mol K 4.81 × 101 pK −1.68 - 9Na4[Fe(CN)6]Ionized aqueous solution + 3KMnO4Ionized aqueous solution4Na3[Fe(CN)6]Ionized aqueous solution + 24NaCNIonized aqueous solution + K3[Fe(CN)6]Ionized aqueous solution + 2Fe2O3Crystalline solid + 3MnO2Crystalline solid🔥⟶
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 | 740.1 | −9.6 | 2515.3 | – |
per 1 mol of | 82.23 | −1.1 | 279.48 | – |
per 1 mol of | 246.7 | −3.2 | 838.43 | – |
per 1 mol of | 185.0 | −2.4 | 628.83 | – |
per 1 mol of | 30.84 | −0.40 | 104.80 | – |
per 1 mol of | 740.1 | −9.6 | 2515.3 | – |
per 1 mol of | 370.1 | −4.8 | 1257.7 | – |
per 1 mol of | 246.7 | −3.2 | 838.43 | – |
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] | – |
NaCN (cr) cubic | -87.49[1] | -76.43[1] | 115.60[1] | 70.37[1] |
NaCN (cr) orthorhombic | -90.75[1] | – | – | – |
NaCN (g) | 109[1] | 79.94[1] | 249.43[1] | 51.17[1] |
NaCN (ai) | -89.5[1] | -89.5[1] | 153.1[1] | – |
NaCN (cr) 1/2 hydrate | -235.77[1] | – | – | – |
NaCN (cr) 2 hydrate | -679.77[1] | – | – | – |
K3[Fe(CN)6] (cr) | -249.8[1] | -129.6[1] | 426.06[1] | – |
K3[Fe(CN)6] (ai) | -195.4[1] | -120.4[1] | 577.8[1] | – |
Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
MnO2 (am) precipitated | -502.5[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°, -87.49 kJ · mol−1
- ^ ΔfG°, -76.43 kJ · mol−1
- ^ S°, 115.60 J · K−1 · mol−1
- ^ Cp°, 70.37 J · K−1 · mol−1
- ^ ΔfH°, -90.75 kJ · mol−1
- ^ ΔfH°, 109. kJ · mol−1
- ^ ΔfG°, 79.94 kJ · mol−1
- ^ S°, 249.43 J · K−1 · mol−1
- ^ Cp°, 51.17 J · K−1 · mol−1
- ^ ΔfH°, -89.5 kJ · mol−1
- ^ ΔfG°, -89.5 kJ · mol−1
- ^ S°, 153.1 J · K−1 · mol−1
- ^ ΔfH°, -235.77 kJ · mol−1
- ^ ΔfH°, -679.77 kJ · mol−1
- ^ ΔfH°, -249.8 kJ · mol−1
- ^ ΔfG°, -129.6 kJ · mol−1
- ^ S°, 426.06 J · K−1 · mol−1
- ^ ΔfH°, -195.4 kJ · mol−1
- ^ ΔfG°, -120.4 kJ · mol−1
- ^ S°, 577.8 J · K−1 · mol−1
- ^ ΔfH°, -824.2 kJ · mol−1
- ^ ΔfG°, -742.2 kJ · mol−1
- ^ S°, 87.40 J · K−1 · mol−1
- ^ Cp°, 103.85 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