9Na4[Fe(CN)6] + 440MnO2 → 36NaNO3 + 6Fe(NO3)3 + Fe3O4 + 220Mn2O3 + 54CO↑
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The reaction of sodium hexacyanidoferrate(II) and manganese(IV) oxide yields sodium nitrate, iron(III) nitrate, iron(II,III) oxide, manganese(III) oxide, and carbon monoxide (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 manganese(IV) oxide
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of sodium hexacyanidoferrate(II) and manganese(IV) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na4[Fe(CN)6] | Sodium hexacyanidoferrate(II) | 9 | Reducing | Reducing |
| MnO2 | Manganese(IV) oxide | 440 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaNO3 | Sodium nitrate | 36 | Oxidized | – |
| Fe(NO3)3 | Iron(III) nitrate | 6 | Oxidized | – |
| Fe3O4 | Iron(II,III) oxide | 1 | Oxidized | – |
| Mn2O3 | Manganese(III) oxide | 220 | Reduced | – |
| CO | Carbon monoxide | 54 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of sodium hexacyanidoferrate(II) and manganese(IV) oxide◆
ΔrG −9893.3 kJ/mol K 1.70 × 101733 pK −1733.23
| 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 | −4842.0 | −9893.3 | 16944.6 | – |
per 1 mol of | −538.00 | −1099.3 | 1882.73 | – |
per 1 mol of | −11.005 | −22.485 | 38.5105 | – |
per 1 mol of | −134.50 | −274.81 | 470.683 | – |
per 1 mol of | −807.00 | −1648.9 | 2824.10 | – |
per 1 mol of | −4842.0 | −9893.3 | 16944.6 | – |
per 1 mol of | −22.009 | −44.970 | 77.0209 | – |
per 1 mol of | −89.667 | −183.21 | 313.789 | – |
Changes in aqueous solution (2)
- Reaction of sodium hexacyanidoferrate(II) and manganese(IV) oxide◆
ΔrG −8960.8 kJ/mol K 7.32 × 101569 pK −1569.86
| 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 | −5405.5 | −8960.8 | 11918.6 | – |
per 1 mol of | −600.61 | −995.64 | 1324.29 | – |
per 1 mol of | −12.285 | −20.365 | 27.0877 | – |
per 1 mol of | −150.15 | −248.91 | 331.072 | – |
per 1 mol of | −900.92 | −1493.5 | 1986.43 | – |
per 1 mol of | −5405.5 | −8960.8 | 11918.6 | – |
per 1 mol of | −24.570 | −40.731 | 54.1755 | – |
per 1 mol of | −100.10 | −165.94 | 220.715 | – |
Changes in aqueous solution (3)
- Reaction of sodium hexacyanidoferrate(II) and manganese(IV) oxide
| 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 | −4867.2 | – | – | – |
per 1 mol of | −540.80 | – | – | – |
per 1 mol of | −11.062 | – | – | – |
per 1 mol of | −135.20 | – | – | – |
per 1 mol of | −811.20 | – | – | – |
per 1 mol of | −4867.2 | – | – | – |
per 1 mol of | −22.124 | – | – | – |
per 1 mol of | −90.133 | – | – | – |
Changes in aqueous solution (4)
- Reaction of sodium hexacyanidoferrate(II) and manganese(IV) oxide
| 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 | −5430.7 | – | – | – |
per 1 mol of | −603.41 | – | – | – |
per 1 mol of | −12.342 | – | – | – |
per 1 mol of | −150.85 | – | – | – |
per 1 mol of | −905.12 | – | – | – |
per 1 mol of | −5430.7 | – | – | – |
per 1 mol of | −24.685 | – | – | – |
per 1 mol of | −100.57 | – | – | – |
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] | – |
| 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, (am):Amorphous 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 |
|---|---|---|---|---|
| NaNO3 (cr) | -467.85[1] | -367.00[1] | 116.52[1] | 92.88[1] |
| NaNO3 (ai) | -447.48[1] | -373.15[1] | 205.4[1] | -40.2[1] |
| Fe(NO3)3 (ai) | -670.7[1] | -338.3[1] | 123.4[1] | – |
| Fe(NO3)3 (aq) | -674.9[1] | – | – | – |
| Fe(NO3)3 (cr) 9 hydrate | -3285.3[1] | – | – | – |
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
| Mn2O3 (cr) | -959.0[1] | -881.1[1] | 110.5[1] | 107.65[1] |
| CO (g) | -110.525[1] | -137.168[1] | 197.674[1] | 29.142[1] |
| CO (ao) | -120.96[1] | -119.90[1] | 104.6[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (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°, -505.0 kJ · mol−1
- ^ ΔfG°, -352.53 kJ · mol−1
- ^ S°, 331.0 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°, -467.85 kJ · mol−1
- ^ ΔfG°, -367.00 kJ · mol−1
- ^ S°, 116.52 J · K−1 · mol−1
- ^ Cp°, 92.88 J · K−1 · mol−1
- ^ ΔfH°, -447.48 kJ · mol−1
- ^ ΔfG°, -373.15 kJ · mol−1
- ^ S°, 205.4 J · K−1 · mol−1
- ^ Cp°, -40.2 J · K−1 · mol−1
- ^ ΔfH°, -670.7 kJ · mol−1
- ^ ΔfG°, -338.3 kJ · mol−1
- ^ S°, 123.4 J · K−1 · mol−1
- ^ ΔfH°, -674.9 kJ · mol−1
- ^ ΔfH°, -3285.3 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°, -959.0 kJ · mol−1
- ^ ΔfG°, -881.1 kJ · mol−1
- ^ S°, 110.5 J · K−1 · mol−1
- ^ Cp°, 107.65 J · K−1 · mol−1
- ^ ΔfH°, -110.525 kJ · mol−1
- ^ ΔfG°, -137.168 kJ · mol−1
- ^ S°, 197.674 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -120.96 kJ · mol−1
- ^ ΔfG°, -119.90 kJ · mol−1
- ^ S°, 104.6 J · K−1 · mol−1