2K3[Fe(CN)6] + 27H2O 💧⚡→ 3K2CO3 + 2Fe(NO3)3 + 9CH4↑ + 6NH3↑
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- Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
Electrolysis of aqueous potassium hexacyanidoferrate(III) yields potassium carbonate, iron(III) nitrate, , and ammonia (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
General equation
- Electrolysis of aqueous solution with water as non redox agent
- Miscible with water/Very soluble in water/Soluble in waterSelf redox agent + H2ONon-redox agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K3[Fe(CN)6] | Potassium hexacyanidoferrate(III) | 2 | Reducing | Very soluble in water |
| H2O | Water | 27 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2CO3 | Potassium carbonate | 3 | Oxidized | – |
| Fe(NO3)3 | Iron(III) nitrate | 2 | Oxidized | – |
| 9 | Reduced | – | ||
| NH3 | Ammonia | 6 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent◆
ΔrG 2128.4 kJ/mol K 0.13 × 10−372 pK 372.88 - 2K3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3K2CO3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 9↑Gas + 6NH3↑Gas💧⚡⟶
| 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 | 2271.2 | 2128.4 | 479.0 | – |
per 1 mol of | 1135.6 | 1064.2 | 239.5 | – |
per 1 mol of | 84.119 | 78.830 | 17.74 | – |
per 1 mol of | 757.07 | 709.47 | 159.7 | – |
per 1 mol of | 1135.6 | 1064.2 | 239.5 | – |
| 252.36 | 236.49 | 53.22 | – | |
per 1 mol of | 378.53 | 354.73 | 79.83 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent◆
ΔrG 2068.1 kJ/mol K 0.48 × 10−362 pK 362.32 - 2K3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3K2CO3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 9↑Gas + 6NH3↑Un-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 | 2066.1 | 2068.1 | −7.9 | – |
per 1 mol of | 1033.0 | 1034.0 | −4.0 | – |
per 1 mol of | 76.522 | 76.596 | −0.29 | – |
per 1 mol of | 688.70 | 689.37 | −2.6 | – |
per 1 mol of | 1033.0 | 1034.0 | −4.0 | – |
| 229.57 | 229.79 | −0.88 | – | |
per 1 mol of | 344.35 | 344.68 | −1.3 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent◆
ΔrG 2275.9 kJ/mol K 0.19 × 10−398 pK 398.72 - 2K3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3K2CO3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 9↑Un-ionized aqueous solution + 6NH3↑Gas💧⚡⟶
| 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 | 2143.1 | 2275.9 | −444.1 | – |
per 1 mol of | 1071.5 | 1138.0 | −222.1 | – |
per 1 mol of | 79.374 | 84.293 | −16.45 | – |
per 1 mol of | 714.37 | 758.63 | −148.0 | – |
per 1 mol of | 1071.5 | 1138.0 | −222.1 | – |
| 238.12 | 252.88 | −49.34 | – | |
per 1 mol of | 357.18 | 379.32 | −74.02 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent◆
ΔrG 2215.6 kJ/mol K 0.70 × 10−388 pK 388.16 - 2K3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3K2CO3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 9↑Un-ionized aqueous solution + 6NH3↑Un-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 | 1938.0 | 2215.6 | −931.0 | – |
per 1 mol of | 969.00 | 1107.8 | −465.5 | – |
per 1 mol of | 71.778 | 82.059 | −34.48 | – |
per 1 mol of | 646.00 | 738.53 | −310.3 | – |
per 1 mol of | 969.00 | 1107.8 | −465.5 | – |
| 215.33 | 246.18 | −103.4 | – | |
per 1 mol of | 323.00 | 369.27 | −155.2 | – |
Changes in aqueous solution (5)
- Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
- 2K3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3K2CO3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 9↑Gas + 6NH3↑Gas💧⚡⟶
| 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 | 2262.8 | – | – | – |
per 1 mol of | 1131.4 | – | – | – |
per 1 mol of | 83.807 | – | – | – |
per 1 mol of | 754.27 | – | – | – |
per 1 mol of | 1131.4 | – | – | – |
| 251.42 | – | – | – | |
per 1 mol of | 377.13 | – | – | – |
Changes in aqueous solution (6)
- Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
- 2K3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3K2CO3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 9↑Gas + 6NH3↑Un-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 | 2057.7 | – | – | – |
per 1 mol of | 1028.8 | – | – | – |
per 1 mol of | 76.211 | – | – | – |
per 1 mol of | 685.90 | – | – | – |
per 1 mol of | 1028.8 | – | – | – |
| 228.63 | – | – | – | |
per 1 mol of | 342.95 | – | – | – |
Changes in aqueous solution (7)
- Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
- 2K3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3K2CO3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 9↑Un-ionized aqueous solution + 6NH3↑Gas💧⚡⟶
| 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 | 2134.7 | – | – | – |
per 1 mol of | 1067.3 | – | – | – |
per 1 mol of | 79.063 | – | – | – |
per 1 mol of | 711.57 | – | – | – |
per 1 mol of | 1067.3 | – | – | – |
| 237.19 | – | – | – | |
per 1 mol of | 355.78 | – | – | – |
Changes in aqueous solution (8)
- Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
- 2K3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3K2CO3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 9↑Un-ionized aqueous solution + 6NH3↑Un-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 | 1929.6 | – | – | – |
per 1 mol of | 964.80 | – | – | – |
per 1 mol of | 71.467 | – | – | – |
per 1 mol of | 643.20 | – | – | – |
per 1 mol of | 964.80 | – | – | – |
| 214.40 | – | – | – | |
per 1 mol of | 321.60 | – | – | – |
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 |
|---|---|---|---|---|
| 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] | – |
| 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, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas
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] | – |
| 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] | – | – | – |
| (g) | -74.81[1] | -50.72[1] | 186.264[1] | 35.309[1] |
| (ao) | -89.04[1] | -34.33[1] | 83.7[1] | – |
| NH3 (g) | -46.11[1] | -16.45[1] | 192.45[1] | 35.06[1] |
| NH3 (ao) | -80.29[1] | -26.50[1] | 111.3[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°, -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°, -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
- ^ 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°, -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°, -74.81 kJ · mol−1
- ^ ΔfG°, -50.72 kJ · mol−1
- ^ S°, 186.264 J · K−1 · mol−1
- ^ Cp°, 35.309 J · K−1 · mol−1
- ^ ΔfH°, -89.04 kJ · mol−1
- ^ ΔfG°, -34.33 kJ · mol−1
- ^ S°, 83.7 J · K−1 · mol−1
- ^ ΔfH°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1