2K4[Fe(CN)6] + 50H2O 💧⚡→ 6KNO3 + K2CO3 + 2Fe(NO3)3 + 11CO↑ + 50H2↑
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- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent
Electrolysis of aqueous potassium hexacyanidoferrate(II) yields potassium nitrate, potassium carbonate, iron(III) nitrate, carbon monoxide, and (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(II) with water as oxidizing agent
General equation
- Electrolysis of aqueous solution with water as oxidizing agent
- Miscible with water/Very soluble in water/Soluble in waterReducing agent + H2OOxidizing agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K4[Fe(CN)6] | Potassium hexacyanidoferrate(II) | 2 | Reducing | Soluble in water |
| H2O | Water | 50 | Oxidizing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KNO3 | Potassium nitrate | 6 | Oxidized | – |
| K2CO3 | Potassium carbonate | 1 | Oxidized | – |
| Fe(NO3)3 | Iron(III) nitrate | 2 | Oxidized | – |
| CO | Carbon monoxide | 11 | – | – |
| 50 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 7085.5 kJ/mol K 0.47 × 10−1241 pK 1241.33
| 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 | 8902.0 | 7085.5 | 6091.4 | – |
per 1 mol of | 4451.0 | 3542.8 | 3045.7 | – |
per 1 mol of | 178.04 | 141.71 | 121.83 | – |
per 1 mol of | 1483.7 | 1180.9 | 1015.2 | – |
per 1 mol of | 8902.0 | 7085.5 | 6091.4 | – |
per 1 mol of | 4451.0 | 3542.8 | 3045.7 | – |
per 1 mol of | 809.27 | 644.14 | 553.76 | – |
| 178.04 | 141.71 | 121.83 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 7965.5 kJ/mol K 0.32 × 10−1395 pK 1395.50
| 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 | 8692.0 | 7965.5 | 28407 | – |
per 1 mol of | 4346.0 | 3982.8 | 14204 | – |
per 1 mol of | 173.84 | 159.31 | 568.14 | – |
per 1 mol of | 1448.7 | 1327.6 | 4734.5 | – |
per 1 mol of | 8692.0 | 7965.5 | 28407 | – |
per 1 mol of | 4346.0 | 3982.8 | 14204 | – |
per 1 mol of | 790.18 | 724.14 | 2582.5 | – |
| 173.84 | 159.31 | 568.14 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 7275.4 kJ/mol K 0.25 × 10−1274 pK 1274.59
| 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 | 8787.2 | 7275.4 | 5067.6 | – |
per 1 mol of | 4393.6 | 3637.7 | 2533.8 | – |
per 1 mol of | 175.74 | 145.51 | 101.35 | – |
per 1 mol of | 1464.5 | 1212.6 | 844.60 | – |
per 1 mol of | 8787.2 | 7275.4 | 5067.6 | – |
per 1 mol of | 4393.6 | 3637.7 | 2533.8 | – |
per 1 mol of | 798.84 | 661.40 | 460.69 | – |
| 175.74 | 145.51 | 101.35 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 8155.4 kJ/mol K 0.17 × 10−1428 pK 1428.76
| 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 | 8577.2 | 8155.4 | 27383 | – |
per 1 mol of | 4288.6 | 4077.7 | 13692 | – |
per 1 mol of | 171.54 | 163.11 | 547.66 | – |
per 1 mol of | 1429.5 | 1359.2 | 4563.8 | – |
per 1 mol of | 8577.2 | 8155.4 | 27383 | – |
per 1 mol of | 4288.6 | 4077.7 | 13692 | – |
per 1 mol of | 779.75 | 741.40 | 2489.4 | – |
| 171.54 | 163.11 | 547.66 | – |
Changes in aqueous solution (5)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent
| 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 | 8893.6 | – | – | – |
per 1 mol of | 4446.8 | – | – | – |
per 1 mol of | 177.87 | – | – | – |
per 1 mol of | 1482.3 | – | – | – |
per 1 mol of | 8893.6 | – | – | – |
per 1 mol of | 4446.8 | – | – | – |
per 1 mol of | 808.51 | – | – | – |
| 177.87 | – | – | – |
Changes in aqueous solution (6)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent
| 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 | 8683.6 | – | – | – |
per 1 mol of | 4341.8 | – | – | – |
per 1 mol of | 173.67 | – | – | – |
per 1 mol of | 1447.3 | – | – | – |
per 1 mol of | 8683.6 | – | – | – |
per 1 mol of | 4341.8 | – | – | – |
per 1 mol of | 789.42 | – | – | – |
| 173.67 | – | – | – |
Changes in aqueous solution (7)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent
| 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 | 8778.8 | – | – | – |
per 1 mol of | 4389.4 | – | – | – |
per 1 mol of | 175.58 | – | – | – |
per 1 mol of | 1463.1 | – | – | – |
per 1 mol of | 8778.8 | – | – | – |
per 1 mol of | 4389.4 | – | – | – |
per 1 mol of | 798.07 | – | – | – |
| 175.58 | – | – | – |
Changes in aqueous solution (8)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent
| 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 | 8568.8 | – | – | – |
per 1 mol of | 4284.4 | – | – | – |
per 1 mol of | 171.38 | – | – | – |
per 1 mol of | 1428.1 | – | – | – |
per 1 mol of | 8568.8 | – | – | – |
per 1 mol of | 4284.4 | – | – | – |
per 1 mol of | 778.98 | – | – | – |
| 171.38 | – | – | – |
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] |
| 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 |
|---|---|---|---|---|
| KNO3 (cr) | -494.63[1] | -394.86[1] | 133.05[1] | 96.40[1] |
| KNO3 (ai) | -459.74[1] | -394.53[1] | 248.9[1] | -64.9[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] | – | – | – |
| 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] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[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°, -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°, -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°, -494.63 kJ · mol−1
- ^ ΔfG°, -394.86 kJ · mol−1
- ^ S°, 133.05 J · K−1 · mol−1
- ^ Cp°, 96.40 J · K−1 · mol−1
- ^ ΔfH°, -459.74 kJ · mol−1
- ^ ΔfG°, -394.53 kJ · mol−1
- ^ S°, 248.9 J · K−1 · mol−1
- ^ Cp°, -64.9 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°, -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
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1