2K4[Fe(CN)6] + 35H2O 💧⚡→ 4K2CO3 + Fe2O3 + 12NO↑ + 8CO↑ + 35H2↑
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- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent
Electrolysis of aqueous potassium hexacyanidoferrate(II) yields potassium carbonate, iron(III) oxide, nitrogen monoxide, 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 | 35 | Oxidizing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2CO3 | Potassium carbonate | 4 | Oxidized | – |
| Fe2O3 | Iron(III) oxide | 1 | Oxidized | – |
| NO | Nitrogen monoxide | 12 | Oxidized | – |
| CO | Carbon monoxide | 8 | – | – |
| 35 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 4150.6 kJ/mol K 0.70 × 10−727 pK 727.15
| 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 | 5962.8 | 4150.6 | 6109.5 | −1137.93 |
per 1 mol of | 2981.4 | 2075.3 | 3054.8 | −568.965 |
per 1 mol of | 170.37 | 118.59 | 174.56 | −32.5123 |
per 1 mol of | 1490.7 | 1037.7 | 1527.4 | −284.483 |
per 1 mol of | 5962.8 | 4150.6 | 6109.5 | −1137.93 |
per 1 mol of | 496.90 | 345.88 | 509.13 | −94.8275 |
per 1 mol of | 745.35 | 518.83 | 763.69 | −142.241 |
| 170.37 | 118.59 | 174.56 | −32.5123 |
Changes in aqueous solution (1)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 3997.2 kJ/mol K 0.53 × 10−700 pK 700.28
| 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 | 5759.1 | 3997.2 | 5907.4 | – |
per 1 mol of | 2879.6 | 1998.6 | 2953.7 | – |
per 1 mol of | 164.55 | 114.21 | 168.78 | – |
per 1 mol of | 1439.8 | 999.30 | 1476.8 | – |
per 1 mol of | 5759.1 | 3997.2 | 5907.4 | – |
per 1 mol of | 479.93 | 333.10 | 492.28 | – |
per 1 mol of | 719.89 | 499.65 | 738.42 | – |
| 164.55 | 114.21 | 168.78 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 4613.2 kJ/mol K 0.63 × 10−808 pK 808.20
| 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 | 5612.1 | 4613.2 | 21528 | – |
per 1 mol of | 2806.1 | 2306.6 | 10764 | – |
per 1 mol of | 160.35 | 131.81 | 615.09 | – |
per 1 mol of | 1403.0 | 1153.3 | 5382.0 | – |
per 1 mol of | 5612.1 | 4613.2 | 21528 | – |
per 1 mol of | 467.68 | 384.43 | 1794.0 | – |
per 1 mol of | 701.51 | 576.65 | 2691.0 | – |
| 160.35 | 131.81 | 615.09 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 4135.3 kJ/mol K 0.34 × 10−724 pK 724.47
| 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 | 5675.6 | 4135.3 | 5162.8 | – |
per 1 mol of | 2837.8 | 2067.7 | 2581.4 | – |
per 1 mol of | 162.16 | 118.15 | 147.51 | – |
per 1 mol of | 1418.9 | 1033.8 | 1290.7 | – |
per 1 mol of | 5675.6 | 4135.3 | 5162.8 | – |
per 1 mol of | 472.97 | 344.61 | 430.23 | – |
per 1 mol of | 709.45 | 516.91 | 645.35 | – |
| 162.16 | 118.15 | 147.51 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous potassium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 4751.3 kJ/mol K 0.41 × 10−832 pK 832.39
| 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 | 5528.6 | 4751.3 | 20784 | – |
per 1 mol of | 2764.3 | 2375.7 | 10392 | – |
per 1 mol of | 157.96 | 135.75 | 593.83 | – |
per 1 mol of | 1382.2 | 1187.8 | 5196.0 | – |
per 1 mol of | 5528.6 | 4751.3 | 20784 | – |
per 1 mol of | 460.72 | 395.94 | 1732.0 | – |
per 1 mol of | 691.08 | 593.91 | 2598.0 | – |
| 157.96 | 135.75 | 593.83 | – |
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 |
|---|---|---|---|---|
| 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] | – |
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[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, (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°, -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°, -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°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 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
- ^ 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