Na4[Fe(CN)6] + 25H2O 💧⚡→ 4NaNO2 + 2HNO2 + FeCO3 + 5CO2↑ + 24H2↑
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- Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent
Electrolysis of aqueous sodium hexacyanidoferrate(II) yields sodium nitrite, nitrous acid, iron(II) carbonate, carbon dioxide, 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 sodium 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 sodium hexacyanidoferrate(II) with water as oxidizing agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na4[Fe(CN)6] | Sodium hexacyanidoferrate(II) | 1 | Reducing | Soluble in water |
| H2O | Water | 25 | Oxidizing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaNO2 | Sodium nitrite | 4 | Oxidized | – |
| HNO2 | Nitrous acid | 2 | Oxidized | – |
| FeCO3 | Iron(II) carbonate | 1 | Oxidized | – |
| CO2 | Carbon dioxide | 5 | Oxidized | – |
| 24 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 2364.7 kJ/mol K 0.53 × 10−414 pK 414.28
| 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 | 3325.0 | 2364.7 | 3218.5 | – |
per 1 mol of | 3325.0 | 2364.7 | 3218.5 | – |
per 1 mol of | 133.00 | 94.588 | 128.74 | – |
per 1 mol of | 831.25 | 591.17 | 804.63 | – |
per 1 mol of | 1662.5 | 1182.3 | 1609.3 | – |
per 1 mol of | 3325.0 | 2364.7 | 3218.5 | – |
per 1 mol of | 665.00 | 472.94 | 643.70 | – |
| 138.54 | 98.529 | 134.10 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 2787.1 kJ/mol K 0.53 × 10−488 pK 488.28
| 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 | 3224.2 | 2787.1 | 13930 | – |
per 1 mol of | 3224.2 | 2787.1 | 13930 | – |
per 1 mol of | 128.97 | 111.48 | 557.20 | – |
per 1 mol of | 806.05 | 696.77 | 3482.5 | – |
per 1 mol of | 1612.1 | 1393.5 | 6965.0 | – |
per 1 mol of | 3224.2 | 2787.1 | 13930 | – |
per 1 mol of | 644.84 | 557.42 | 2786.0 | – |
| 134.34 | 116.13 | 580.42 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 2406.6 kJ/mol K 0.24 × 10−421 pK 421.62
| 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 | 3223.6 | 2406.6 | 2737.8 | – |
per 1 mol of | 3223.6 | 2406.6 | 2737.8 | – |
per 1 mol of | 128.94 | 96.264 | 109.51 | – |
per 1 mol of | 805.90 | 601.65 | 684.45 | – |
per 1 mol of | 1611.8 | 1203.3 | 1368.9 | – |
per 1 mol of | 3223.6 | 2406.6 | 2737.8 | – |
per 1 mol of | 644.72 | 481.32 | 547.56 | – |
| 134.32 | 100.27 | 114.08 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 2829.0 kJ/mol K 0.24 × 10−495 pK 495.62
| 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 | 3122.8 | 2829.0 | 13449 | – |
per 1 mol of | 3122.8 | 2829.0 | 13449 | – |
per 1 mol of | 124.91 | 113.16 | 537.96 | – |
per 1 mol of | 780.70 | 707.25 | 3362.3 | – |
per 1 mol of | 1561.4 | 1414.5 | 6724.5 | – |
per 1 mol of | 3122.8 | 2829.0 | 13449 | – |
per 1 mol of | 624.56 | 565.80 | 2689.8 | – |
| 130.12 | 117.88 | 560.38 | – |
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 |
|---|---|---|---|---|
| Na4[Fe(CN)6] (ai) | -505.0[1] | -352.53[1] | 331.0[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] |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| NaNO2 (cr) | -358.65[1] | -284.55[1] | 103.8[1] | – |
| NaNO2 (ai) | -344.8[1] | -294.1[1] | 182.0[1] | -51.0[1] |
| HNO2 (g) cis | -77.99[1] | -42.94[1] | 248.76[1] | 44.77[1] |
| HNO2 (g) trans | -80.12[1] | -45.24[1] | 249.22[1] | 46.07[1] |
| HNO2 (g) | -79.5[1] | -46.0[1] | 254.1[1] | 45.6[1] |
| HNO2 (ao) | -119.2[1] | -50.6[1] | 135.6[1] | – |
| FeCO3 (cr) siderite | -740.57[1] | -666.67[1] | 92.9[1] | 82.13[1] |
| CO2 (g) | -393.509[1] | -394.359[1] | 213.74[1] | 37.11[1] |
| CO2 (ao) | -413.80[1] | -385.98[1] | 117.6[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°, -505.0 kJ · mol−1
- ^ ΔfG°, -352.53 kJ · mol−1
- ^ S°, 331.0 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°, -358.65 kJ · mol−1
- ^ ΔfG°, -284.55 kJ · mol−1
- ^ S°, 103.8 J · K−1 · mol−1
- ^ ΔfH°, -344.8 kJ · mol−1
- ^ ΔfG°, -294.1 kJ · mol−1
- ^ S°, 182.0 J · K−1 · mol−1
- ^ Cp°, -51.0 J · K−1 · mol−1
- ^ ΔfH°, -77.99 kJ · mol−1
- ^ ΔfG°, -42.94 kJ · mol−1
- ^ S°, 248.76 J · K−1 · mol−1
- ^ Cp°, 44.77 J · K−1 · mol−1
- ^ ΔfH°, -80.12 kJ · mol−1
- ^ ΔfG°, -45.24 kJ · mol−1
- ^ S°, 249.22 J · K−1 · mol−1
- ^ Cp°, 46.07 J · K−1 · mol−1
- ^ ΔfH°, -79.5 kJ · mol−1
- ^ ΔfG°, -46.0 kJ · mol−1
- ^ S°, 254.1 J · K−1 · mol−1
- ^ Cp°, 45.6 J · K−1 · mol−1
- ^ ΔfH°, -119.2 kJ · mol−1
- ^ ΔfG°, -50.6 kJ · mol−1
- ^ S°, 135.6 J · K−1 · mol−1
- ^ ΔfH°, -740.57 kJ · mol−1
- ^ ΔfG°, -666.67 kJ · mol−1
- ^ S°, 92.9 J · K−1 · mol−1
- ^ Cp°, 82.13 J · K−1 · mol−1
- ^ ΔfH°, -393.509 kJ · mol−1
- ^ ΔfG°, -394.359 kJ · mol−1
- ^ S°, 213.74 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -413.80 kJ · mol−1
- ^ ΔfG°, -385.98 kJ · mol−1
- ^ S°, 117.6 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