Na4[Fe(CN)6] + 18H2O 💧⚡→ 2Na2CO3 + 6NO↑ + FeCO3 + 3CO↑ + 18H2↑
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- Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent
Electrolysis of aqueous sodium hexacyanidoferrate(II) yields sodium carbonate, nitrogen monoxide, iron(II) carbonate, 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 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 | 18 | Oxidizing | Water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2CO3 | Sodium carbonate | 2 | Oxidized | – |
NO | Nitrogen monoxide | 6 | Oxidized | – |
FeCO3 | Iron(II) carbonate | 1 | Oxidized | – |
CO | Carbon monoxide | 3 | – | – |
18 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 1958.70 kJ/mol K 0.71 × 10−343 pK 343.15
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 | 2804.5 | 1958.70 | 2835.6 | – |
per 1 mol of | 2804.5 | 1958.70 | 2835.6 | – |
per 1 mol of | 155.81 | 108.817 | 157.53 | – |
per 1 mol of | 1402.3 | 979.350 | 1417.8 | – |
per 1 mol of | 467.42 | 326.450 | 472.60 | – |
per 1 mol of | 2804.5 | 1958.70 | 2835.6 | – |
per 1 mol of | 934.83 | 652.900 | 945.20 | – |
155.81 | 108.817 | 157.53 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 2275.5 kJ/mol K 0.22 × 10−398 pK 398.65
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 | 2728.9 | 2275.5 | 10869 | – |
per 1 mol of | 2728.9 | 2275.5 | 10869 | – |
per 1 mol of | 151.61 | 126.42 | 603.83 | – |
per 1 mol of | 1364.5 | 1137.8 | 5434.5 | – |
per 1 mol of | 454.82 | 379.25 | 1811.5 | – |
per 1 mol of | 2728.9 | 2275.5 | 10869 | – |
per 1 mol of | 909.63 | 758.50 | 3623.0 | – |
151.61 | 126.42 | 603.83 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 2010.50 kJ/mol K 0.60 × 10−352 pK 352.22
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 | 2773.2 | 2010.50 | 2556.4 | – |
per 1 mol of | 2773.2 | 2010.50 | 2556.4 | – |
per 1 mol of | 154.07 | 111.694 | 142.02 | – |
per 1 mol of | 1386.6 | 1005.25 | 1278.2 | – |
per 1 mol of | 462.20 | 335.083 | 426.07 | – |
per 1 mol of | 2773.2 | 2010.50 | 2556.4 | – |
per 1 mol of | 924.40 | 670.167 | 852.13 | – |
154.07 | 111.694 | 142.02 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent◆
ΔrG 2327.3 kJ/mol K 0.19 × 10−407 pK 407.73
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 | 2697.6 | 2327.3 | 10590 | – |
per 1 mol of | 2697.6 | 2327.3 | 10590 | – |
per 1 mol of | 149.87 | 129.29 | 588.33 | – |
per 1 mol of | 1348.8 | 1163.7 | 5295.0 | – |
per 1 mol of | 449.60 | 387.88 | 1765.0 | – |
per 1 mol of | 2697.6 | 2327.3 | 10590 | – |
per 1 mol of | 899.20 | 775.77 | 3530.0 | – |
149.87 | 129.29 | 588.33 | – |
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 |
---|---|---|---|---|
Na2CO3 (cr) | -1130.68[1] | -1044.44[1] | 134.98[1] | 112.30[1] |
Na2CO3 (ai) | -1157.38[1] | -1051.64[1] | 61.1[1] | – |
Na2CO3 (cr) 1 hydrate | -1431.26[1] | -1285.31[1] | 168.11[1] | 145.60[1] |
Na2CO3 (cr) 7 hydrate | -3199.96[1] | -2714.2[1] | 422.2[1] | – |
Na2CO3 (cr) 10 hydrate | -4081.32[1] | -3427.66[1] | 562.7[1] | 550.32[1] |
NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
FeCO3 (cr) siderite | -740.57[1] | -666.67[1] | 92.9[1] | 82.13[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°, -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°, -1130.68 kJ · mol−1
- ^ ΔfG°, -1044.44 kJ · mol−1
- ^ S°, 134.98 J · K−1 · mol−1
- ^ Cp°, 112.30 J · K−1 · mol−1
- ^ ΔfH°, -1157.38 kJ · mol−1
- ^ ΔfG°, -1051.64 kJ · mol−1
- ^ S°, 61.1 J · K−1 · mol−1
- ^ ΔfH°, -1431.26 kJ · mol−1
- ^ ΔfG°, -1285.31 kJ · mol−1
- ^ S°, 168.11 J · K−1 · mol−1
- ^ Cp°, 145.60 J · K−1 · mol−1
- ^ ΔfH°, -3199.96 kJ · mol−1
- ^ ΔfG°, -2714.2 kJ · mol−1
- ^ S°, 422.2 J · K−1 · mol−1
- ^ ΔfH°, -4081.32 kJ · mol−1
- ^ ΔfG°, -3427.66 kJ · mol−1
- ^ S°, 562.7 J · K−1 · mol−1
- ^ Cp°, 550.32 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°, -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°, -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