2Na3[Fe(CN)6] + 27H2O 💧⚡→ 3Na2CO3 + 2Fe(NO3)3 + 9CH4↑ + 6NH3↑
Last updated:
- Electrolysis of aqueous sodium hexacyanidoferrate(III) with water as non-redox agent
Electrolysis of aqueous sodium hexacyanidoferrate(III) yields sodium 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 sodium 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 sodium hexacyanidoferrate(III) with water as non-redox agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na3[Fe(CN)6] | Sodium hexacyanidoferrate(III) | 2 | Reducing | Soluble in water |
| H2O | Water | 27 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2CO3 | Sodium 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 sodium hexacyanidoferrate(III) with water as non-redox agent◆
ΔrG 2128.6 kJ/mol K 0.12 × 10−372 pK 372.91 - 2Na3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3Na2CO3Ionized 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 | 2271.1 | 2128.6 | 479.0 | – |
per 1 mol of | 1135.5 | 1064.3 | 239.5 | – |
per 1 mol of | 84.115 | 78.837 | 17.74 | – |
per 1 mol of | 757.03 | 709.53 | 159.7 | – |
per 1 mol of | 1135.5 | 1064.3 | 239.5 | – |
| 252.34 | 236.51 | 53.22 | – | |
per 1 mol of | 378.52 | 354.77 | 79.83 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous sodium hexacyanidoferrate(III) with water as non-redox agent◆
ΔrG 2068.3 kJ/mol K 0.45 × 10−362 pK 362.35 - 2Na3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3Na2CO3Ionized 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 | 2066.0 | 2068.3 | −7.9 | – |
per 1 mol of | 1033.0 | 1034.2 | −4.0 | – |
per 1 mol of | 76.519 | 76.604 | −0.29 | – |
per 1 mol of | 688.67 | 689.43 | −2.6 | – |
per 1 mol of | 1033.0 | 1034.2 | −4.0 | – |
| 229.56 | 229.81 | −0.88 | – | |
per 1 mol of | 344.33 | 344.72 | −1.3 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous sodium hexacyanidoferrate(III) with water as non-redox agent◆
ΔrG 2276.1 kJ/mol K 0.18 × 10−398 pK 398.76 - 2Na3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3Na2CO3Ionized 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 | 2276.1 | −444.1 | – |
per 1 mol of | 1071.5 | 1138.0 | −222.1 | – |
per 1 mol of | 79.374 | 84.300 | −16.45 | – |
per 1 mol of | 714.37 | 758.70 | −148.0 | – |
per 1 mol of | 1071.5 | 1138.0 | −222.1 | – |
| 238.12 | 252.90 | −49.34 | – | |
per 1 mol of | 357.18 | 379.35 | −74.02 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous sodium hexacyanidoferrate(III) with water as non-redox agent◆
ΔrG 2215.8 kJ/mol K 0.64 × 10−388 pK 388.19 - 2Na3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3Na2CO3Ionized 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 | 2215.8 | −931.0 | – |
per 1 mol of | 969.00 | 1107.9 | −465.5 | – |
per 1 mol of | 71.778 | 82.067 | −34.48 | – |
per 1 mol of | 646.00 | 738.60 | −310.3 | – |
per 1 mol of | 969.00 | 1107.9 | −465.5 | – |
| 215.33 | 246.20 | −103.4 | – | |
per 1 mol of | 323.00 | 369.30 | −155.2 | – |
Changes in aqueous solution (5)
- Electrolysis of aqueous sodium hexacyanidoferrate(III) with water as non-redox agent
- 2Na3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3Na2CO3Ionized 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 | 2262.7 | – | – | – |
per 1 mol of | 1131.3 | – | – | – |
per 1 mol of | 83.804 | – | – | – |
per 1 mol of | 754.23 | – | – | – |
per 1 mol of | 1131.3 | – | – | – |
| 251.41 | – | – | – | |
per 1 mol of | 377.12 | – | – | – |
Changes in aqueous solution (6)
- Electrolysis of aqueous sodium hexacyanidoferrate(III) with water as non-redox agent
- 2Na3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3Na2CO3Ionized 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 | 2057.6 | – | – | – |
per 1 mol of | 1028.8 | – | – | – |
per 1 mol of | 76.207 | – | – | – |
per 1 mol of | 685.87 | – | – | – |
per 1 mol of | 1028.8 | – | – | – |
| 228.62 | – | – | – | |
per 1 mol of | 342.93 | – | – | – |
Changes in aqueous solution (7)
- Electrolysis of aqueous sodium hexacyanidoferrate(III) with water as non-redox agent
- 2Na3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3Na2CO3Ionized 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 sodium hexacyanidoferrate(III) with water as non-redox agent
- 2Na3[Fe(CN)6]Ionized aqueous solution + 27H2OLiquid3Na2CO3Ionized 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 |
|---|---|---|---|---|
| Na3[Fe(CN)6] (ai) | -158.6[1] | -56.4[1] | 447.3[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] |
| 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°, -158.6 kJ · mol−1
- ^ ΔfG°, -56.4 kJ · mol−1
- ^ S°, 447.3 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°, -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