6Fe(NO3)3 + 100H2O 💧⚡→ 2Fe3O4 + 18NH3↑ + 73H2O2
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- Electrolysis of aqueous iron(III) nitrate with water as reducing agent
Electrolysis of aqueous iron(III) nitrate yields iron(II,III) oxide, ammonia, 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 iron(III) nitrate with water as reducing agent
General equation
- Electrolysis of aqueous solution with water as reducing agent
- Miscible with water/Very soluble in water/Soluble in waterOxidizing agent + H2OReducing agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous iron(III) nitrate with water as reducing agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe(NO3)3 | Iron(III) nitrate | 6 | Oxidizing | Very soluble in water |
| H2O | Water | 100 | Reducing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe3O4 | Iron(II,III) oxide | 2 | Reduced | – |
| NH3 | Ammonia | 18 | Reduced | – |
| 73 | Oxidized | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Electrolysis of aqueous iron(III) nitrate with water as reducing agent◆
ΔrG 13631.6 kJ/mol K 0.70 × 10−2388 pK 2388.15
| 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 | 15585.0 | 13631.6 | 6530.2 | – |
per 1 mol of | 2597.50 | 2271.93 | 1088.4 | – |
per 1 mol of | 155.850 | 136.316 | 65.302 | – |
per 1 mol of | 7792.50 | 6815.80 | 3265.1 | – |
per 1 mol of | 865.833 | 757.311 | 362.79 | – |
| 213.493 | 186.734 | 89.455 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous iron(III) nitrate with water as reducing agent◆
ΔrG 13450.7 kJ/mol K 0.35 × 10−2356 pK 2356.46
| 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 | 14969.8 | 13450.7 | 5069.5 | – |
per 1 mol of | 2494.97 | 2241.78 | 844.92 | – |
per 1 mol of | 149.698 | 134.507 | 50.695 | – |
per 1 mol of | 7484.90 | 6725.35 | 2534.8 | – |
per 1 mol of | 831.656 | 747.261 | 281.64 | – |
| 205.066 | 184.256 | 69.445 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous iron(III) nitrate with water as reducing 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 | 15610.2 | – | – | – |
per 1 mol of | 2601.70 | – | – | – |
per 1 mol of | 156.102 | – | – | – |
per 1 mol of | 7805.10 | – | – | – |
per 1 mol of | 867.233 | – | – | – |
| 213.838 | – | – | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous iron(III) nitrate with water as reducing 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 | 14995.0 | – | – | – |
per 1 mol of | 2499.17 | – | – | – |
per 1 mol of | 149.950 | – | – | – |
per 1 mol of | 7497.50 | – | – | – |
per 1 mol of | 833.056 | – | – | – |
| 205.411 | – | – | – |
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 |
|---|---|---|---|---|
| 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] | – | – | – |
| 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, (aq):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 |
|---|---|---|---|---|
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[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] | – |
| (l) | -187.78[1] | -120.35[1] | 109.6[1] | 89.1[1] |
| (g) | -136.31[1] | -105.57[1] | 232.7[1] | 43.1[1] |
| (ao) | -191.17[1] | -134.03[1] | 143.9[1] | – |
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -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°, -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°, -1118.4 kJ · mol−1
- ^ ΔfG°, -1015.4 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, 143.43 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
- ^ ΔfH°, -187.78 kJ · mol−1
- ^ ΔfG°, -120.35 kJ · mol−1
- ^ S°, 109.6 J · K−1 · mol−1
- ^ Cp°, 89.1 J · K−1 · mol−1
- ^ ΔfH°, -136.31 kJ · mol−1
- ^ ΔfG°, -105.57 kJ · mol−1
- ^ S°, 232.7 J · K−1 · mol−1
- ^ Cp°, 43.1 J · K−1 · mol−1
- ^ ΔfH°, -191.17 kJ · mol−1
- ^ ΔfG°, -134.03 kJ · mol−1
- ^ S°, 143.9 J · K−1 · mol−1