2Fe2(SO4)3 + 6H2O 💧⚡→ 4Fe(OH)3 + 6S + 9O2↑
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- Electrolysis of aqueous iron(III) sulfate with water as non-redox agent
Electrolysis of aqueous iron(III) sulfate yields iron(III) hydroxide, , 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) sulfate 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 iron(III) sulfate with water as non-redox agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe2(SO4)3 | Iron(III) sulfate | 2 | Self redox agent | Soluble in water |
| H2O | Water | 6 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe(OH)3 | Iron(III) hydroxide | 4 | – | – |
| 6 | Reduced | – | ||
| 9 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Electrolysis of aqueous iron(III) sulfate with water as non-redox 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 | 3586.0 | – | – | – |
per 1 mol of | 1793.0 | – | – | – |
per 1 mol of | 597.67 | – | – | – |
per 1 mol of | 896.50 | – | – | – |
| 597.67 | – | – | – | |
| 398.44 | – | – | – |
Changes in standard condition (2)
- Electrolysis of aqueous iron(III) sulfate with water as non-redox 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 | 3588.0 | – | – | – |
per 1 mol of | 1794.0 | – | – | – |
per 1 mol of | 598.00 | – | – | – |
per 1 mol of | 897.00 | – | – | – |
| 598.00 | – | – | – | |
| 398.67 | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous iron(III) sulfate with water as non-redox agent◆
ΔrG 3271.2 kJ/mol K 0.81 × 10−573 pK 573.09
| 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 | – | 3271.2 | – | – |
per 1 mol of | – | 1635.6 | – | – |
per 1 mol of | – | 545.20 | – | – |
per 1 mol of | – | 817.80 | – | – |
| – | 545.20 | – | – | |
| – | 363.47 | – | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous iron(III) sulfate with water as non-redox agent◆
ΔrG 3418.8 kJ/mol K 0.11 × 10−598 pK 598.95
| 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 | – | 3418.8 | – | – |
per 1 mol of | – | 1709.4 | – | – |
per 1 mol of | – | 569.80 | – | – |
per 1 mol of | – | 854.70 | – | – |
| – | 569.80 | – | – | |
| – | 379.87 | – | – |
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 |
|---|---|---|---|---|
| Fe2(SO4)3 (cr) | -2581.5[1] | – | – | – |
| Fe2(SO4)3 (ai) | -2825.0[1] | -2242.8[1] | -571.5[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 |
|---|---|---|---|---|
| Fe(OH)3 (cr) precipitated | -823.0[1] | -696.5[1] | 106.7[1] | – |
| Fe(OH)3 (ao) | – | -659.3[1] | – | – |
| (cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
| (cr) monoclinic | 0.33[1] | – | – | – |
| (g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (g):Gas
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°, -2581.5 kJ · mol−1
- ^ ΔfH°, -2825.0 kJ · mol−1
- ^ ΔfG°, -2242.8 kJ · mol−1
- ^ S°, -571.5 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°, -823.0 kJ · mol−1
- ^ ΔfG°, -696.5 kJ · mol−1
- ^ S°, 106.7 J · K−1 · mol−1
- ^ ΔfG°, -659.3 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 J · K−1 · mol−1