Fe2(SO4)3 + H2O 💧⚡→ 2FeSO4 + H2SO3 + O2↑
Last updated:
- Electrolysis of aqueous iron(III) sulfate with water as non-redox agent
Electrolysis of aqueous iron(III) sulfate yields iron(II) sulfate, sulfurous acid, 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 | 1 | Self redox agent | Soluble in water |
| H2O | Water | 1 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeSO4 | Iron(II) sulfate | 2 | Reduced | – |
| H2SO3 | Sulfurous acid | 1 | Reduced | – |
| 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Electrolysis of aqueous iron(III) sulfate with water as non-redox agent◆
ΔrG 300.5 kJ/mol K 0.23 × 10−52 pK 52.65
| 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 | 645.2 | 300.5 | 1153.9 | – |
per 1 mol of | 645.2 | 300.5 | 1153.9 | – |
per 1 mol of | 645.2 | 300.5 | 1153.9 | – |
per 1 mol of | 322.6 | 150.3 | 576.95 | – |
per 1 mol of | 645.2 | 300.5 | 1153.9 | – |
| 645.2 | 300.5 | 1153.9 | – |
Changes in standard condition (2)
- Electrolysis of aqueous iron(III) sulfate with water as non-redox agent◆
ΔrG 316.9 kJ/mol K 0.30 × 10−55 pK 55.52
| 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 | 633.5 | 316.9 | 1059.7 | – |
per 1 mol of | 633.5 | 316.9 | 1059.7 | – |
per 1 mol of | 633.5 | 316.9 | 1059.7 | – |
per 1 mol of | 316.8 | 158.4 | 529.85 | – |
per 1 mol of | 633.5 | 316.9 | 1059.7 | – |
| 633.5 | 316.9 | 1059.7 | – |
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 |
|---|---|---|---|---|
| FeSO4 (cr) | -928.4[1] | -820.8[1] | 107.5[1] | 100.58[1] |
| FeSO4 (ai) | -998.3[1] | -823.43[1] | -117.6[1] | – |
| FeSO4 (cr) 1 hydrate | -1243.69[1] | – | – | – |
| FeSO4 (cr) 4 hydrate | -2129.2[1] | – | – | – |
| FeSO4 (cr) 7 hydrate | -3014.57[1] | -2509.87[1] | 409.2[1] | 394.47[1] |
| H2SO3 (ao) | -608.81[1] | -537.81[1] | 232.2[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, (ai):Ionized aqueous solution, (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°, -928.4 kJ · mol−1
- ^ ΔfG°, -820.8 kJ · mol−1
- ^ S°, 107.5 J · K−1 · mol−1
- ^ Cp°, 100.58 J · K−1 · mol−1
- ^ ΔfH°, -998.3 kJ · mol−1
- ^ ΔfG°, -823.43 kJ · mol−1
- ^ S°, -117.6 J · K−1 · mol−1
- ^ ΔfH°, -1243.69 kJ · mol−1
- ^ ΔfH°, -2129.2 kJ · mol−1
- ^ ΔfH°, -3014.57 kJ · mol−1
- ^ ΔfG°, -2509.87 kJ · mol−1
- ^ S°, 409.2 J · K−1 · mol−1
- ^ Cp°, 394.47 J · K−1 · mol−1
- ^ ΔfH°, -608.81 kJ · mol−1
- ^ ΔfG°, -537.81 kJ · mol−1
- ^ S°, 232.2 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