4FeCl3 + 3H2O 💧⚡→ 4Fe + 3Cl2O↑ + 6HCl↑
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- Electrolysis of aqueous iron(III) chloride with water as non-redox agent
Electrolysis of aqueous iron(III) chloride yields , dichlorine monoxide, and hydrogen chloride (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) chloride 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) chloride with water as non-redox agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeCl3 | Iron(III) chloride | 4 | Self redox agent | Very soluble in water |
| H2O | Water | 3 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 4 | Reduced | – | ||
| Cl2O | Dichlorine monoxide | 3 | Oxidized | – |
| HCl | Hydrogen chloride | 6 | – | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 1769.3 kJ/mol K 0.11 × 10−309 pK 309.97
| 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 | 2142.5 | 1769.3 | 1250.3 | −201.15 |
per 1 mol of | 535.63 | 442.32 | 312.57 | −50.288 |
per 1 mol of | 714.17 | 589.77 | 416.77 | −67.050 |
| 535.63 | 442.32 | 312.57 | −50.288 | |
per 1 mol of | 714.17 | 589.77 | 416.77 | −67.050 |
per 1 mol of | 357.08 | 294.88 | 208.38 | −33.525 |
Changes in aqueous solution (1)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 2051.3 kJ/mol K 0.42 × 10−359 pK 359.37
| 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 | – | 2051.3 | – | – |
per 1 mol of | – | 512.83 | – | – |
per 1 mol of | – | 683.77 | – | – |
| – | 512.83 | – | – | |
per 1 mol of | – | 683.77 | – | – |
per 1 mol of | – | 341.88 | – | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 1835.7 kJ/mol K 0.25 × 10−321 pK 321.60
| 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 | – | 1835.7 | – | – |
per 1 mol of | – | 458.93 | – | – |
per 1 mol of | – | 611.90 | – | – |
| – | 458.93 | – | – | |
per 1 mol of | – | 611.90 | – | – |
per 1 mol of | – | 305.95 | – | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 2026.5 kJ/mol K 0.94 × 10−355 pK 355.03
| 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 | 2745.3 | 2026.5 | 2405.1 | – |
per 1 mol of | 686.33 | 506.63 | 601.27 | – |
per 1 mol of | 915.10 | 675.50 | 801.70 | – |
| 686.33 | 506.63 | 601.27 | – | |
per 1 mol of | 915.10 | 675.50 | 801.70 | – |
per 1 mol of | 457.55 | 337.75 | 400.85 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 1810.9 kJ/mol K 0.55 × 10−317 pK 317.26
| 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 | 2296.2 | 1810.9 | 1622.6 | – |
per 1 mol of | 574.05 | 452.73 | 405.65 | – |
per 1 mol of | 765.40 | 603.63 | 540.87 | – |
| 574.05 | 452.73 | 405.65 | – | |
per 1 mol of | 765.40 | 603.63 | 540.87 | – |
per 1 mol of | 382.70 | 301.82 | 270.43 | – |
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 |
|---|---|---|---|---|
| FeCl3 (cr) | -399.49[1] | -334.00[1] | 142.3[1] | 96.65[1] |
| FeCl3 (g) | -254.0[1] | – | – | – |
| FeCl3 (ai) | -550.2[1] | -398.3[1] | -146.4[1] | – |
| FeCl3 (ao) | – | -404.5[1] | – | – |
| FeCl3 (cr) 6 hydrate | -2223.8[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, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 27.28[1] | 25.10[1] |
| (g) | 416.3[1] | 370.7[1] | 180.490[1] | 25.677[1] |
| Cl2O (g) | 80.3[1] | 97.9[1] | 266.21[1] | 45.40[1] |
| HCl (g) | -92.307[1] | -95.299[1] | 186.908[1] | 29.12[1] |
| HCl (ai) | -167.159[1] | -131.228[1] | 56.5[1] | -136.4[1] |
* (cr):Crystalline solid, (g):Gas, (ai):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°, -399.49 kJ · mol−1
- ^ ΔfG°, -334.00 kJ · mol−1
- ^ S°, 142.3 J · K−1 · mol−1
- ^ Cp°, 96.65 J · K−1 · mol−1
- ^ ΔfH°, -254.0 kJ · mol−1
- ^ ΔfH°, -550.2 kJ · mol−1
- ^ ΔfG°, -398.3 kJ · mol−1
- ^ S°, -146.4 J · K−1 · mol−1
- ^ ΔfG°, -404.5 kJ · mol−1
- ^ ΔfH°, -2223.8 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 27.28 J · K−1 · mol−1
- ^ Cp°, 25.10 J · K−1 · mol−1
- ^ ΔfH°, 416.3 kJ · mol−1
- ^ ΔfG°, 370.7 kJ · mol−1
- ^ S°, 180.490 J · K−1 · mol−1
- ^ Cp°, 25.677 J · K−1 · mol−1
- ^ ΔfH°, 80.3 kJ · mol−1
- ^ ΔfG°, 97.9 kJ · mol−1
- ^ S°, 266.21 J · K−1 · mol−1
- ^ Cp°, 45.40 J · K−1 · mol−1
- ^ ΔfH°, -92.307 kJ · mol−1
- ^ ΔfG°, -95.299 kJ · mol−1
- ^ S°, 186.908 J · K−1 · mol−1
- ^ Cp°, 29.12 J · K−1 · mol−1
- ^ ΔfH°, -167.159 kJ · mol−1
- ^ ΔfG°, -131.228 kJ · mol−1
- ^ S°, 56.5 J · K−1 · mol−1
- ^ Cp°, -136.4 J · K−1 · mol−1