8FeCl3 + 4H2O 💧⚡→ 8FeCl2 + HClO4 + 7HCl↑
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- Electrolysis of aqueous iron(III) chloride with water as non-redox agent
Electrolysis of aqueous iron(III) chloride yields iron(II) chloride, perchloric acid, 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 | 8 | Self redox agent | Very soluble in water |
H2O | Water | 4 | – | Water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
FeCl2 | Iron(II) chloride | 8 | Reduced | – |
HClO4 | Perchloric acid | 1 | Oxidized | – |
HCl | Hydrogen chloride | 7 | – | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous iron(III) chloride 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 | 918.19 | – | – | – |
per 1 mol of | 114.77 | – | – | – |
per 1 mol of | 229.55 | – | – | – |
per 1 mol of | 114.77 | – | – | – |
per 1 mol of | 918.19 | – | – | – |
per 1 mol of | 131.17 | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 1276.1 kJ/mol K 0.27 × 10−223 pK 223.56
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 | – | 1276.1 | – | – |
per 1 mol of | – | 159.51 | – | – |
per 1 mol of | – | 319.02 | – | – |
per 1 mol of | – | 159.51 | – | – |
per 1 mol of | – | 1276.1 | – | – |
per 1 mol of | – | 182.30 | – | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 1024.6 kJ/mol K 0.31 × 10−179 pK 179.50
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 | – | 1024.6 | – | – |
per 1 mol of | – | 128.07 | – | – |
per 1 mol of | – | 256.15 | – | – |
per 1 mol of | – | 128.07 | – | – |
per 1 mol of | – | 1024.6 | – | – |
per 1 mol of | – | 146.37 | – | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 778.2 kJ/mol K 0.46 × 10−136 pK 136.33
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 | – | 778.2 | – | – |
per 1 mol of | – | 97.28 | – | – |
per 1 mol of | – | 194.6 | – | – |
per 1 mol of | – | 97.28 | – | – |
per 1 mol of | – | 778.2 | – | – |
per 1 mol of | – | 111.2 | – | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 526.7 kJ/mol K 0.53 × 10−92 pK 92.27
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 | – | 526.7 | – | – |
per 1 mol of | – | 65.84 | – | – |
per 1 mol of | – | 131.7 | – | – |
per 1 mol of | – | 65.84 | – | – |
per 1 mol of | – | 526.7 | – | – |
per 1 mol of | – | 75.24 | – | – |
Changes in aqueous solution (5)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 1226.5 kJ/mol K 0.13 × 10−214 pK 214.87
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 | – | 1226.5 | – | – |
per 1 mol of | – | 153.31 | – | – |
per 1 mol of | – | 306.63 | – | – |
per 1 mol of | – | 153.31 | – | – |
per 1 mol of | – | 1226.5 | – | – |
per 1 mol of | – | 175.21 | – | – |
Changes in aqueous solution (6)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 975.0 kJ/mol K 0.15 × 10−170 pK 170.81
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 | – | 975.0 | – | – |
per 1 mol of | – | 121.9 | – | – |
per 1 mol of | – | 243.8 | – | – |
per 1 mol of | – | 121.9 | – | – |
per 1 mol of | – | 975.0 | – | – |
per 1 mol of | – | 139.3 | – | – |
Changes in aqueous solution (7)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 728.6 kJ/mol K 0.23 × 10−127 pK 127.65
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 | 1382.2 | 728.6 | 2184.3 | – |
per 1 mol of | 172.78 | 91.08 | 273.04 | – |
per 1 mol of | 345.55 | 182.2 | 546.08 | – |
per 1 mol of | 172.78 | 91.08 | 273.04 | – |
per 1 mol of | 1382.2 | 728.6 | 2184.3 | – |
per 1 mol of | 197.46 | 104.1 | 312.04 | – |
Changes in aqueous solution (8)
- Electrolysis of aqueous iron(III) chloride with water as non-redox agent◆
ΔrG 477.1 kJ/mol K 0.26 × 10−83 pK 83.58
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 | 858.3 | 477.1 | 1271.5 | – |
per 1 mol of | 107.3 | 59.64 | 158.94 | – |
per 1 mol of | 214.6 | 119.3 | 317.88 | – |
per 1 mol of | 107.3 | 59.64 | 158.94 | – |
per 1 mol of | 858.3 | 477.1 | 1271.5 | – |
per 1 mol of | 122.6 | 68.16 | 181.64 | – |
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 |
---|---|---|---|---|
FeCl2 (cr) | -341.79[1] | -302.30[1] | 117.95[1] | 76.65[1] |
FeCl2 (g) | -148.5[1] | – | – | – |
FeCl2 (ai) | -423.4[1] | -341.34[1] | -24.7[1] | – |
FeCl2 (ao) | – | -279.1[1] | – | – |
FeCl2 (cr) 2 hydrate | -953.1[1] | – | – | – |
FeCl2 (cr) 4 hydrate | -1549.3[1] | – | – | – |
HClO4 (l) | -40.58[1] | – | – | – |
HClO4 (ai) | -129.33[1] | -8.52[1] | 182.0[1] | – |
HClO4 (cr) 1 hydrate | -382.21[1] | – | – | – |
HClO4 (l) 2 hydrate | -677.98[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, (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°, -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°, -341.79 kJ · mol−1
- ^ ΔfG°, -302.30 kJ · mol−1
- ^ S°, 117.95 J · K−1 · mol−1
- ^ Cp°, 76.65 J · K−1 · mol−1
- ^ ΔfH°, -148.5 kJ · mol−1
- ^ ΔfH°, -423.4 kJ · mol−1
- ^ ΔfG°, -341.34 kJ · mol−1
- ^ S°, -24.7 J · K−1 · mol−1
- ^ ΔfG°, -279.1 kJ · mol−1
- ^ ΔfH°, -953.1 kJ · mol−1
- ^ ΔfH°, -1549.3 kJ · mol−1
- ^ ΔfH°, -40.58 kJ · mol−1
- ^ ΔfH°, -129.33 kJ · mol−1
- ^ ΔfG°, -8.52 kJ · mol−1
- ^ S°, 182.0 J · K−1 · mol−1
- ^ ΔfH°, -382.21 kJ · mol−1
- ^ ΔfH°, -677.98 kJ · 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