FeOH2+ → Fe3+ + OH−
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- Electrolytic dissociation of iron(III) hydroxide ion
- FeOH2+Iron(III) hydroxide ionFe3+Iron(III) ion + OH−Hydroxide ion⟶
Electrolytic dissociation of iron(III) hydroxide ion yields iron(III) ion and hydroxide ion. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolytic dissociation of iron(III) hydroxide ion
- FeOH2+Iron(III) hydroxide ionFe3+Iron(III) ion + OH−Hydroxide ion⟶
General equation
- Electrolytic dissociation of ion
- Polyatomic ion ⟶ Cation/Electrically neutral + Anion/Electrically neutral
Oxidation state of each atom
- Electrolytic dissociation of iron(III) hydroxide ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeOH2+ | Iron(III) hydroxide ion | 1 | – | Polyatomic ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe3+ | Iron(III) ion | 1 | – | Cation |
| OH− | Hydroxide ion | 1 | – | Anion |
Thermodynamic changes
Changes in standard condition
- Electrolytic dissociation of iron(III) hydroxide ion◆
ΔrG 67.5 kJ/mol K 0.15 × 10−11 pK 11.83 - FeOH2+Un-ionized aqueous solutionFe3+Un-ionized aqueous solution + OH−Un-ionized aqueous solution⟶
| 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 | 12.3 | 67.5 | −185 | – |
per 1 mol of Iron(III) hydroxide ion | 12.3 | 67.5 | −185 | – |
per 1 mol of Iron(III) ion | 12.3 | 67.5 | −185 | – |
per 1 mol of Hydroxide ion | 12.3 | 67.5 | −185 | – |
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 |
|---|---|---|---|---|
| FeOH2+ (ao) | -290.8[1] | -229.41[1] | -142[1] | – |
* (ao):Un-ionized aqueous solution
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 |
|---|---|---|---|---|
| Fe3+ (g) | 5712.8[1] | – | – | – |
| Fe3+ (ao) | -48.5[1] | -4.7[1] | -315.9[1] | – |
| OH− (g) | -143.5[1] | – | – | – |
| OH− (ao) | -229.994[1] | -157.244[1] | -10.75[1] | -148.5[1] |
* (g):Gas, (ao):Un-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°, -290.8 kJ · mol−1
- ^ ΔfG°, -229.41 kJ · mol−1
- ^ S°, -142. J · K−1 · mol−1
- ^ ΔfH°, 5712.8 kJ · mol−1
- ^ ΔfH°, -48.5 kJ · mol−1
- ^ ΔfG°, -4.7 kJ · mol−1
- ^ S°, -315.9 J · K−1 · mol−1
- ^ ΔfH°, -143.5 kJ · mol−1
- ^ ΔfH°, -229.994 kJ · mol−1
- ^ ΔfG°, -157.244 kJ · mol−1
- ^ S°, -10.75 J · K−1 · mol−1
- ^ Cp°, -148.5 J · K−1 · mol−1