Fe2(SO4)3 + Fe3+ → 3FeSO4+
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- Reaction of iron(III) sulfate and iron(III) ion
The reaction of iron(III) sulfate and iron(III) ion yields iron(III) sulfate ion. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(III) sulfate and iron(III) ion
General equation
- Reaction of neutral species and cation
- CompoundLewis base + CationLewis acid ⟶ CationLewis conjugate
Oxidation state of each atom
- Reaction of iron(III) sulfate and iron(III) ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe2(SO4)3 | Iron(III) sulfate | 1 | Lewis base | Compound |
| Fe3+ | Iron(III) ion | 1 | Lewis acid | Cation |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeSO4+ | Iron(III) sulfate ion | 3 | Lewis conjugate | Cation |
Thermodynamic changes
Changes in standard condition
- Reaction of iron(III) sulfate and iron(III) ion◆
ΔrG −70.6 kJ/mol K 2.34 × 1012 pK −12.37 - Fe2(SO4)3Ionized aqueous solution + Fe3+Un-ionized aqueous solution3FeSO4+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 | 78.1 | −70.6 | 497 | – |
per 1 mol of | 78.1 | −70.6 | 497 | – |
per 1 mol of Iron(III) ion | 78.1 | −70.6 | 497 | – |
per 1 mol of Iron(III) sulfate ion | 26.0 | −23.5 | 166 | – |
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] | – |
| Fe3+ (g) | 5712.8[1] | – | – | – |
| Fe3+ (ao) | -48.5[1] | -4.7[1] | -315.9[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (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 |
|---|---|---|---|---|
| FeSO4+ (ao) | -931.8[1] | -772.7[1] | -130[1] | – |
* (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)