FePO4 + e− → Fe2+ + PO43−
Last updated:
- Reduction of iron(III) phosphate
Reduction of iron(III) phosphate yields iron(II) ion and phosphate ion (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reduction of iron(III) phosphate
General equation
- Reduction of reducible species
- ReactantOxidizing agent + e− ⟶ ProductReduction product
Oxidation state of each atom
- Reduction of iron(III) phosphate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FePO4 | Iron(III) phosphate | 1 | Oxidizing | – |
| e− | Electron | 1 | – | Electron |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe2+ | Iron(II) ion | 1 | Reduced | – |
| PO43− | Phosphate ion | 1 | – | – |
Thermodynamic changes
Changes in standard condition
- Reduction of iron(III) phosphate
| 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 | −69.0 | – | – | – |
per 1 mol of | −69.0 | – | – | – |
per 1 mol of Electron | −69.0 | – | – | – |
per 1 mol of Iron(II) ion | −69.0 | – | – | – |
per 1 mol of Phosphate ion | −69.0 | – | – | – |
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 |
|---|---|---|---|---|
| FePO4 (cr) | -1297.5[1] | – | – | – |
| FePO4 (cr) 2 hydrate strengite | -1888.2[1] | -1657.5[1] | 171.25[1] | 180.54[1] |
| e− | – | – | – | – |
* (cr):Crystalline solid
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 |
|---|---|---|---|---|
| Fe2+ (g) | 2749.93[1] | – | – | – |
| Fe2+ (ao) | -89.1[1] | -78.90[1] | -137.7[1] | – |
| PO43− (ao) | -1277.4[1] | -1018.7[1] | -220.3[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°, -1297.5 kJ · mol−1
- ^ ΔfH°, -1888.2 kJ · mol−1
- ^ ΔfG°, -1657.5 kJ · mol−1
- ^ S°, 171.25 J · K−1 · mol−1
- ^ Cp°, 180.54 J · K−1 · mol−1
- ^ ΔfH°, 2749.93 kJ · mol−1
- ^ ΔfH°, -89.1 kJ · mol−1
- ^ ΔfG°, -78.90 kJ · mol−1
- ^ S°, -137.7 J · K−1 · mol−1
- ^ ΔfH°, -1277.4 kJ · mol−1
- ^ ΔfG°, -1018.7 kJ · mol−1
- ^ S°, -220.3 J · K−1 · mol−1