2(NH4)3PO4 + 19Fe2O3 → 6NH2OH + 12Fe3O4 + 2FePO4 + 3H2O
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- Reaction of ammonium phosphate and iron(III) oxide
- 2(NH4)3PO4Ammonium phosphate + 19Fe2O3Iron(III) oxide6NH2OHHydroxylamine + 12Fe3O4Iron(II,III) oxide + 2FePO4Iron(III) phosphate + 3H2OWater⟶
The reaction of ammonium phosphate and iron(III) oxide yields hydroxylamine, iron(II,III) oxide, iron(III) phosphate, and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of ammonium phosphate and iron(III) oxide
- 2(NH4)3PO4Ammonium phosphate + 19Fe2O3Iron(III) oxide6NH2OHHydroxylamine + 12Fe3O4Iron(II,III) oxide + 2FePO4Iron(III) phosphate + 3H2OWater⟶
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of ammonium phosphate and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| (NH4)3PO4 | Ammonium phosphate | 2 | Reducing | Reducing |
| Fe2O3 | Iron(III) oxide | 19 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH2OH | Hydroxylamine | 6 | Oxidized | – |
| Fe3O4 | Iron(II,III) oxide | 12 | Reduced | – |
| FePO4 | Iron(III) phosphate | 2 | – | – |
| H2O | Water | 3 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium phosphate and iron(III) oxide
| 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 | 1445.1 | – | – | – |
per 1 mol of | 722.55 | – | – | – |
per 1 mol of | 76.058 | – | – | – |
per 1 mol of Hydroxylamine | 240.85 | – | – | – |
per 1 mol of | 120.42 | – | – | – |
per 1 mol of | 722.55 | – | – | – |
per 1 mol of | 481.70 | – | – | – |
Changes in aqueous solution
- Reaction of ammonium phosphate and iron(III) oxide
| 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 | 1546.5 | – | – | – |
per 1 mol of | 773.25 | – | – | – |
per 1 mol of | 81.395 | – | – | – |
per 1 mol of Hydroxylamine | 257.75 | – | – | – |
per 1 mol of | 128.88 | – | – | – |
per 1 mol of | 773.25 | – | – | – |
per 1 mol of | 515.50 | – | – | – |
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 |
|---|---|---|---|---|
| (NH4)3PO4 (cr) | -1671.9[1] | – | – | – |
| (NH4)3PO4 (ai) | -1674.9[1] | -1256.6[1] | 117[1] | – |
| (NH4)3PO4 (cr) 3 hydrate | -2555.6[1] | – | – | – |
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
* (cr):Crystalline solid, (ai):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 |
|---|---|---|---|---|
| NH2OH (cr) | -114.2[1] | – | – | – |
| NH2OH (aq) | -98.3[1] | – | – | – |
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
| FePO4 (cr) | -1297.5[1] | – | – | – |
| FePO4 (cr) 2 hydrate strengite | -1888.2[1] | -1657.5[1] | 171.25[1] | 180.54[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, (aq):Aqueous solution, (l):Liquid, (g):Gas
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°, -1671.9 kJ · mol−1
- ^ ΔfH°, -1674.9 kJ · mol−1
- ^ ΔfG°, -1256.6 kJ · mol−1
- ^ S°, 117. J · K−1 · mol−1
- ^ ΔfH°, -2555.6 kJ · mol−1
- ^ ΔfH°, -824.2 kJ · mol−1
- ^ ΔfG°, -742.2 kJ · mol−1
- ^ S°, 87.40 J · K−1 · mol−1
- ^ Cp°, 103.85 J · K−1 · mol−1
- ^ ΔfH°, -114.2 kJ · mol−1
- ^ ΔfH°, -98.3 kJ · mol−1
- ^ ΔfH°, -1118.4 kJ · mol−1
- ^ ΔfG°, -1015.4 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, 143.43 J · K−1 · mol−1
- ^ 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°, -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