6NH4F + 7Fe2O3 → 6NH2OH + 12FeO + 2FeF3 + 3H2O
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- Reaction of ammonium fluoride and iron(III) oxide
- 6NH4FAmmonium fluoride + 7Fe2O3Iron(III) oxide6NH2OHHydroxylamine + 12FeOIron(II) oxide + 2FeF3Iron(III) fluoride + 3H2OWater⟶
The reaction of ammonium fluoride and iron(III) oxide yields hydroxylamine, iron(II) oxide, iron(III) fluoride, 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 fluoride and iron(III) oxide
- 6NH4FAmmonium fluoride + 7Fe2O3Iron(III) oxide6NH2OHHydroxylamine + 12FeOIron(II) oxide + 2FeF3Iron(III) fluoride + 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 fluoride and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4F | Ammonium fluoride | 6 | Reducing | Reducing |
| Fe2O3 | Iron(III) oxide | 7 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH2OH | Hydroxylamine | 6 | Oxidized | – |
| FeO | Iron(II) oxide | 12 | Reduced | – |
| FeF3 | Iron(III) fluoride | 2 | – | – |
| H2O | Water | 3 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of ammonium fluoride 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 | 1816.4 | – | – | – |
per 1 mol of | 302.73 | – | – | – |
per 1 mol of | 259.49 | – | – | – |
per 1 mol of Hydroxylamine | 302.73 | – | – | – |
per 1 mol of | 151.37 | – | – | – |
per 1 mol of | 908.20 | – | – | – |
per 1 mol of | 605.47 | – | – | – |
Changes in aqueous solution (2)
- Reaction of ammonium fluoride 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 | 1756.2 | – | – | – |
per 1 mol of | 292.70 | – | – | – |
per 1 mol of | 250.89 | – | – | – |
per 1 mol of Hydroxylamine | 292.70 | – | – | – |
per 1 mol of | 146.35 | – | – | – |
per 1 mol of | 878.10 | – | – | – |
per 1 mol of | 585.40 | – | – | – |
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 |
|---|---|---|---|---|
| NH4F (cr) | -463.96[1] | -348.68[1] | 71.96[1] | 65.27[1] |
| NH4F (ai) | -465.14[1] | -358.09[1] | 99.6[1] | -26.8[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] | – | – | – |
| FeO (cr) | -272.0[1] | – | – | – |
| FeF3 (ai) | -1046.4[1] | -840.9[1] | -357.3[1] | – |
| FeF3 (aq) | -1016.3[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, (ai):Ionized 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°, -463.96 kJ · mol−1
- ^ ΔfG°, -348.68 kJ · mol−1
- ^ S°, 71.96 J · K−1 · mol−1
- ^ Cp°, 65.27 J · K−1 · mol−1
- ^ ΔfH°, -465.14 kJ · mol−1
- ^ ΔfG°, -358.09 kJ · mol−1
- ^ S°, 99.6 J · K−1 · mol−1
- ^ Cp°, -26.8 J · K−1 · 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°, -272.0 kJ · mol−1
- ^ ΔfH°, -1046.4 kJ · mol−1
- ^ ΔfG°, -840.9 kJ · mol−1
- ^ S°, -357.3 J · K−1 · mol−1
- ^ ΔfH°, -1016.3 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