6NH2OH + 46Fe2O3 → 2Fe(NO3)3 + 9Fe(OH)2 + 27Fe3O4
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- Reaction of hydroxylamine and iron(III) oxide
- 6NH2OHHydroxylamine + 46Fe2O3Iron(III) oxide2Fe(NO3)3Iron(III) nitrate + 9Fe(OH)2Iron(II) hydroxide + 27Fe3O4Iron(II,III) oxide⟶
The reaction of hydroxylamine and iron(III) oxide yields iron(III) nitrate, iron(II) hydroxide, and iron(II,III) oxide (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 hydroxylamine and iron(III) oxide
- 6NH2OHHydroxylamine + 46Fe2O3Iron(III) oxide2Fe(NO3)3Iron(III) nitrate + 9Fe(OH)2Iron(II) hydroxide + 27Fe3O4Iron(II,III) oxide⟶
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 hydroxylamine and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH2OH | Hydroxylamine | 6 | Reducing | Reducing |
| Fe2O3 | Iron(III) oxide | 46 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe(NO3)3 | Iron(III) nitrate | 2 | Oxidized | – |
| Fe(OH)2 | Iron(II) hydroxide | 9 | Reduced | – |
| Fe3O4 | Iron(II,III) oxide | 27 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of hydroxylamine 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 | 1843.8 | – | – | – |
per 1 mol of Hydroxylamine | 307.30 | – | – | – |
per 1 mol of | 40.083 | – | – | – |
per 1 mol of | 921.90 | – | – | – |
per 1 mol of | 204.87 | – | – | – |
per 1 mol of | 68.289 | – | – | – |
Changes in aqueous solution (2)
- Reaction of hydroxylamine 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 | 1835.4 | – | – | – |
per 1 mol of Hydroxylamine | 305.90 | – | – | – |
per 1 mol of | 39.900 | – | – | – |
per 1 mol of | 917.70 | – | – | – |
per 1 mol of | 203.93 | – | – | – |
per 1 mol of | 67.978 | – | – | – |
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 |
|---|---|---|---|---|
| NH2OH (cr) | -114.2[1] | – | – | – |
| NH2OH (aq) | -98.3[1] | – | – | – |
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
* (cr):Crystalline solid, (aq):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 |
|---|---|---|---|---|
| Fe(NO3)3 (ai) | -670.7[1] | -338.3[1] | 123.4[1] | – |
| Fe(NO3)3 (aq) | -674.9[1] | – | – | – |
| Fe(NO3)3 (cr) 9 hydrate | -3285.3[1] | – | – | – |
| Fe(OH)2 (cr) precipitated | -569.0[1] | -486.5[1] | 88[1] | – |
| Fe(OH)2 (g) | -372[1] | – | – | – |
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (cr):Crystalline solid, (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°, -114.2 kJ · mol−1
- ^ ΔfH°, -98.3 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°, -670.7 kJ · mol−1
- ^ ΔfG°, -338.3 kJ · mol−1
- ^ S°, 123.4 J · K−1 · mol−1
- ^ ΔfH°, -674.9 kJ · mol−1
- ^ ΔfH°, -3285.3 kJ · mol−1
- ^ ΔfH°, -569.0 kJ · mol−1
- ^ ΔfG°, -486.5 kJ · mol−1
- ^ S°, 88. J · K−1 · mol−1
- ^ ΔfH°, -372. 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