6NH4F + 58Fe2O3 🔥→ 2Fe(NO3)3 + 3FeF2 + 12Fe(OH)2 + 33Fe3O4
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The reaction of ammonium fluoride and iron(III) oxide yields iron(III) nitrate, iron(II) fluoride, 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 ammonium fluoride and iron(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 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 | 58 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe(NO3)3 | Iron(III) nitrate | 2 | Oxidized | – |
| FeF2 | Iron(II) fluoride | 3 | Reduced | – |
| Fe(OH)2 | Iron(II) hydroxide | 12 | Reduced | – |
| Fe3O4 | Iron(II,III) oxide | 33 | Reduced | – |
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 | 3282.2 | – | – | – |
per 1 mol of | 547.03 | – | – | – |
per 1 mol of | 56.590 | – | – | – |
per 1 mol of | 1641.1 | – | – | – |
per 1 mol of | 1094.1 | – | – | – |
per 1 mol of | 273.52 | – | – | – |
per 1 mol of | 99.461 | – | – | – |
Changes in aqueous solution (2)
- Reaction of ammonium fluoride and iron(III) oxide◆
ΔrG 3167.5 kJ/mol K 0.12 × 10−554 pK 554.92
| 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 | 3383.9 | 3167.5 | 728 | – |
per 1 mol of | 563.98 | 527.92 | 121 | – |
per 1 mol of | 58.343 | 54.612 | 12.6 | – |
per 1 mol of | 1692.0 | 1583.8 | 364 | – |
per 1 mol of | 1128.0 | 1055.8 | 243 | – |
per 1 mol of | 281.99 | 263.96 | 60.7 | – |
per 1 mol of | 102.54 | 95.985 | 22.1 | – |
Changes in aqueous solution (3)
- 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 | 3273.8 | – | – | – |
per 1 mol of | 545.63 | – | – | – |
per 1 mol of | 56.445 | – | – | – |
per 1 mol of | 1636.9 | – | – | – |
per 1 mol of | 1091.3 | – | – | – |
per 1 mol of | 272.82 | – | – | – |
per 1 mol of | 99.206 | – | – | – |
Changes in aqueous solution (4)
- 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 | 3375.5 | – | – | – |
per 1 mol of | 562.58 | – | – | – |
per 1 mol of | 58.198 | – | – | – |
per 1 mol of | 1687.8 | – | – | – |
per 1 mol of | 1125.2 | – | – | – |
per 1 mol of | 281.29 | – | – | – |
per 1 mol of | 102.29 | – | – | – |
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 |
|---|---|---|---|---|
| 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] | – | – | – |
| FeF2 (cr) | -711.3[1] | -668.6[1] | 86.99[1] | 68.12[1] |
| FeF2 (ai) | -754.4[1] | -636.48[1] | -165.3[1] | – |
| FeF2 (aq) | -745.2[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°, -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°, -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°, -711.3 kJ · mol−1
- ^ ΔfG°, -668.6 kJ · mol−1
- ^ S°, 86.99 J · K−1 · mol−1
- ^ Cp°, 68.12 J · K−1 · mol−1
- ^ ΔfH°, -754.4 kJ · mol−1
- ^ ΔfG°, -636.48 kJ · mol−1
- ^ S°, -165.3 J · K−1 · mol−1
- ^ ΔfH°, -745.2 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