20NH4F + 5Fe2O3 🔥→ 2NO↑ + 10FeF2 + 13H2O + 18NH3↑
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- Reaction of ammonium fluoride and iron(III) oxide
- 20NH4FAmmonium fluoride + 5Fe2O3Iron(III) oxide2NO↑Nitrogen monoxide + 10FeF2Iron(II) fluoride + 13H2OWater + 18NH3↑Ammonia🔥⟶
The reaction of ammonium fluoride and iron(III) oxide yields nitrogen monoxide, iron(II) fluoride, water, and ammonia (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
- 20NH4FAmmonium fluoride + 5Fe2O3Iron(III) oxide2NO↑Nitrogen monoxide + 10FeF2Iron(II) fluoride + 13H2OWater + 18NH3↑Ammonia🔥⟶
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 | 20 | Reducing | Reducing |
| Fe2O3 | Iron(III) oxide | 5 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NO | Nitrogen monoxide | 2 | Oxidized | – |
| FeF2 | Iron(II) fluoride | 10 | Reduced | – |
| H2O | Water | 13 | – | – |
| NH3 | Ammonia | 18 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium fluoride and iron(III) oxide◆
ΔrG 792.9 kJ/mol K 0.12 × 10−138 pK 138.91
| 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 | 1921.9 | 792.9 | 3788.15 | 526.10 |
per 1 mol of | 96.095 | 39.64 | 189.407 | 26.305 |
per 1 mol of | 384.38 | 158.6 | 757.630 | 105.22 |
per 1 mol of | 960.95 | 396.4 | 1894.08 | 263.05 |
per 1 mol of | 192.19 | 79.29 | 378.815 | 52.610 |
per 1 mol of | 147.84 | 60.99 | 291.396 | 40.469 |
per 1 mol of | 106.77 | 44.05 | 210.453 | 29.228 |
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 | 1606.5 | – | – | – |
per 1 mol of | 80.325 | – | – | – |
per 1 mol of | 321.30 | – | – | – |
per 1 mol of | 803.25 | – | – | – |
per 1 mol of | 160.65 | – | – | – |
per 1 mol of | 123.58 | – | – | – |
per 1 mol of | 89.250 | – | – | – |
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 | 991.3 | – | – | – |
per 1 mol of | 49.56 | – | – | – |
per 1 mol of | 198.3 | – | – | – |
per 1 mol of | 495.6 | – | – | – |
per 1 mol of | 99.13 | – | – | – |
per 1 mol of | 76.25 | – | – | – |
per 1 mol of | 55.07 | – | – | – |
Changes in aqueous solution (3)
- Reaction of ammonium fluoride and iron(III) oxide◆
ΔrG 981.1 kJ/mol K 0.13 × 10−171 pK 171.88
| 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 | 1945.5 | 981.1 | 3235.4 | 2367.5 |
per 1 mol of | 97.275 | 49.05 | 161.77 | 118.38 |
per 1 mol of | 389.10 | 196.2 | 647.08 | 473.50 |
per 1 mol of | 972.75 | 490.6 | 1617.7 | 1183.8 |
per 1 mol of | 194.55 | 98.11 | 323.54 | 236.75 |
per 1 mol of | 149.65 | 75.47 | 248.88 | 182.12 |
per 1 mol of | 108.08 | 54.51 | 179.74 | 131.53 |
Changes in aqueous solution (4)
- Reaction of ammonium fluoride and iron(III) oxide◆
ΔrG 800.2 kJ/mol K 0.65 × 10−140 pK 140.19
| 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 | 1330.3 | 800.2 | 1774.7 | – |
per 1 mol of | 66.515 | 40.01 | 88.735 | – |
per 1 mol of | 266.06 | 160.0 | 354.94 | – |
per 1 mol of | 665.15 | 400.1 | 887.35 | – |
per 1 mol of | 133.03 | 80.02 | 177.47 | – |
per 1 mol of | 102.33 | 61.55 | 136.52 | – |
per 1 mol of | 73.906 | 44.46 | 98.594 | – |
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 |
|---|---|---|---|---|
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[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] | – | – | – |
| 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] |
| NH3 (g) | -46.11[1] | -16.45[1] | 192.45[1] | 35.06[1] |
| NH3 (ao) | -80.29[1] | -26.50[1] | 111.3[1] | – |
* (g):Gas, (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (l):Liquid, (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°, -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°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 J · K−1 · 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°, -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
- ^ ΔfH°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1