6NH4Cl + 46Fe2O3 🔥→ 6NO↑ + 3FeCl2 + 27Fe3O4 + 8Fe(OH)3
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The reaction of ammonium chloride and iron(III) oxide yields nitrogen monoxide, iron(II) chloride, iron(II,III) oxide, and iron(III) hydroxide (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 chloride 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 chloride and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4Cl | Ammonium chloride | 6 | Reducing | Reducing |
| Fe2O3 | Iron(III) oxide | 46 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NO | Nitrogen monoxide | 6 | Oxidized | – |
| FeCl2 | Iron(II) chloride | 3 | Reduced | – |
| Fe3O4 | Iron(II,III) oxide | 27 | Reduced | – |
| Fe(OH)3 | Iron(III) hydroxide | 8 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium chloride and iron(III) oxide◆
ΔrG 1983.0 kJ/mol K 0.39 × 10−347 pK 347.41
| 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 | 2535.1 | 1983.0 | 1836.8 | – |
per 1 mol of | 422.52 | 330.50 | 306.13 | – |
per 1 mol of | 55.111 | 43.109 | 39.930 | – |
per 1 mol of | 422.52 | 330.50 | 306.13 | – |
per 1 mol of | 845.03 | 661.00 | 612.27 | – |
per 1 mol of | 93.893 | 73.444 | 68.030 | – |
per 1 mol of | 316.89 | 247.88 | 229.60 | – |
Changes in aqueous solution (1)
- Reaction of ammonium chloride and iron(III) oxide◆
ΔrG 2396.1 kJ/mol K 0.17 × 10−419 pK 419.78
| 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 | – | 2396.1 | – | – |
per 1 mol of | – | 399.35 | – | – |
per 1 mol of | – | 52.089 | – | – |
per 1 mol of | – | 399.35 | – | – |
per 1 mol of | – | 798.70 | – | – |
per 1 mol of | – | 88.744 | – | – |
per 1 mol of | – | 299.51 | – | – |
Changes in aqueous solution (2)
- Reaction of ammonium chloride and iron(III) oxide◆
ΔrG 2209.4 kJ/mol K 0.85 × 10−387 pK 387.07
| 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 | – | 2209.4 | – | – |
per 1 mol of | – | 368.23 | – | – |
per 1 mol of | – | 48.030 | – | – |
per 1 mol of | – | 368.23 | – | – |
per 1 mol of | – | 736.47 | – | – |
per 1 mol of | – | 81.830 | – | – |
per 1 mol of | – | 276.18 | – | – |
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 |
|---|---|---|---|---|
| NH4Cl (cr) | -314.43[1] | -202.87[1] | 94.6[1] | 84.1[1] |
| NH4Cl (ai) | -299.66[1] | -210.52[1] | 169.9[1] | -56.5[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] |
| FeCl2 (cr) | -341.79[1] | -302.30[1] | 117.95[1] | 76.65[1] |
| FeCl2 (g) | -148.5[1] | – | – | – |
| FeCl2 (ai) | -423.4[1] | -341.34[1] | -24.7[1] | – |
| FeCl2 (ao) | – | -279.1[1] | – | – |
| FeCl2 (cr) 2 hydrate | -953.1[1] | – | – | – |
| FeCl2 (cr) 4 hydrate | -1549.3[1] | – | – | – |
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
| Fe(OH)3 (cr) precipitated | -823.0[1] | -696.5[1] | 106.7[1] | – |
| Fe(OH)3 (ao) | – | -659.3[1] | – | – |
* (g):Gas, (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, -314.43 kJ · mol−1
- ^ ΔfG°, -202.87 kJ · mol−1
- ^ S°, 94.6 J · K−1 · mol−1
- ^ Cp°, 84.1 J · K−1 · mol−1
- ^ ΔfH°, -299.66 kJ · mol−1
- ^ ΔfG°, -210.52 kJ · mol−1
- ^ S°, 169.9 J · K−1 · mol−1
- ^ Cp°, -56.5 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°, -341.79 kJ · mol−1
- ^ ΔfG°, -302.30 kJ · mol−1
- ^ S°, 117.95 J · K−1 · mol−1
- ^ Cp°, 76.65 J · K−1 · mol−1
- ^ ΔfH°, -148.5 kJ · mol−1
- ^ ΔfH°, -423.4 kJ · mol−1
- ^ ΔfG°, -341.34 kJ · mol−1
- ^ S°, -24.7 J · K−1 · mol−1
- ^ ΔfG°, -279.1 kJ · mol−1
- ^ ΔfH°, -953.1 kJ · mol−1
- ^ ΔfH°, -1549.3 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°, -823.0 kJ · mol−1
- ^ ΔfG°, -696.5 kJ · mol−1
- ^ S°, 106.7 J · K−1 · mol−1
- ^ ΔfG°, -659.3 kJ · mol−1