2NH4Cl + 8Fe2O3 🔥→ N2↑ + FeCl2 + 5Fe3O4 + 4H2O
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- Reaction of ammonium chloride and iron(III) oxide
The reaction of ammonium chloride and iron(III) oxide yields , iron(II) chloride, iron(II,III) oxide, 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 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 | 2 | Reducing | Reducing |
| Fe2O3 | Iron(III) oxide | 8 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Oxidized | – | ||
| FeCl2 | Iron(II) chloride | 1 | Reduced | – |
| Fe3O4 | Iron(II,III) oxide | 5 | Reduced | – |
| H2O | Water | 4 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium chloride and iron(III) oxide◆
ΔrG 15.5 kJ/mol K 0.19 × 10−2 pK 2.72
| 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 | 145.4 | 15.5 | 432.8 | 125.1 |
per 1 mol of | 72.70 | 7.75 | 216.4 | 62.55 |
per 1 mol of | 18.18 | 1.94 | 54.10 | 15.64 |
| 145.4 | 15.5 | 432.8 | 125.1 | |
per 1 mol of | 145.4 | 15.5 | 432.8 | 125.1 |
per 1 mol of | 29.08 | 3.10 | 86.56 | 25.02 |
per 1 mol of | 36.35 | 3.88 | 108.2 | 31.27 |
Changes in aqueous solution (1)
- Reaction of ammonium chloride and iron(III) oxide◆
ΔrG 54.0 kJ/mol K 0.35 × 10−9 pK 9.46
| 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 | – | 54.0 | – | – |
per 1 mol of | – | 27.0 | – | – |
per 1 mol of | – | 6.75 | – | – |
| – | 54.0 | – | – | |
per 1 mol of | – | 54.0 | – | – |
per 1 mol of | – | 10.8 | – | – |
per 1 mol of | – | 13.5 | – | – |
Changes in aqueous solution (2)
- Reaction of ammonium chloride and iron(III) oxide◆
ΔrG −8.2 kJ/mol K 2.73 × 101 pK −1.44
| 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 | 34.2 | −8.2 | 139.6 | – |
per 1 mol of | 17.1 | −4.1 | 69.80 | – |
per 1 mol of | 4.28 | −1.0 | 17.45 | – |
| 34.2 | −8.2 | 139.6 | – | |
per 1 mol of | 34.2 | −8.2 | 139.6 | – |
per 1 mol of | 6.84 | −1.6 | 27.92 | – |
per 1 mol of | 8.55 | −2.0 | 34.90 | – |
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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 191.61[1] | 29.125[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] |
| 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] |
* (g):Gas, (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid
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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 191.61 J · K−1 · mol−1
- ^ Cp°, 29.125 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°, -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