6NH4Cl + 58Fe2O3 🔥→ 6NO↑ + 3Cl2↑ + 36Fe3O4 + 8Fe(OH)3
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- Reaction of ammonium chloride and iron(III) oxide
The reaction of ammonium chloride and iron(III) oxide yields nitrogen monoxide, , 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 | 58 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NO | Nitrogen monoxide | 6 | Oxidized | – |
| 3 | Oxidized | – | ||
| Fe3O4 | Iron(II,III) oxide | 36 | Reduced | – |
| Fe(OH)3 | Iron(III) hydroxide | 8 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium chloride and iron(III) oxide◆
ΔrG 2657.7 kJ/mol K 0.25 × 10−465 pK 465.61
| 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 | 3385.3 | 2657.7 | 2421.0 | – |
per 1 mol of | 564.22 | 442.95 | 403.50 | – |
per 1 mol of | 58.367 | 45.822 | 41.741 | – |
per 1 mol of | 564.22 | 442.95 | 403.50 | – |
| 1128.4 | 885.90 | 807.00 | – | |
per 1 mol of | 94.036 | 73.825 | 67.250 | – |
per 1 mol of | 423.16 | 332.21 | 302.63 | – |
Changes in aqueous solution (1)
- Reaction of ammonium chloride and iron(III) oxide◆
ΔrG 3001.2 kJ/mol K 0.16 × 10−525 pK 525.79
| 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 | – | 3001.2 | – | – |
per 1 mol of | – | 500.20 | – | – |
per 1 mol of | – | 51.745 | – | – |
per 1 mol of | – | 500.20 | – | – |
| – | 1000.4 | – | – | |
per 1 mol of | – | 83.367 | – | – |
per 1 mol of | – | 375.15 | – | – |
Changes in aqueous solution (2)
- Reaction of ammonium chloride and iron(III) oxide◆
ΔrG 3022.0 kJ/mol K 0.37 × 10−529 pK 529.43
| 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 | – | 3022.0 | – | – |
per 1 mol of | – | 503.67 | – | – |
per 1 mol of | – | 52.103 | – | – |
per 1 mol of | – | 503.67 | – | – |
| – | 1007.3 | – | – | |
per 1 mol of | – | 83.944 | – | – |
per 1 mol of | – | 377.75 | – | – |
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] |
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[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, (ao):Un-ionized aqueous solution, (cr):Crystalline solid
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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. J · K−1 · 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