3(NH4)2SO3 + 59Fe2O3 🔥→ 6NO↑ + Fe2(SO4)3 + 36Fe3O4 + 8Fe(OH)3
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The reaction of ammonium sulfite and iron(III) oxide yields nitrogen monoxide, iron(III) sulfate, 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 sulfite 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 sulfite and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| (NH4)2SO3 | Ammonium sulfite | 3 | Reducing | Reducing |
| Fe2O3 | Iron(III) oxide | 59 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NO | Nitrogen monoxide | 6 | Oxidized | – |
| Fe2(SO4)3 | Iron(III) sulfate | 1 | Oxidized | – |
| Fe3O4 | Iron(II,III) oxide | 36 | Reduced | – |
| Fe(OH)3 | Iron(III) hydroxide | 8 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium sulfite 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 | 2397.3 | – | – | – |
per 1 mol of | 799.10 | – | – | – |
per 1 mol of | 40.632 | – | – | – |
per 1 mol of | 399.55 | – | – | – |
per 1 mol of | 2397.3 | – | – | – |
per 1 mol of | 66.592 | – | – | – |
per 1 mol of | 299.66 | – | – | – |
Changes in aqueous solution
- Reaction of ammonium sulfite and iron(III) oxide◆
ΔrG 2172.5 kJ/mol K 0.25 × 10−380 pK 380.61
| 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 | – | 2172.5 | – | – |
per 1 mol of | – | 724.17 | – | – |
per 1 mol of | – | 36.822 | – | – |
per 1 mol of | – | 362.08 | – | – |
per 1 mol of | – | 2172.5 | – | – |
per 1 mol of | – | 60.347 | – | – |
per 1 mol of | – | 271.56 | – | – |
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 |
|---|---|---|---|---|
| (NH4)2SO3 (cr) | -885.3[1] | – | – | – |
| (NH4)2SO3 (ai) | -900.4[1] | -645.0[1] | 197.5[1] | – |
| (NH4)2SO3 (cr) 1 hydrate | -1187.4[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] |
| Fe2(SO4)3 (cr) | -2581.5[1] | – | – | – |
| Fe2(SO4)3 (ai) | -2825.0[1] | -2242.8[1] | -571.5[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°, -885.3 kJ · mol−1
- ^ ΔfH°, -900.4 kJ · mol−1
- ^ ΔfG°, -645.0 kJ · mol−1
- ^ S°, 197.5 J · K−1 · mol−1
- ^ ΔfH°, -1187.4 kJ · 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°, -2581.5 kJ · mol−1
- ^ ΔfH°, -2825.0 kJ · mol−1
- ^ ΔfG°, -2242.8 kJ · mol−1
- ^ S°, -571.5 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