3(NH4)2SO3 + 5Fe2O3 🔥→ 3N2↑ + Fe2(SO4)3 + 8Fe + 12H2O
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- Reaction of ammonium sulfite and iron(III) oxide
- 3(NH4)2SO3Ammonium sulfite + 5Fe2O3Iron(III) oxide3↑ + Fe2(SO4)3Iron(III) sulfate + 8 + 12H2OWater🔥⟶
The reaction of ammonium sulfite and iron(III) oxide yields , iron(III) sulfate, , 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 sulfite and iron(III) oxide
- 3(NH4)2SO3Ammonium sulfite + 5Fe2O3Iron(III) oxide3↑ + Fe2(SO4)3Iron(III) sulfate + 8 + 12H2OWater🔥⟶
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 | 5 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 3 | Oxidized | – | ||
| Fe2(SO4)3 | Iron(III) sulfate | 1 | Oxidized | – |
| 8 | Reduced | – | ||
| H2O | Water | 12 | – | – |
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 | 765.4 | – | – | – |
per 1 mol of | 255.1 | – | – | – |
per 1 mol of | 153.1 | – | – | – |
| 255.1 | – | – | – | |
per 1 mol of | 765.4 | – | – | – |
| 95.67 | – | – | – | |
per 1 mol of | 63.78 | – | – | – |
Changes in aqueous solution
- Reaction of ammonium sulfite and iron(III) oxide◆
ΔrG 557.7 kJ/mol K 0.20 × 10−97 pK 97.70
| 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 | 567.2 | 557.7 | 31.0 | – |
per 1 mol of | 189.1 | 185.9 | 10.3 | – |
per 1 mol of | 113.4 | 111.5 | 6.20 | – |
| 189.1 | 185.9 | 10.3 | – | |
per 1 mol of | 567.2 | 557.7 | 31.0 | – |
| 70.90 | 69.71 | 3.88 | – | |
per 1 mol of | 47.27 | 46.48 | 2.58 | – |
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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 191.61[1] | 29.125[1] |
| Fe2(SO4)3 (cr) | -2581.5[1] | – | – | – |
| Fe2(SO4)3 (ai) | -2825.0[1] | -2242.8[1] | -571.5[1] | – |
| (cr) | 0[1] | 0[1] | 27.28[1] | 25.10[1] |
| (g) | 416.3[1] | 370.7[1] | 180.490[1] | 25.677[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, (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°, -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°, 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°, -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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 27.28 J · K−1 · mol−1
- ^ Cp°, 25.10 J · K−1 · mol−1
- ^ ΔfH°, 416.3 kJ · mol−1
- ^ ΔfG°, 370.7 kJ · mol−1
- ^ S°, 180.490 J · K−1 · mol−1
- ^ Cp°, 25.677 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