MgS + 3Fe2O3 → MgSO3 + 6FeO
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The reaction of magnesium sulfide and iron(III) oxide yields magnesium sulfite and iron(II) oxide (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 magnesium sulfide 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 magnesium sulfide and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgS | Magnesium sulfide | 1 | Reducing | Reducing |
| Fe2O3 | Iron(III) oxide | 3 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgSO3 | Magnesium sulfite | 1 | Oxidized | – |
| FeO | Iron(II) oxide | 6 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of magnesium sulfide 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 | 178.3 | – | – | – |
per 1 mol of | 178.3 | – | – | – |
per 1 mol of | 59.43 | – | – | – |
per 1 mol of | 178.3 | – | – | – |
per 1 mol of | 29.72 | – | – | – |
Changes in aqueous solution
- Reaction of magnesium sulfide 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 | 178.3 | – | – | – |
per 1 mol of | 178.3 | – | – | – |
per 1 mol of | 59.43 | – | – | – |
per 1 mol of | 178.3 | – | – | – |
per 1 mol of | 29.72 | – | – | – |
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 |
|---|---|---|---|---|
| MgS (cr) | -346.0[1] | -341.8[1] | 50.33[1] | 45.56[1] |
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
* (cr):Crystalline solid
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 |
|---|---|---|---|---|
| MgSO3 (cr) | -1008.3[1] | -923.8[1] | 87.9[1] | – |
| MgSO3 (cr) 3 hydrate | -1931.8[1] | -1674.7[1] | 209.2[1] | – |
| MgSO3 (cr) 6 hydrate | -2817.5[1] | -2385.4[1] | 322.2[1] | – |
| FeO (cr) | -272.0[1] | – | – | – |
* (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°, -346.0 kJ · mol−1
- ^ ΔfG°, -341.8 kJ · mol−1
- ^ S°, 50.33 J · K−1 · mol−1
- ^ Cp°, 45.56 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°, -1008.3 kJ · mol−1
- ^ ΔfG°, -923.8 kJ · mol−1
- ^ S°, 87.9 J · K−1 · mol−1
- ^ ΔfH°, -1931.8 kJ · mol−1
- ^ ΔfG°, -1674.7 kJ · mol−1
- ^ S°, 209.2 J · K−1 · mol−1
- ^ ΔfH°, -2817.5 kJ · mol−1
- ^ ΔfG°, -2385.4 kJ · mol−1
- ^ S°, 322.2 J · K−1 · mol−1
- ^ ΔfH°, -272.0 kJ · mol−1