MgS + 12Fe2O3 🔥→ MgSO4 + 8Fe3O4
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The reaction of magnesium sulfide and iron(III) oxide yields magnesium sulfate and iron(II,III) 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 | 12 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgSO4 | Magnesium sulfate | 1 | Oxidized | – |
| Fe3O4 | Iron(II,III) oxide | 8 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of magnesium sulfide and iron(III) oxide◆
ΔrG −45.6 kJ/mol K 9.74 × 107 pK −7.99
| 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 | 4.3 | −45.6 | 163.7 | −47.84 |
per 1 mol of | 4.3 | −45.6 | 163.7 | −47.84 |
per 1 mol of | 0.36 | −3.80 | 13.64 | −3.987 |
per 1 mol of | 4.3 | −45.6 | 163.7 | −47.84 |
per 1 mol of | 0.54 | −5.70 | 20.46 | −5.980 |
Changes in aqueous solution (1)
- Reaction of magnesium sulfide and iron(III) oxide◆
ΔrG −74.5 kJ/mol K 1.13 × 1013 pK −13.05
| 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 | −86.9 | −74.5 | −45.9 | – |
per 1 mol of | −86.9 | −74.5 | −45.9 | – |
per 1 mol of | −7.24 | −6.21 | −3.82 | – |
per 1 mol of | −86.9 | −74.5 | −45.9 | – |
per 1 mol of | −10.9 | −9.31 | −5.74 | – |
Changes in aqueous solution (2)
- Reaction of magnesium sulfide and iron(III) oxide◆
ΔrG −87.2 kJ/mol K 1.89 × 1015 pK −15.28
| 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 | −66.8 | −87.2 | 65.0 | – |
per 1 mol of | −66.8 | −87.2 | 65.0 | – |
per 1 mol of | −5.57 | −7.27 | 5.42 | – |
per 1 mol of | −66.8 | −87.2 | 65.0 | – |
per 1 mol of | −8.35 | −10.9 | 8.13 | – |
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 |
|---|---|---|---|---|
| MgSO4 (cr) | -1284.9[1] | -1170.6[1] | 91.6[1] | 96.48[1] |
| MgSO4 (ai) | -1376.12[1] | -1199.5[1] | -118.0[1] | – |
| MgSO4 (ao) | -1356.0[1] | -1212.21[1] | -7.1[1] | – |
| MgSO4 (cr) 1 hydrate | -1602.1[1] | -1428.7[1] | 126.4[1] | – |
| MgSO4 (am) 1 hydrate | -1574.9[1] | -1404.9[1] | 138.1[1] | – |
| MgSO4 (cr) 2 hydrate | -1896.2[1] | – | – | – |
| MgSO4 (cr) 4 hydrate | -2496.6[1] | – | – | – |
| MgSO4 (cr) 6 hydrate | -3087.0[1] | -2631.8[1] | 348.1[1] | 348.11[1] |
| MgSO4 (cr) 7 hydrate | -3388.71[1] | -2871.5[1] | 372[1] | – |
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (am):Amorphous 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°, -1284.9 kJ · mol−1
- ^ ΔfG°, -1170.6 kJ · mol−1
- ^ S°, 91.6 J · K−1 · mol−1
- ^ Cp°, 96.48 J · K−1 · mol−1
- ^ ΔfH°, -1376.12 kJ · mol−1
- ^ ΔfG°, -1199.5 kJ · mol−1
- ^ S°, -118.0 J · K−1 · mol−1
- ^ ΔfH°, -1356.0 kJ · mol−1
- ^ ΔfG°, -1212.21 kJ · mol−1
- ^ S°, -7.1 J · K−1 · mol−1
- ^ ΔfH°, -1602.1 kJ · mol−1
- ^ ΔfG°, -1428.7 kJ · mol−1
- ^ S°, 126.4 J · K−1 · mol−1
- ^ ΔfH°, -1574.9 kJ · mol−1
- ^ ΔfG°, -1404.9 kJ · mol−1
- ^ S°, 138.1 J · K−1 · mol−1
- ^ ΔfH°, -1896.2 kJ · mol−1
- ^ ΔfH°, -2496.6 kJ · mol−1
- ^ ΔfH°, -3087.0 kJ · mol−1
- ^ ΔfG°, -2631.8 kJ · mol−1
- ^ S°, 348.1 J · K−1 · mol−1
- ^ Cp°, 348.11 J · K−1 · mol−1
- ^ ΔfH°, -3388.71 kJ · mol−1
- ^ ΔfG°, -2871.5 kJ · mol−1
- ^ S°, 372. 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