9FeS + 80MnO2 → 3Fe2(SO4)3 + Fe3O4 + 40Mn2O3
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The reaction of iron(II) sulfide and manganese(IV) oxide yields iron(III) sulfate, iron(II,III) oxide, and manganese(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 iron(II) sulfide and manganese(IV) 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 iron(II) sulfide and manganese(IV) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeS | Iron(II) sulfide | 9 | Reducing | Reducing |
| MnO2 | Manganese(IV) oxide | 80 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe2(SO4)3 | Iron(III) sulfate | 3 | Oxidized | – |
| Fe3O4 | Iron(II,III) oxide | 1 | Oxidized | – |
| Mn2O3 | Manganese(III) oxide | 40 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(II) sulfide and manganese(IV) 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 | −4720.5 | – | – | – |
per 1 mol of | −524.50 | – | – | – |
per 1 mol of | −59.006 | – | – | – |
per 1 mol of | −1573.5 | – | – | – |
per 1 mol of | −4720.5 | – | – | – |
per 1 mol of | −118.01 | – | – | – |
Changes in standard condition (2)
- Reaction of iron(II) sulfide and manganese(IV) 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 | −6122.9 | – | – | – |
per 1 mol of | −680.32 | – | – | – |
per 1 mol of | −76.536 | – | – | – |
per 1 mol of | −2041.0 | – | – | – |
per 1 mol of | −6122.9 | – | – | – |
per 1 mol of | −153.07 | – | – | – |
Changes in aqueous solution
- Reaction of iron(II) sulfide and manganese(IV) oxide◆
ΔrG −4873.0 kJ/mol K 5.16 × 10853 pK −853.71
| 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 | −5451.0 | −4873.0 | −1934.7 | – |
per 1 mol of | −605.67 | −541.44 | −214.97 | – |
per 1 mol of | −68.138 | −60.913 | −24.184 | – |
per 1 mol of | −1817.0 | −1624.3 | −644.90 | – |
per 1 mol of | −5451.0 | −4873.0 | −1934.7 | – |
per 1 mol of | −136.28 | −121.83 | −48.367 | – |
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 |
|---|---|---|---|---|
| FeS (cr) iron-rich pyrrhotite, α | -100.0[1] | -100.4[1] | 60.29[1] | 50.54[1] |
| MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
| MnO2 (am) precipitated | -502.5[1] | – | – | – |
* (cr):Crystalline solid, (am):Amorphous 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 |
|---|---|---|---|---|
| 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] |
| Mn2O3 (cr) | -959.0[1] | -881.1[1] | 110.5[1] | 107.65[1] |
* (cr):Crystalline solid, (ai):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°, -100.0 kJ · mol−1
- ^ ΔfG°, -100.4 kJ · mol−1
- ^ S°, 60.29 J · K−1 · mol−1
- ^ Cp°, 50.54 J · K−1 · mol−1
- ^ ΔfH°, -520.03 kJ · mol−1
- ^ ΔfG°, -465.14 kJ · mol−1
- ^ S°, 53.05 J · K−1 · mol−1
- ^ Cp°, 54.14 J · K−1 · mol−1
- ^ ΔfH°, -502.5 kJ · 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°, -959.0 kJ · mol−1
- ^ ΔfG°, -881.1 kJ · mol−1
- ^ S°, 110.5 J · K−1 · mol−1
- ^ Cp°, 107.65 J · K−1 · mol−1