4Fe(OH)2 + MnO2 🔥→ 2Fe2O3 + Mn + 4H2O
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- Reaction of iron(II) hydroxide and manganese(IV) oxide
The reaction of iron(II) hydroxide and manganese(IV) oxide yields iron(III) oxide, , 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 iron(II) hydroxide and manganese(IV) oxide
General equation
- Reaction of oxidizable species and reducible species
- Oxidizable speciesReducing agent + Reducible speciesOxidizing agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of iron(II) hydroxide and manganese(IV) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe(OH)2 | Iron(II) hydroxide | 4 | Reducing | Oxidizable |
| MnO2 | Manganese(IV) oxide | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe2O3 | Iron(III) oxide | 2 | Oxidized | – |
| 1 | Reduced | – | ||
| H2O | Water | 4 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(II) hydroxide and manganese(IV) oxide◆
ΔrG −21.8 kJ/mol K 6.59 × 103 pK −3.82
| 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 | −21.8 | 81 | – |
per 1 mol of | 1.1 | −5.45 | 20 | – |
per 1 mol of | 4.3 | −21.8 | 81 | – |
per 1 mol of | 2.1 | −10.9 | 41 | – |
| 4.3 | −21.8 | 81 | – | |
per 1 mol of | 1.1 | −5.45 | 20 | – |
Changes in standard condition (2)
- Reaction of iron(II) hydroxide 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 | – | – | 84 | – |
per 1 mol of | – | – | 21 | – |
per 1 mol of | – | – | 84 | – |
per 1 mol of | – | – | 42 | – |
| – | – | 84 | – | |
per 1 mol of | – | – | 21 | – |
Changes in standard condition (3)
- Reaction of iron(II) hydroxide and manganese(IV) oxide◆
ΔrG −20.4 kJ/mol K 3.75 × 103 pK −3.57
| 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 | 5.9 | −20.4 | 82 | – |
per 1 mol of | 1.5 | −5.10 | 21 | – |
per 1 mol of | 5.9 | −20.4 | 82 | – |
per 1 mol of | 3.0 | −10.2 | 41 | – |
| 5.9 | −20.4 | 82 | – | |
per 1 mol of | 1.5 | −5.10 | 21 | – |
Changes in standard condition (4)
- Reaction of iron(II) hydroxide 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 | −13.2 | – | – | – |
per 1 mol of | −3.30 | – | – | – |
per 1 mol of | −13.2 | – | – | – |
per 1 mol of | −6.60 | – | – | – |
| −13.2 | – | – | – | |
per 1 mol of | −3.30 | – | – | – |
Changes in standard condition (5)
- Reaction of iron(II) hydroxide 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
Changes in standard condition (6)
- Reaction of iron(II) hydroxide 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 | −11.7 | – | – | – |
per 1 mol of | −2.92 | – | – | – |
per 1 mol of | −11.7 | – | – | – |
per 1 mol of | −5.85 | – | – | – |
| −11.7 | – | – | – | |
per 1 mol of | −2.92 | – | – | – |
Changes in aqueous solution
- Reaction of iron(II) hydroxide and manganese(IV) oxide◆
ΔrG −21.8 kJ/mol K 6.59 × 103 pK −3.82
| 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 | −21.8 | 81 | – |
per 1 mol of | 1.1 | −5.45 | 20 | – |
per 1 mol of | 4.3 | −21.8 | 81 | – |
per 1 mol of | 2.1 | −10.9 | 41 | – |
| 4.3 | −21.8 | 81 | – | |
per 1 mol of | 1.1 | −5.45 | 20 | – |
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 |
|---|---|---|---|---|
| Fe(OH)2 (cr) precipitated | -569.0[1] | -486.5[1] | 88[1] | – |
| Fe(OH)2 (g) | -372[1] | – | – | – |
| MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
| MnO2 (am) precipitated | -502.5[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (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 |
|---|---|---|---|---|
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
| (cr) α | 0[1] | 0[1] | 32.01[1] | 26.32[1] |
| (cr) β | – | – | 34.39[1] | 26.53[1] |
| (cr) γ | 1.55[1] | 1.42[1] | 32.43[1] | 27.57[1] |
| (g) | 280.7[1] | 238.5[1] | 173.70[1] | 20.79[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] |
* (cr):Crystalline solid, (g):Gas, (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°, -569.0 kJ · mol−1
- ^ ΔfG°, -486.5 kJ · mol−1
- ^ S°, 88. J · K−1 · mol−1
- ^ ΔfH°, -372. kJ · 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°, -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°, 32.01 J · K−1 · mol−1
- ^ Cp°, 26.32 J · K−1 · mol−1
- ^ S°, 34.39 J · K−1 · mol−1
- ^ Cp°, 26.53 J · K−1 · mol−1
- ^ ΔfH°, 1.55 kJ · mol−1
- ^ ΔfG°, 1.42 kJ · mol−1
- ^ S°, 32.43 J · K−1 · mol−1
- ^ Cp°, 27.57 J · K−1 · mol−1
- ^ ΔfH°, 280.7 kJ · mol−1
- ^ ΔfG°, 238.5 kJ · mol−1
- ^ S°, 173.70 J · K−1 · mol−1
- ^ Cp°, 20.79 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