CH4 + 9Fe2O3 🔥→ FeCO3 + 2Fe(OH)2 + 5Fe3O4
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- Reaction of and iron(III) oxide
The reaction of and iron(III) oxide yields iron(II) carbonate, iron(II) hydroxide, 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 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 and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Reducing | Reducing | ||
| Fe2O3 | Iron(III) oxide | 9 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeCO3 | Iron(II) carbonate | 1 | Redoxed product | – |
| Fe(OH)2 | Iron(II) hydroxide | 2 | Reduced | – |
| Fe3O4 | Iron(II,III) oxide | 5 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and iron(III) oxide◆
ΔrG 13.9 kJ/mol K 0.37 × 10−2 pK 2.44
| 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 | 22.0 | 13.9 | 28 | – |
| 22.0 | 13.9 | 28 | – | |
per 1 mol of | 2.44 | 1.54 | 3.1 | – |
per 1 mol of | 22.0 | 13.9 | 28 | – |
per 1 mol of | 11.0 | 6.95 | 14 | – |
per 1 mol of | 4.40 | 2.78 | 5.6 | – |
Changes in aqueous solution
- Reaction of and iron(III) oxide◆
ΔrG −2.5 kJ/mol K 2.74 × 100 pK −0.44
| 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 | 36.3 | −2.5 | 131 | – |
| 36.3 | −2.5 | 131 | – | |
per 1 mol of | 4.03 | −0.28 | 14.6 | – |
per 1 mol of | 36.3 | −2.5 | 131 | – |
per 1 mol of | 18.1 | −1.3 | 65.5 | – |
per 1 mol of | 7.26 | −0.50 | 26.2 | – |
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 |
|---|---|---|---|---|
| (g) | -74.81[1] | -50.72[1] | 186.264[1] | 35.309[1] |
| (ao) | -89.04[1] | -34.33[1] | 83.7[1] | – |
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
* (g):Gas, (ao):Un-ionized aqueous solution, (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 |
|---|---|---|---|---|
| FeCO3 (cr) siderite | -740.57[1] | -666.67[1] | 92.9[1] | 82.13[1] |
| Fe(OH)2 (cr) precipitated | -569.0[1] | -486.5[1] | 88[1] | – |
| Fe(OH)2 (g) | -372[1] | – | – | – |
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
* (cr):Crystalline solid, (g):Gas
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°, -74.81 kJ · mol−1
- ^ ΔfG°, -50.72 kJ · mol−1
- ^ S°, 186.264 J · K−1 · mol−1
- ^ Cp°, 35.309 J · K−1 · mol−1
- ^ ΔfH°, -89.04 kJ · mol−1
- ^ ΔfG°, -34.33 kJ · mol−1
- ^ S°, 83.7 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°, -740.57 kJ · mol−1
- ^ ΔfG°, -666.67 kJ · mol−1
- ^ S°, 92.9 J · K−1 · mol−1
- ^ Cp°, 82.13 J · K−1 · mol−1
- ^ 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°, -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