CH4 + 9Fe2O3 🔥→ 6Fe3O4 + CO + 2H2O
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- Reaction of and iron(III) oxide
The reaction of and iron(III) oxide yields iron(II,III) oxide, carbon monoxide, 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 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 |
|---|---|---|---|---|
| Fe3O4 | Iron(II,III) oxide | 6 | Reduced | – |
| CO | Carbon monoxide | 1 | Oxidized | – |
| H2O | Water | 2 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and iron(III) oxide◆
ΔrG 26.7 kJ/mol K 0.21 × 10−4 pK 4.68
| 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 | 100.0 | 26.7 | 243.0 | 70.35 |
| 100.0 | 26.7 | 243.0 | 70.35 | |
per 1 mol of | 11.11 | 2.97 | 27.00 | 7.817 |
per 1 mol of | 16.67 | 4.45 | 40.50 | 11.72 |
per 1 mol of | 100.0 | 26.7 | 243.0 | 70.35 |
per 1 mol of | 50.00 | 13.3 | 121.5 | 35.17 |
Changes in aqueous solution (1)
- Reaction of and iron(III) oxide◆
ΔrG 10.3 kJ/mol K 0.16 × 10−1 pK 1.80
| 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 | 114.3 | 10.3 | 345.6 | – |
| 114.3 | 10.3 | 345.6 | – | |
per 1 mol of | 12.70 | 1.14 | 38.40 | – |
per 1 mol of | 19.05 | 1.72 | 57.60 | – |
per 1 mol of | 114.3 | 10.3 | 345.6 | – |
per 1 mol of | 57.15 | 5.15 | 172.8 | – |
Changes in aqueous solution (2)
- Reaction of and iron(III) oxide◆
ΔrG 27.6 kJ/mol K 0.15 × 10−4 pK 4.84
| 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 | 103.8 | 27.6 | 252.5 | – |
| 103.8 | 27.6 | 252.5 | – | |
per 1 mol of | 11.53 | 3.07 | 28.06 | – |
per 1 mol of | 17.30 | 4.60 | 42.08 | – |
per 1 mol of | 103.8 | 27.6 | 252.5 | – |
per 1 mol of | 51.90 | 13.8 | 126.3 | – |
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 |
|---|---|---|---|---|
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
| CO (g) | -110.525[1] | -137.168[1] | 197.674[1] | 29.142[1] |
| CO (ao) | -120.96[1] | -119.90[1] | 104.6[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, (ao):Un-ionized aqueous solution, (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°, -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°, -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°, -110.525 kJ · mol−1
- ^ ΔfG°, -137.168 kJ · mol−1
- ^ S°, 197.674 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -120.96 kJ · mol−1
- ^ ΔfG°, -119.90 kJ · mol−1
- ^ S°, 104.6 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