4C + Fe3O4 🔥→ 3Fe + 4CO↑
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- Reaction of and iron(II,III) oxide
The reaction of and iron(II,III) oxide yields and carbon monoxide (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(II,III) oxide
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
- Reducing agent + OxideOxidizing agent🔥⟶ Elementary substance/OxideReduction product + Oxidation product
Oxidation state of each atom
- Reaction of and iron(II,III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 4 | Reducing | Reducing Reducing nonmetal | ||
| Fe3O4 | Iron(II,III) oxide | 1 | Oxidizing | Reducible Oxide |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 3 | Reduced | – Elementary substance | ||
| CO | Carbon monoxide | 4 | Oxidized | – Oxide |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and iron(II,III) oxide◆
ΔrG 466.7 kJ/mol K 0.17 × 10−81 pK 81.76
| 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 | 676.3 | 466.7 | 703.2 | 14.33 |
| 169.1 | 116.7 | 175.8 | 3.583 | |
per 1 mol of | 676.3 | 466.7 | 703.2 | 14.33 |
| 225.4 | 155.6 | 234.4 | 4.777 | |
per 1 mol of | 169.1 | 116.7 | 175.8 | 3.583 |
Changes in standard condition (2)
- Reaction of and iron(II,III) oxide◆
ΔrG 455.1 kJ/mol K 0.19 × 10−79 pK 79.73
| 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 | 668.7 | 455.1 | 716.6 | 23.99 |
| 167.2 | 113.8 | 179.2 | 5.997 | |
per 1 mol of | 668.7 | 455.1 | 716.6 | 23.99 |
| 222.9 | 151.7 | 238.9 | 7.997 | |
per 1 mol of | 167.2 | 113.8 | 179.2 | 5.997 |
Changes in aqueous solution (1)
- Reaction of and iron(II,III) oxide◆
ΔrG 466.7 kJ/mol K 0.17 × 10−81 pK 81.76
| 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 | 676.3 | 466.7 | 703.2 | 14.33 |
| 169.1 | 116.7 | 175.8 | 3.583 | |
per 1 mol of | 676.3 | 466.7 | 703.2 | 14.33 |
| 225.4 | 155.6 | 234.4 | 4.777 | |
per 1 mol of | 169.1 | 116.7 | 175.8 | 3.583 |
Changes in aqueous solution (2)
- Reaction of and iron(II,III) oxide◆
ΔrG 535.8 kJ/mol K 0.14 × 10−93 pK 93.87
| 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 | 634.6 | 535.8 | 330.9 | – |
| 158.7 | 133.9 | 82.72 | – | |
per 1 mol of | 634.6 | 535.8 | 330.9 | – |
| 211.5 | 178.6 | 110.3 | – | |
per 1 mol of | 158.7 | 133.9 | 82.72 | – |
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 |
|---|---|---|---|---|
| (cr) graphite | 0[1] | 0[1] | 5.740[1] | 8.527[1] |
| (cr) diamond | 1.895[1] | 2.900[1] | 2.377[1] | 6.113[1] |
| (g) | 716.682[1] | 671.257[1] | 158.096[1] | 20.838[1] |
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
* (cr):Crystalline solid, (g):Gas
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 27.28[1] | 25.10[1] |
| (g) | 416.3[1] | 370.7[1] | 180.490[1] | 25.677[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] | – |
* (cr):Crystalline solid, (g):Gas, (ao):Un-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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 5.740 J · K−1 · mol−1
- ^ Cp°, 8.527 J · K−1 · mol−1
- ^ ΔfH°, 1.895 kJ · mol−1
- ^ ΔfG°, 2.900 kJ · mol−1
- ^ S°, 2.377 J · K−1 · mol−1
- ^ Cp°, 6.113 J · K−1 · mol−1
- ^ ΔfH°, 716.682 kJ · mol−1
- ^ ΔfG°, 671.257 kJ · mol−1
- ^ S°, 158.096 J · K−1 · mol−1
- ^ Cp°, 20.838 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 27.28 J · K−1 · mol−1
- ^ Cp°, 25.10 J · K−1 · mol−1
- ^ ΔfH°, 416.3 kJ · mol−1
- ^ ΔfG°, 370.7 kJ · mol−1
- ^ S°, 180.490 J · K−1 · mol−1
- ^ Cp°, 25.677 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