2Fe + 3CO2 → 2FeCO3 + C
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- Reaction of and carbon dioxide
The reaction of and carbon dioxide yields iron(II) carbonate and (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 carbon dioxide
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 carbon dioxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
2 | Reducing | Reducing | ||
CO2 | Carbon dioxide | 3 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
FeCO3 | Iron(II) carbonate | 2 | Oxidized | – |
1 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and carbon dioxide◆
ΔrG −150.26 kJ/mol K 2.11 × 1026 pK −26.32
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 | −300.61 | −150.26 | −504.2 | 11.26 |
−150.31 | −75.130 | −252.1 | 5.630 | |
per 1 mol of | −100.20 | −50.087 | −168.1 | 3.753 |
per 1 mol of | −150.31 | −75.130 | −252.1 | 5.630 |
−300.61 | −150.26 | −504.2 | 11.26 |
Changes in standard condition (2)
- Reaction of and carbon dioxide◆
ΔrG −147.36 kJ/mol K 6.55 × 1025 pK −25.82
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 | −298.72 | −147.36 | −507.6 | 8.84 |
−149.36 | −73.680 | −253.8 | 4.42 | |
per 1 mol of | −99.573 | −49.120 | −169.2 | 2.95 |
per 1 mol of | −149.36 | −73.680 | −253.8 | 4.42 |
−298.72 | −147.36 | −507.6 | 8.84 |
Changes in aqueous solution
- Reaction of and carbon dioxide◆
ΔrG −175.40 kJ/mol K 5.35 × 1030 pK −30.73
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 | −239.74 | −175.40 | −215.8 | – |
−119.87 | −87.700 | −107.9 | – | |
per 1 mol of | −79.913 | −58.467 | −71.93 | – |
per 1 mol of | −119.87 | −87.700 | −107.9 | – |
−239.74 | −175.40 | −215.8 | – |
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) | 0[1] | 0[1] | 27.28[1] | 25.10[1] |
(g) | 416.3[1] | 370.7[1] | 180.490[1] | 25.677[1] |
CO2 (g) | -393.509[1] | -394.359[1] | 213.74[1] | 37.11[1] |
CO2 (ao) | -413.80[1] | -385.98[1] | 117.6[1] | – |
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution
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] |
(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] |
* (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°, 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°, -393.509 kJ · mol−1
- ^ ΔfG°, -394.359 kJ · mol−1
- ^ S°, 213.74 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -413.80 kJ · mol−1
- ^ ΔfG°, -385.98 kJ · mol−1
- ^ S°, 117.6 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°, 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