3FeCO3 🔥→ Fe3O4 + O2↑ + 3CO↑
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- Decomposition of iron(II) carbonate
Decomposition of iron(II) carbonate yields iron(II,III) oxide, , 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
- Decomposition of iron(II) carbonate
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
- Thermal decomposition of oxoacid salt with redox
- Oxoacid saltSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of iron(II) carbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeCO3 | Iron(II) carbonate | 3 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe3O4 | Iron(II,III) oxide | 1 | Oxidized | – |
| 1 | Oxidized | – | ||
| CO | Carbon monoxide | 3 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Decomposition of iron(II) carbonate◆
ΔrG 573.1 kJ/mol K 0.40 × 10−100 pK 100.40
| 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 | 771.7 | 573.1 | 665.9 | 13.82 |
per 1 mol of | 257.2 | 191.0 | 222.0 | 4.607 |
per 1 mol of | 771.7 | 573.1 | 665.9 | 13.82 |
| 771.7 | 573.1 | 665.9 | 13.82 | |
per 1 mol of | 257.2 | 191.0 | 222.0 | 4.607 |
Changes in aqueous solution (1)
- Decomposition of iron(II) carbonate◆
ΔrG 573.1 kJ/mol K 0.40 × 10−100 pK 100.40
| 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 | 771.7 | 573.1 | 665.9 | 13.82 |
per 1 mol of | 257.2 | 191.0 | 222.0 | 4.607 |
per 1 mol of | 771.7 | 573.1 | 665.9 | 13.82 |
| 771.7 | 573.1 | 665.9 | 13.82 | |
per 1 mol of | 257.2 | 191.0 | 222.0 | 4.607 |
Changes in aqueous solution (2)
- Decomposition of iron(II) carbonate◆
ΔrG 624.9 kJ/mol K 0.33 × 10−109 pK 109.48
| 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 | 740.4 | 624.9 | 386.6 | – |
per 1 mol of | 246.8 | 208.3 | 128.9 | – |
per 1 mol of | 740.4 | 624.9 | 386.6 | – |
| 740.4 | 624.9 | 386.6 | – | |
per 1 mol of | 246.8 | 208.3 | 128.9 | – |
Changes in aqueous solution (3)
- Decomposition of iron(II) carbonate◆
ΔrG 589.5 kJ/mol K 0.53 × 10−103 pK 103.28
| 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 | 760.0 | 589.5 | 571.6 | – |
per 1 mol of | 253.3 | 196.5 | 190.5 | – |
per 1 mol of | 760.0 | 589.5 | 571.6 | – |
| 760.0 | 589.5 | 571.6 | – | |
per 1 mol of | 253.3 | 196.5 | 190.5 | – |
Changes in aqueous solution (4)
- Decomposition of iron(II) carbonate◆
ΔrG 641.3 kJ/mol K 0.45 × 10−112 pK 112.35
| 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 | 728.7 | 641.3 | 292.4 | – |
per 1 mol of | 242.9 | 213.8 | 97.47 | – |
per 1 mol of | 728.7 | 641.3 | 292.4 | – |
| 728.7 | 641.3 | 292.4 | – | |
per 1 mol of | 242.9 | 213.8 | 97.47 | – |
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 |
|---|---|---|---|---|
| FeCO3 (cr) siderite | -740.57[1] | -666.67[1] | 92.9[1] | 82.13[1] |
* (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] |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[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°, -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°, -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°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 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