9FeO + ZnCO3 🔥→ 3Fe3O4 + Zn + C
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- Reaction of iron(II) oxide and zinc carbonate
The reaction of iron(II) oxide and zinc carbonate yields iron(II,III) oxide, , 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 iron(II) oxide and zinc carbonate
General equation
- Reaction of oxidizable species and reducible species
- Oxidizable speciesReducing agent + Reducible speciesOxidizing agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of iron(II) oxide and zinc carbonate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
FeO | Iron(II) oxide | 9 | Reducing | Oxidizable |
ZnCO3 | Zinc carbonate | 1 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Fe3O4 | Iron(II,III) oxide | 3 | Oxidized | – |
1 | Reduced | – | ||
1 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(II) oxide and zinc carbonate
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 | −94.4 | – | – | – |
per 1 mol of | −10.5 | – | – | – |
per 1 mol of | −94.4 | – | – | – |
per 1 mol of | −31.5 | – | – | – |
−94.4 | – | – | – | |
−94.4 | – | – | – |
Changes in standard condition (2)
- Reaction of iron(II) oxide and zinc carbonate
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 | −92.5 | – | – | – |
per 1 mol of | −10.3 | – | – | – |
per 1 mol of | −92.5 | – | – | – |
per 1 mol of | −30.8 | – | – | – |
−92.5 | – | – | – | |
−92.5 | – | – | – |
Changes in aqueous solution
- Reaction of iron(II) oxide and zinc carbonate
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 | −94.4 | – | – | – |
per 1 mol of | −10.5 | – | – | – |
per 1 mol of | −94.4 | – | – | – |
per 1 mol of | −31.5 | – | – | – |
−94.4 | – | – | – | |
−94.4 | – | – | – |
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 |
---|---|---|---|---|
FeO (cr) | -272.0[1] | – | – | – |
ZnCO3 (cr) | -812.78[1] | -731.52[1] | 82.4[1] | 79.71[1] |
ZnCO3 (cr) 1 hydrate | – | -970.6[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] |
(cr) | 0[1] | 0[1] | 41.63[1] | 25.40[1] |
(g) | 130.729[1] | 95.145[1] | 160.984[1] | 20.786[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°, -272.0 kJ · mol−1
- ^ ΔfH°, -812.78 kJ · mol−1
- ^ ΔfG°, -731.52 kJ · mol−1
- ^ S°, 82.4 J · K−1 · mol−1
- ^ Cp°, 79.71 J · K−1 · mol−1
- ^ ΔfG°, -970.6 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
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 41.63 J · K−1 · mol−1
- ^ Cp°, 25.40 J · K−1 · mol−1
- ^ ΔfH°, 130.729 kJ · mol−1
- ^ ΔfG°, 95.145 kJ · mol−1
- ^ S°, 160.984 J · K−1 · mol−1
- ^ Cp°, 20.786 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