2Cu + FeSO4 🔥→ Cu2SO3 + FeO
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- Reaction of and iron(II) sulfate
The reaction of and iron(II) sulfate yields copper(I) sulfite and iron(II) oxide (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) sulfate
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 and iron(II) sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 2 | Reducing | Oxidizable | ||
| FeSO4 | Iron(II) sulfate | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cu2SO3 | Copper(I) sulfite | 1 | Redoxed product | – |
| FeO | Iron(II) oxide | 1 | – | – |
Thermodynamic changes
Changes in aqueous solution
- Reaction of and iron(II) sulfate
| 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 | 164.4 | – | – | – |
| 82.20 | – | – | – | |
per 1 mol of | 164.4 | – | – | – |
per 1 mol of | 164.4 | – | – | – |
per 1 mol of | 164.4 | – | – | – |
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 33.150[1] | 24.435[1] |
| (g) | 338.32[1] | 298.58[1] | 166.38[1] | 20.786[1] |
| FeSO4 (cr) | -928.4[1] | -820.8[1] | 107.5[1] | 100.58[1] |
| FeSO4 (ai) | -998.3[1] | -823.43[1] | -117.6[1] | – |
| FeSO4 (cr) 1 hydrate | -1243.69[1] | – | – | – |
| FeSO4 (cr) 4 hydrate | -2129.2[1] | – | – | – |
| FeSO4 (cr) 7 hydrate | -3014.57[1] | -2509.87[1] | 409.2[1] | 394.47[1] |
* (cr):Crystalline solid, (g):Gas, (ai):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 |
|---|---|---|---|---|
| Cu2SO3 (ai) | -492.0[1] | -386.6[1] | 50[1] | – |
| FeO (cr) | -272.0[1] | – | – | – |
* (ai):Ionized aqueous solution, (cr):Crystalline solid
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°, 33.150 J · K−1 · mol−1
- ^ Cp°, 24.435 J · K−1 · mol−1
- ^ ΔfH°, 338.32 kJ · mol−1
- ^ ΔfG°, 298.58 kJ · mol−1
- ^ S°, 166.38 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -928.4 kJ · mol−1
- ^ ΔfG°, -820.8 kJ · mol−1
- ^ S°, 107.5 J · K−1 · mol−1
- ^ Cp°, 100.58 J · K−1 · mol−1
- ^ ΔfH°, -998.3 kJ · mol−1
- ^ ΔfG°, -823.43 kJ · mol−1
- ^ S°, -117.6 J · K−1 · mol−1
- ^ ΔfH°, -1243.69 kJ · mol−1
- ^ ΔfH°, -2129.2 kJ · mol−1
- ^ ΔfH°, -3014.57 kJ · mol−1
- ^ ΔfG°, -2509.87 kJ · mol−1
- ^ S°, 409.2 J · K−1 · mol−1
- ^ Cp°, 394.47 J · K−1 · mol−1
- ^ ΔfH°, -492.0 kJ · mol−1
- ^ ΔfG°, -386.6 kJ · mol−1
- ^ S°, 50. J · K−1 · mol−1
- ^ ΔfH°, -272.0 kJ · mol−1