13Cu + Fe2(SO4)3 🔥→ 3CuS + 10CuO + 2FeO
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- Reaction of and iron(III) sulfate
The reaction of and iron(III) sulfate yields copper(II) sulfide, copper(II) oxide, 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(III) 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(III) sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 13 | Reducing | Oxidizable | ||
| Fe2(SO4)3 | Iron(III) sulfate | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuS | Copper(II) sulfide | 3 | Redoxed product | – |
| CuO | Copper(II) oxide | 10 | Oxidized | – |
| FeO | Iron(II) oxide | 2 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and iron(III) 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 | 305.2 | – | – | – |
| 23.48 | – | – | – | |
per 1 mol of | 305.2 | – | – | – |
per 1 mol of | 101.7 | – | – | – |
per 1 mol of | 30.52 | – | – | – |
per 1 mol of | 152.6 | – | – | – |
Changes in aqueous solution
- Reaction of and iron(III) 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 | 548.7 | – | – | – |
| 42.21 | – | – | – | |
per 1 mol of | 548.7 | – | – | – |
per 1 mol of | 182.9 | – | – | – |
per 1 mol of | 54.87 | – | – | – |
per 1 mol of | 274.4 | – | – | – |
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] |
| Fe2(SO4)3 (cr) | -2581.5[1] | – | – | – |
| Fe2(SO4)3 (ai) | -2825.0[1] | -2242.8[1] | -571.5[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 |
|---|---|---|---|---|
| CuS (cr) | -53.1[1] | -53.6[1] | 66.5[1] | 47.82[1] |
| CuO (cr) | -157.3[1] | -129.7[1] | 42.63[1] | 42.30[1] |
| FeO (cr) | -272.0[1] | – | – | – |
* (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°, -2581.5 kJ · mol−1
- ^ ΔfH°, -2825.0 kJ · mol−1
- ^ ΔfG°, -2242.8 kJ · mol−1
- ^ S°, -571.5 J · K−1 · mol−1
- ^ ΔfH°, -53.1 kJ · mol−1
- ^ ΔfG°, -53.6 kJ · mol−1
- ^ S°, 66.5 J · K−1 · mol−1
- ^ Cp°, 47.82 J · K−1 · mol−1
- ^ ΔfH°, -157.3 kJ · mol−1
- ^ ΔfG°, -129.7 kJ · mol−1
- ^ S°, 42.63 J · K−1 · mol−1
- ^ Cp°, 42.30 J · K−1 · mol−1
- ^ ΔfH°, -272.0 kJ · mol−1