6CuF + Fe2O3 🔥→ 3CuF2 + 3CuO + 2Fe
Last updated:
- Reaction of copper(I) fluoride and iron(III) oxide
The reaction of copper(I) fluoride and iron(III) oxide yields copper(II) fluoride, copper(II) 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 copper(I) fluoride and iron(III) oxide
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 copper(I) fluoride and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuF | Copper(I) fluoride | 6 | Reducing | Oxidizable |
| Fe2O3 | Iron(III) oxide | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuF2 | Copper(II) fluoride | 3 | Oxidized | – |
| CuO | Copper(II) oxide | 3 | Oxidized | – |
| 2 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of copper(I) fluoride and iron(III) oxide
| 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 | 404 | – | – | – |
per 1 mol of | 67.3 | – | – | – |
per 1 mol of | 404 | – | – | – |
per 1 mol of | 135 | – | – | – |
per 1 mol of | 135 | – | – | – |
| 202 | – | – | – |
Changes in aqueous solution
- Reaction of copper(I) fluoride and iron(III) oxide
| 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 | 404 | – | – | – |
per 1 mol of | 67.3 | – | – | – |
per 1 mol of | 404 | – | – | – |
per 1 mol of | 135 | – | – | – |
per 1 mol of | 135 | – | – | – |
| 202 | – | – | – |
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 |
|---|---|---|---|---|
| CuF (s) | -280 | -260 | 64.9 | – |
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
* (s):Solid, (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 |
|---|---|---|---|---|
| CuF2 (cr) | -542.7[1] | – | – | – |
| CuF2 (cr) 2 hydrate | – | -981.4[1] | – | – |
| CuO (cr) | -157.3[1] | -129.7[1] | 42.63[1] | 42.30[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] |
* (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°, -824.2 kJ · mol−1
- ^ ΔfG°, -742.2 kJ · mol−1
- ^ S°, 87.40 J · K−1 · mol−1
- ^ Cp°, 103.85 J · K−1 · mol−1
- ^ ΔfH°, -542.7 kJ · mol−1
- ^ ΔfG°, -981.4 kJ · 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°, 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