FeO + 2CuBr2 🔥→ FeBr3 + CuBr + CuO
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The reaction of iron(II) oxide and copper(II) bromide yields iron(III) bromide, copper(I) bromide, and copper(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 iron(II) oxide and copper(II) bromide
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 copper(II) bromide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeO | Iron(II) oxide | 1 | Reducing | Oxidizable |
| CuBr2 | Copper(II) bromide | 2 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeBr3 | Iron(III) bromide | 1 | Oxidized | – |
| CuBr | Copper(I) bromide | 1 | Reduced | – |
| CuO | Copper(II) oxide | 1 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of iron(II) oxide and copper(II) bromide
| 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 | 25.5 | – | – | – |
per 1 mol of | 25.5 | – | – | – |
per 1 mol of | 12.8 | – | – | – |
per 1 mol of | 25.5 | – | – | – |
per 1 mol of | 25.5 | – | – | – |
per 1 mol of | 25.5 | – | – | – |
Changes in aqueous solution
- Reaction of iron(II) oxide and copper(II) bromide
| 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 | −119.7 | – | – | – |
per 1 mol of | −119.7 | – | – | – |
per 1 mol of | −59.85 | – | – | – |
per 1 mol of | −119.7 | – | – | – |
per 1 mol of | −119.7 | – | – | – |
per 1 mol of | −119.7 | – | – | – |
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] | – | – | – |
| CuBr2 (cr) | -141.8[1] | – | – | – |
| CuBr2 (cr) 4 hydrate | -1326.3[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 |
|---|---|---|---|---|
| FeBr3 (cr) | -268.2[1] | – | – | – |
| FeBr3 (g) | -123.8[1] | – | – | – |
| FeBr3 (ai) | -413.4[1] | -316.7[1] | -68.6[1] | – |
| CuBr (cr) | -104.6[1] | -100.8[1] | 96.11[1] | 54.73[1] |
| CuO (cr) | -157.3[1] | -129.7[1] | 42.63[1] | 42.30[1] |
* (cr):Crystalline solid, (g):Gas, (ai):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°, -272.0 kJ · mol−1
- ^ ΔfH°, -141.8 kJ · mol−1
- ^ ΔfH°, -1326.3 kJ · mol−1
- ^ ΔfH°, -268.2 kJ · mol−1
- ^ ΔfH°, -123.8 kJ · mol−1
- ^ ΔfH°, -413.4 kJ · mol−1
- ^ ΔfG°, -316.7 kJ · mol−1
- ^ S°, -68.6 J · K−1 · mol−1
- ^ ΔfH°, -104.6 kJ · mol−1
- ^ ΔfG°, -100.8 kJ · mol−1
- ^ S°, 96.11 J · K−1 · mol−1
- ^ Cp°, 54.73 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