2CuBr2 🔥⚡→ 2CuBr + Br2
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- Molten salt electrolysis of copper(II) bromide
Molten salt electrolysis of copper(II) bromide yields copper(I) bromide and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Molten salt electrolysis of copper(II) bromide
General equation
- Molten salt electrolysis
- SaltSelf redox agent🔥⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Molten salt electrolysis of copper(II) bromide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuBr2 | Copper(II) bromide | 2 | Self redox agent | Salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuBr | Copper(I) bromide | 2 | Reduced | – |
| 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition
- Molten salt electrolysis of 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 | 74.4 | – | – | – |
per 1 mol of | 37.2 | – | – | – |
per 1 mol of | 37.2 | – | – | – |
| 74.4 | – | – | – |
Changes in aqueous solution
- Molten salt electrolysis of 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 | 71.8 | – | – | – |
per 1 mol of | 35.9 | – | – | – |
per 1 mol of | 35.9 | – | – | – |
| 71.8 | – | – | – |
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 |
|---|---|---|---|---|
| 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 |
|---|---|---|---|---|
| CuBr (cr) | -104.6[1] | -100.8[1] | 96.11[1] | 54.73[1] |
| (cr) | – | – | – | – |
| (l) | 0[1] | 0[1] | 152.231[1] | 75.689[1] |
| (g) | 30.907[1] | 3.110[1] | 245.463[1] | 36.02[1] |
| (ao) | -2.59[1] | 3.93[1] | 130.5[1] | – |
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (ao):Un-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°, -141.8 kJ · mol−1
- ^ ΔfH°, -1326.3 kJ · 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 152.231 J · K−1 · mol−1
- ^ Cp°, 75.689 J · K−1 · mol−1
- ^ ΔfH°, 30.907 kJ · mol−1
- ^ ΔfG°, 3.110 kJ · mol−1
- ^ S°, 245.463 J · K−1 · mol−1
- ^ Cp°, 36.02 J · K−1 · mol−1
- ^ ΔfH°, -2.59 kJ · mol−1
- ^ ΔfG°, 3.93 kJ · mol−1
- ^ S°, 130.5 J · K−1 · mol−1