3CuBr2 + 2KMnO4 → 3CuO + 3Br2 + 2MnO2 + K2O
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The reaction of copper(II) bromide and potassium permanganate yields copper(II) oxide, , manganese(IV) oxide, and potassium 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 copper(II) bromide and potassium permanganate
General equation
- Reaction of hardly oxidizable species and oxidizing species
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of copper(II) bromide and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuBr2 | Copper(II) bromide | 3 | Reducing | Hardly oxidizable |
| KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuO | Copper(II) oxide | 3 | – | – |
| 3 | Oxidized | – | ||
| MnO2 | Manganese(IV) oxide | 2 | Reduced | – |
| K2O | Potassium oxide | 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of copper(II) bromide and potassium permanganate
| 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 | 226.3 | – | – | – |
per 1 mol of | 75.43 | – | – | – |
per 1 mol of | 113.2 | – | – | – |
per 1 mol of | 75.43 | – | – | – |
| 75.43 | – | – | – | |
per 1 mol of | 113.2 | – | – | – |
per 1 mol of | 226.3 | – | – | – |
Changes in standard condition (2)
- Reaction of copper(II) bromide and potassium permanganate
| 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 | 261.4 | – | – | – |
per 1 mol of | 87.13 | – | – | – |
per 1 mol of | 130.7 | – | – | – |
per 1 mol of | 87.13 | – | – | – |
| 87.13 | – | – | – | |
per 1 mol of | 130.7 | – | – | – |
per 1 mol of | 261.4 | – | – | – |
Changes in aqueous solution
- Reaction of copper(II) bromide and potassium permanganate
| 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 | 131.8 | – | – | – |
per 1 mol of | 43.93 | – | – | – |
per 1 mol of | 65.90 | – | – | – |
per 1 mol of | 43.93 | – | – | – |
| 43.93 | – | – | – | |
per 1 mol of | 65.90 | – | – | – |
per 1 mol of | 131.8 | – | – | – |
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] | – | – | – |
| KMnO4 (cr) | -837.2[1] | -737.6[1] | 171.71[1] | 117.57[1] |
| KMnO4 (ai) | -793.8[1] | -730.5[1] | 293.7[1] | -60.2[1] |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| CuO (cr) | -157.3[1] | -129.7[1] | 42.63[1] | 42.30[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] | – |
| MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
| MnO2 (am) precipitated | -502.5[1] | – | – | – |
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[1] | – | – | – |
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (am):Amorphous 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°, -141.8 kJ · mol−1
- ^ ΔfH°, -1326.3 kJ · mol−1
- ^ ΔfH°, -837.2 kJ · mol−1
- ^ ΔfG°, -737.6 kJ · mol−1
- ^ S°, 171.71 J · K−1 · mol−1
- ^ Cp°, 117.57 J · K−1 · mol−1
- ^ ΔfH°, -793.8 kJ · mol−1
- ^ ΔfG°, -730.5 kJ · mol−1
- ^ S°, 293.7 J · K−1 · mol−1
- ^ Cp°, -60.2 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°, 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
- ^ ΔfH°, -520.03 kJ · mol−1
- ^ ΔfG°, -465.14 kJ · mol−1
- ^ S°, 53.05 J · K−1 · mol−1
- ^ Cp°, 54.14 J · K−1 · mol−1
- ^ ΔfH°, -502.5 kJ · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · mol−1
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfG°, -322.1 kJ · mol−1 - p.280
- ^ S°, 94.1 J · K−1 · mol−1 - p.280
- ^ Cp°, 83.7 J · K−1 · mol−1 - p.280