BaBr2 + 4KMnO4 🔥→ BaO + 2KBrO3 + 4MnO2 + K2O
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The reaction of barium bromide and potassium permanganate yields barium oxide, potassium bromate, 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 barium 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 barium bromide and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaBr2 | Barium bromide | 1 | Reducing | Hardly oxidizable |
| KMnO4 | Potassium permanganate | 4 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaO | Barium oxide | 1 | – | – |
| KBrO3 | Potassium bromate | 2 | Oxidized | – |
| MnO2 | Manganese(IV) oxide | 4 | Reduced | – |
| K2O | Potassium oxide | 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of barium bromide and potassium permanganate◆
ΔrG 437.1 kJ/mol K 0.27 × 10−76 pK 76.58
| 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 | 390.5 | 437.1 | −158 | – |
per 1 mol of | 390.5 | 437.1 | −158 | – |
per 1 mol of | 97.63 | 109.3 | −39.5 | – |
per 1 mol of | 390.5 | 437.1 | −158 | – |
per 1 mol of | 195.3 | 218.6 | −79.0 | – |
per 1 mol of | 97.63 | 109.3 | −39.5 | – |
per 1 mol of | 390.5 | 437.1 | −158 | – |
Changes in standard condition (2)
- Reaction of barium 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 | 460.6 | – | – | – |
per 1 mol of | 460.6 | – | – | – |
per 1 mol of | 115.2 | – | – | – |
per 1 mol of | 460.6 | – | – | – |
per 1 mol of | 230.3 | – | – | – |
per 1 mol of | 115.2 | – | – | – |
per 1 mol of | 460.6 | – | – | – |
Changes in aqueous solution
- Reaction of barium bromide and potassium permanganate◆
ΔrG 453.6 kJ/mol K 0.34 × 10−79 pK 79.47
| 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 | 321.9 | 453.6 | −444.1 | – |
per 1 mol of | 321.9 | 453.6 | −444.1 | – |
per 1 mol of | 80.47 | 113.4 | −111.0 | – |
per 1 mol of | 321.9 | 453.6 | −444.1 | – |
per 1 mol of | 160.9 | 226.8 | −222.1 | – |
per 1 mol of | 80.47 | 113.4 | −111.0 | – |
per 1 mol of | 321.9 | 453.6 | −444.1 | – |
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 |
|---|---|---|---|---|
| BaBr2 (cr) | -757.3[1] | -736.8[1] | 146[1] | – |
| BaBr2 (g) | -439[1] | -473[1] | 331[1] | 61.5[1] |
| BaBr2 (ai) | -780.73[1] | -768.68[1] | 174.5[1] | – |
| BaBr2 (cr) 1 hydrate | -1068.2[1] | – | – | – |
| BaBr2 (cr) 2 hydrate | -1366.1[1] | -1230.4[1] | 226[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, (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 |
|---|---|---|---|---|
| BaO (cr) | -553.5[1] | -525.1[1] | 70.42[1] | 47.78[1] |
| BaO (g) | -117[1] | – | – | 33.1[1] |
| KBrO3 (cr) | -360.24[1] | -271.16[1] | 149.16[1] | 105.19[1] |
| KBrO3 (ai) | -319.45[1] | -264.67[1] | 264.22[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, (g):Gas, (ai):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°, -757.3 kJ · mol−1
- ^ ΔfG°, -736.8 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1
- ^ ΔfH°, -439. kJ · mol−1
- ^ ΔfG°, -473. kJ · mol−1
- ^ S°, 331. J · K−1 · mol−1
- ^ Cp°, 61.5 J · K−1 · mol−1
- ^ ΔfH°, -780.73 kJ · mol−1
- ^ ΔfG°, -768.68 kJ · mol−1
- ^ S°, 174.5 J · K−1 · mol−1
- ^ ΔfH°, -1068.2 kJ · mol−1
- ^ ΔfH°, -1366.1 kJ · mol−1
- ^ ΔfG°, -1230.4 kJ · mol−1
- ^ S°, 226. J · K−1 · 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°, -553.5 kJ · mol−1
- ^ ΔfG°, -525.1 kJ · mol−1
- ^ S°, 70.42 J · K−1 · mol−1
- ^ Cp°, 47.78 J · K−1 · mol−1
- ^ ΔfH°, -117. kJ · mol−1
- ^ Cp°, 33.1 J · K−1 · mol−1
- ^ ΔfH°, -360.24 kJ · mol−1
- ^ ΔfG°, -271.16 kJ · mol−1
- ^ S°, 149.16 J · K−1 · mol−1
- ^ Cp°, 105.19 J · K−1 · mol−1
- ^ ΔfH°, -319.45 kJ · mol−1
- ^ ΔfG°, -264.67 kJ · mol−1
- ^ S°, 264.22 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