8B + 12KOH → K2B4O7 + 2B2H6↑ + 5K2O
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- Reaction of and potassium hydroxide
The reaction of and potassium hydroxide yields potassium tetraborate, diborane(6), 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 and potassium hydroxide
General equation
- Self redox agent + Hydroxide base ⟶ Oxoacid saltOxidation product + Salt of hydracid/HydrideReduction product + OxideNon-redox product
Oxidation state of each atom
- Reaction of and potassium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 8 | – | Nonmetal | ||
| KOH | Potassium hydroxide | 12 | – | Hydroxide base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2B4O7 | Potassium tetraborate | 1 | Oxidized | Oxoacid salt |
| B2H6 | Diborane(6) | 2 | Reduced | Hydride |
| K2O | Potassium oxide | 5 | – | Oxide |
Thermodynamic changes
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 5.86[1] | 11.09[1] |
| (am) x denotes undetermined zero point entropy | 3.8[1] | – | 6.53+x[1] | 11.97[1] |
| (g) | 562.7[1] | 518.8[1] | 153.45[1] | 20.799[1] |
| KOH (cr) | -424.764[1] | -379.08[1] | 78.9[1] | 64.9[1] |
| KOH (g) | -231.0[1] | -232.6[1] | 238.3[1] | 49.20[1] |
| KOH (ai) | -482.37[1] | -440.50[1] | 91.6[1] | -126.8[1] |
| KOH (cr) 1 hydrate | -748.9[1] | -645.1[1] | 117.2[1] | – |
| KOH (cr) 2 hydrate | -1051.0[1] | -887.3[1] | 150.6[1] | – |
* (cr):Crystalline solid, (am):Amorphous 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 |
|---|---|---|---|---|
| K2B4O7 (cr) 4 hydrate | – | -4134.7[1] | – | – |
| B2H6 (g) | 35.6[1] | 86.7[1] | 232.11[1] | 56.90[1] |
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 5.86 J · K−1 · mol−1
- ^ Cp°, 11.09 J · K−1 · mol−1
- ^ ΔfH°, 3.8 kJ · mol−1
- ^ S°, 6.53+x J · K−1 · mol−1
- ^ Cp°, 11.97 J · K−1 · mol−1
- ^ ΔfH°, 562.7 kJ · mol−1
- ^ ΔfG°, 518.8 kJ · mol−1
- ^ S°, 153.45 J · K−1 · mol−1
- ^ Cp°, 20.799 J · K−1 · mol−1
- ^ ΔfH°, -424.764 kJ · mol−1
- ^ ΔfG°, -379.08 kJ · mol−1
- ^ S°, 78.9 J · K−1 · mol−1
- ^ Cp°, 64.9 J · K−1 · mol−1
- ^ ΔfH°, -231.0 kJ · mol−1
- ^ ΔfG°, -232.6 kJ · mol−1
- ^ S°, 238.3 J · K−1 · mol−1
- ^ Cp°, 49.20 J · K−1 · mol−1
- ^ ΔfH°, -482.37 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 91.6 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfH°, -748.9 kJ · mol−1
- ^ ΔfG°, -645.1 kJ · mol−1
- ^ S°, 117.2 J · K−1 · mol−1
- ^ ΔfH°, -1051.0 kJ · mol−1
- ^ ΔfG°, -887.3 kJ · mol−1
- ^ S°, 150.6 J · K−1 · mol−1
- ^ ΔfG°, -4134.7 kJ · mol−1
- ^ ΔfH°, 35.6 kJ · mol−1
- ^ ΔfG°, 86.7 kJ · mol−1
- ^ S°, 232.11 J · K−1 · mol−1
- ^ Cp°, 56.90 J · K−1 · 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