2BBr3 ⚡→ 2B + 3Br2
Last updated:
Electrolysis of yields and . This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
General equation
- Electrolysis of liquid substance
- LiquidSelf redox agent⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
Reactants
Products
Thermodynamic changes
Changes in standard condition (1)
| 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 | 479.4 | 477.0 | 9.0 | – |
| 239.7 | 238.5 | 4.5 | – | |
| 239.7 | 238.5 | 4.5 | – | |
| 159.8 | 159.0 | 3.0 | – |
Changes in standard condition (2)
| 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 | 487.0 | – | 3.8 | – |
| 243.5 | – | 1.9 | – | |
| 243.5 | – | 1.9 | – | |
| 162.3 | – | 1.3 | – |
Changes in aqueous solution
| 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 | 471.6 | 488.8 | −56.2 | – |
| 235.8 | 244.4 | −28.1 | – | |
| 235.8 | 244.4 | −28.1 | – | |
| 157.2 | 162.9 | −18.7 | – |
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 |
|---|---|---|---|---|
| (l) | -239.7[1] | -238.5[1] | 229.7[1] | – |
| (g) | -205.64[1] | -232.50[1] | 324.24[1] | 67.78[1] |
* (l):Liquid, (g):Gas
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 |
|---|---|---|---|---|
| (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] |
| (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, (am):Amorphous solid, (g):Gas, (l):Liquid, (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°, -239.7 kJ · mol−1
- ^ ΔfG°, -238.5 kJ · mol−1
- ^ S°, 229.7 J · K−1 · mol−1
- ^ ΔfH°, -205.64 kJ · mol−1
- ^ ΔfG°, -232.50 kJ · mol−1
- ^ S°, 324.24 J · K−1 · mol−1
- ^ Cp°, 67.78 J · K−1 · mol−1
- ^ 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°, 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