2BeBr2 + 2H2O 💧⚡→ 2Be + O2↑ + 4HBr↑
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- Electrolysis of aqueous beryllium bromide with water as reducing agent
Electrolysis of aqueous beryllium bromide yields , , and hydrogen bromide (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolysis of aqueous beryllium bromide with water as reducing agent
General equation
- Electrolysis of aqueous solution with water as reducing agent
- Miscible with water/Very soluble in water/Soluble in waterOxidizing agent + H2OReducing agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous beryllium bromide with water as reducing agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BeBr2 | Beryllium bromide | 2 | Oxidizing | Very soluble in water |
| H2O | Water | 2 | Reducing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 2 | Reduced | – | ||
| 1 | Oxidized | – | ||
| HBr | Hydrogen bromide | 4 | – | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous beryllium bromide with water as reducing agent
| 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 | 1133.1 | – | – | – |
per 1 mol of | 566.55 | – | – | – |
per 1 mol of | 566.55 | – | – | – |
| 566.55 | – | – | – | |
| 1133.1 | – | – | – | |
per 1 mol of | 283.27 | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous beryllium bromide with water as reducing agent
| 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 | 1133.1 | – | – | – |
per 1 mol of | 566.55 | – | – | – |
per 1 mol of | 566.55 | – | – | – |
| 566.55 | – | – | – | |
| 1133.1 | – | – | – | |
per 1 mol of | 283.27 | – | – | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous beryllium bromide with water as reducing agent
| 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 | 792.5 | – | – | – |
per 1 mol of | 396.3 | – | – | – |
per 1 mol of | 396.3 | – | – | – |
| 396.3 | – | – | – | |
| 792.5 | – | – | – | |
per 1 mol of | 198.1 | – | – | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous beryllium bromide with water as reducing agent
| 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 | 1121.4 | – | – | – |
per 1 mol of | 560.70 | – | – | – |
per 1 mol of | 560.70 | – | – | – |
| 560.70 | – | – | – | |
| 1121.4 | – | – | – | |
per 1 mol of | 280.35 | – | – | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous beryllium bromide with water as reducing agent
| 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 | 780.8 | – | – | – |
per 1 mol of | 390.4 | – | – | – |
per 1 mol of | 390.4 | – | – | – |
| 390.4 | – | – | – | |
| 780.8 | – | – | – | |
per 1 mol of | 195.2 | – | – | – |
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 |
|---|---|---|---|---|
| BeBr2 (cr) | -353.5[1] | – | – | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (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] | 9.50[1] | 16.44[1] |
| (g) | 324.3[1] | 286.6[1] | 136.269[1] | 20.786[1] |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
| HBr (g) | -36.40[1] | -53.45[1] | 198.695[1] | 29.142[1] |
| HBr (ai) | -121.55[1] | -103.96[1] | 82.4[1] | -141.8[1] |
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (ai):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°, -353.5 kJ · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 9.50 J · K−1 · mol−1
- ^ Cp°, 16.44 J · K−1 · mol−1
- ^ ΔfH°, 324.3 kJ · mol−1
- ^ ΔfG°, 286.6 kJ · mol−1
- ^ S°, 136.269 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 J · K−1 · mol−1
- ^ ΔfH°, -36.40 kJ · mol−1
- ^ ΔfG°, -53.45 kJ · mol−1
- ^ S°, 198.695 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -121.55 kJ · mol−1
- ^ ΔfG°, -103.96 kJ · mol−1
- ^ S°, 82.4 J · K−1 · mol−1
- ^ Cp°, -141.8 J · K−1 · mol−1