3Li2B4O7 🔥⚡→ 6Li + 6B2O3 + O3↑
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- Molten salt electrolysis of lithium tetraborate
Molten salt electrolysis of lithium tetraborate yields , diboron trioxide, and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Molten salt electrolysis of lithium tetraborate
General equation
- Molten salt electrolysis
- SaltSelf redox agent🔥⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Molten salt electrolysis of lithium tetraborate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Li2B4O7 | Lithium tetraborate | 3 | Self redox agent | Salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 6 | Reduced | – | ||
| B2O3 | Diboron trioxide | 6 | – | – |
| 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Molten salt electrolysis of lithium tetraborate
| 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 | 2677.0 | – | – | – |
per 1 mol of | 892.33 | – | – | – |
| 446.17 | – | – | – | |
per 1 mol of | 446.17 | – | – | – |
| 2677.0 | – | – | – |
Changes in standard condition (2)
- Molten salt electrolysis of lithium tetraborate
| 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 | 2786.4 | – | – | – |
per 1 mol of | 928.80 | – | – | – |
| 464.40 | – | – | – | |
per 1 mol of | 464.40 | – | – | – |
| 2786.4 | – | – | – |
Changes in aqueous solution (1)
- Molten salt electrolysis of lithium tetraborate
| 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 | 2677.0 | – | – | – |
per 1 mol of | 892.33 | – | – | – |
| 446.17 | – | – | – | |
per 1 mol of | 446.17 | – | – | – |
| 2677.0 | – | – | – |
Changes in aqueous solution (2)
- Molten salt electrolysis of lithium tetraborate
| 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 | 2660.2 | – | – | – |
per 1 mol of | 886.73 | – | – | – |
| 443.37 | – | – | – | |
per 1 mol of | 443.37 | – | – | – |
| 2660.2 | – | – | – |
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 |
|---|---|---|---|---|
| Li2B4O7 (cr) | -3390.3[1] | – | – | – |
| Li2B4O7 (vit) | -3342.2[1] | – | – | – |
* (cr):Crystalline solid, (vit):Vitreous liquid
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] | 29.12[1] | 24.77[1] |
| (g) | 159.37[1] | 126.66[1] | 138.77[1] | 20.786[1] |
| B2O3 (cr) | -1272.77[1] | -1193.65[1] | 53.97[1] | 62.93[1] |
| B2O3 (am) | -1254.53[1] | -1182.3[1] | 77.8[1] | 61.1[1] |
| B2O3 (g) | -843.79[1] | -831.97[1] | 279.81[1] | 66.86[1] |
| (g) | 142.7[1] | 163.2[1] | 238.93[1] | 39.20[1] |
| (ao) | 125.9[1] | 174.1[1] | 146[1] | – |
* (cr):Crystalline solid, (g):Gas, (am):Amorphous solid, (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°, -3390.3 kJ · mol−1
- ^ ΔfH°, -3342.2 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 29.12 J · K−1 · mol−1
- ^ Cp°, 24.77 J · K−1 · mol−1
- ^ ΔfH°, 159.37 kJ · mol−1
- ^ ΔfG°, 126.66 kJ · mol−1
- ^ S°, 138.77 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -1272.77 kJ · mol−1
- ^ ΔfG°, -1193.65 kJ · mol−1
- ^ S°, 53.97 J · K−1 · mol−1
- ^ Cp°, 62.93 J · K−1 · mol−1
- ^ ΔfH°, -1254.53 kJ · mol−1
- ^ ΔfG°, -1182.3 kJ · mol−1
- ^ S°, 77.8 J · K−1 · mol−1
- ^ Cp°, 61.1 J · K−1 · mol−1
- ^ ΔfH°, -843.79 kJ · mol−1
- ^ ΔfG°, -831.97 kJ · mol−1
- ^ S°, 279.81 J · K−1 · mol−1
- ^ Cp°, 66.86 J · K−1 · mol−1
- ^ ΔfH°, 142.7 kJ · mol−1
- ^ ΔfG°, 163.2 kJ · mol−1
- ^ S°, 238.93 J · K−1 · mol−1
- ^ Cp°, 39.20 J · K−1 · mol−1
- ^ ΔfH°, 125.9 kJ · mol−1
- ^ ΔfG°, 174.1 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1