2LiBr + 2H2O 💧⚡→ 2LiOH + Br2 + H2↑
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- Electrolysis of aqueous lithium bromide with water as oxidizing agent
Electrolysis of aqueous lithium bromide yields lithium hydroxide, , and . This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolysis of aqueous lithium bromide with water as oxidizing agent
General equation
- Electrolysis of aqueous solution with water as oxidizing agent
- Miscible with water/Very soluble in water/Soluble in waterReducing agent + H2OOxidizing agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous lithium bromide with water as oxidizing agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| LiBr | Lithium bromide | 2 | Reducing | Very soluble in water |
| H2O | Water | 2 | Oxidizing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| LiOH | Lithium hydroxide | 2 | – | – |
| 1 | Oxidized | – | ||
| 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous lithium bromide with water as oxidizing agent◆
ΔrG 280.36 kJ/mol K 0.76 × 10−49 pK 49.12
| 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 | 304.23 | 280.36 | 80.16 | – |
per 1 mol of | 152.12 | 140.18 | 40.08 | – |
per 1 mol of | 152.12 | 140.18 | 40.08 | – |
per 1 mol of | 152.12 | 140.18 | 40.08 | – |
| 304.23 | 280.36 | 80.16 | – | |
| 304.23 | 280.36 | 80.16 | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous lithium bromide with water as oxidizing agent◆
ΔrG 371.57 kJ/mol K 0.80 × 10−65 pK 65.10
| 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 | 352.19 | 371.57 | −64.6 | – |
per 1 mol of | 176.09 | 185.78 | −32.3 | – |
per 1 mol of | 176.09 | 185.78 | −32.3 | – |
per 1 mol of | 176.09 | 185.78 | −32.3 | – |
| 352.19 | 371.57 | −64.6 | – | |
| 352.19 | 371.57 | −64.6 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous lithium bromide with water as oxidizing agent◆
ΔrG 389.2 kJ/mol K 0.65 × 10−68 pK 68.18
| 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 | 348.0 | 389.2 | 382 | – |
per 1 mol of | 174.0 | 194.6 | 191 | – |
per 1 mol of | 174.0 | 194.6 | 191 | – |
per 1 mol of | 174.0 | 194.6 | 191 | – |
| 348.0 | 389.2 | 382 | – | |
| 348.0 | 389.2 | 382 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous lithium bromide with water as oxidizing agent◆
ΔrG 369.1 kJ/mol K 0.22 × 10−64 pK 64.66
| 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 | 352.4 | 369.1 | −56.0 | – |
per 1 mol of | 176.2 | 184.6 | −28.0 | – |
per 1 mol of | 176.2 | 184.6 | −28.0 | – |
per 1 mol of | 176.2 | 184.6 | −28.0 | – |
| 352.4 | 369.1 | −56.0 | – | |
| 352.4 | 369.1 | −56.0 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous lithium bromide with water as oxidizing agent◆
ΔrG 386.7 kJ/mol K 0.18 × 10−67 pK 67.75
| 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 | 348.2 | 386.7 | 390 | – |
per 1 mol of | 174.1 | 193.3 | 195 | – |
per 1 mol of | 174.1 | 193.3 | 195 | – |
per 1 mol of | 174.1 | 193.3 | 195 | – |
| 348.2 | 386.7 | 390 | – | |
| 348.2 | 386.7 | 390 | – |
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 |
|---|---|---|---|---|
| LiBr (cr) | -351.213[1] | -342.00[1] | 74.27[1] | – |
| LiBr (g) | – | – | 224.33[1] | 33.93[1] |
| LiBr (ai) | -400.041[1] | -397.27[1] | 95.8[1] | -73.2[1] |
| LiBr (cr) 1 hydrate | -662.58[1] | -594.29[1] | 109.6[1] | – |
| LiBr (cr) 2 hydrate | -962.7[1] | -840.5[1] | 162.3[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, (g):Gas, (ai):Ionized aqueous solution, (l):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 |
|---|---|---|---|---|
| LiOH (cr) | -484.93[1] | -438.95[1] | 42.80[1] | 49.66[1] |
| LiOH (g) | -238.1[1] | -242.3[1] | 210.90[1] | 46.02[1] |
| LiOH (ai) | -508.48[1] | -450.58[1] | 2.80[1] | -79.9[1] |
| LiOH (ao) | -508.4[1] | -451.8[1] | 7.1[1] | – |
| LiOH (cr) 1 hydrate | -788.01[1] | -680.95[1] | 71.21[1] | 79.50[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] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -351.213 kJ · mol−1
- ^ ΔfG°, -342.00 kJ · mol−1
- ^ S°, 74.27 J · K−1 · mol−1
- ^ S°, 224.33 J · K−1 · mol−1
- ^ Cp°, 33.93 J · K−1 · mol−1
- ^ ΔfH°, -400.041 kJ · mol−1
- ^ ΔfG°, -397.27 kJ · mol−1
- ^ S°, 95.8 J · K−1 · mol−1
- ^ Cp°, -73.2 J · K−1 · mol−1
- ^ ΔfH°, -662.58 kJ · mol−1
- ^ ΔfG°, -594.29 kJ · mol−1
- ^ S°, 109.6 J · K−1 · mol−1
- ^ ΔfH°, -962.7 kJ · mol−1
- ^ ΔfG°, -840.5 kJ · mol−1
- ^ S°, 162.3 J · K−1 · 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°, -484.93 kJ · mol−1
- ^ ΔfG°, -438.95 kJ · mol−1
- ^ S°, 42.80 J · K−1 · mol−1
- ^ Cp°, 49.66 J · K−1 · mol−1
- ^ ΔfH°, -238.1 kJ · mol−1
- ^ ΔfG°, -242.3 kJ · mol−1
- ^ S°, 210.90 J · K−1 · mol−1
- ^ Cp°, 46.02 J · K−1 · mol−1
- ^ ΔfH°, -508.48 kJ · mol−1
- ^ ΔfG°, -450.58 kJ · mol−1
- ^ S°, 2.80 J · K−1 · mol−1
- ^ Cp°, -79.9 J · K−1 · mol−1
- ^ ΔfH°, -508.4 kJ · mol−1
- ^ ΔfG°, -451.8 kJ · mol−1
- ^ S°, 7.1 J · K−1 · mol−1
- ^ ΔfH°, -788.01 kJ · mol−1
- ^ ΔfG°, -680.95 kJ · mol−1
- ^ S°, 71.21 J · K−1 · mol−1
- ^ Cp°, 79.50 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
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1