CH3COORb + 3H2O 💧⚡→ 2O2↑ + RbOH + 2CH4↑
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- Electrolysis of aqueous rubidium acetate with water as reducing agent
Electrolysis of aqueous rubidium acetate yields , rubidium hydroxide, and (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 rubidium acetate 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 rubidium acetate with water as reducing agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CH3COORb | Rubidium acetate | 1 | Oxidizing | Very soluble in water |
| H2O | Water | 3 | Reducing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 2 | Oxidized | – | ||
| RbOH | Rubidium hydroxide | 1 | – | – |
| 2 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Electrolysis of aqueous rubidium acetate with water as reducing agent◆
ΔrG 822.03 kJ/mol K 0.97 × 10−144 pK 144.01
| 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 | 963.89 | 822.03 | 475.9 | – |
per 1 mol of | 963.89 | 822.03 | 475.9 | – |
per 1 mol of | 321.30 | 274.01 | 158.6 | – |
| 481.94 | 411.01 | 237.9 | – | |
per 1 mol of | 963.89 | 822.03 | 475.9 | – |
| 481.94 | 411.01 | 237.9 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous rubidium acetate with water as reducing agent◆
ΔrG 854.81 kJ/mol K 0.18 × 10−149 pK 149.76
| 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 | 935.43 | 854.81 | 270.8 | – |
per 1 mol of | 935.43 | 854.81 | 270.8 | – |
per 1 mol of | 311.81 | 284.94 | 90.27 | – |
| 467.71 | 427.40 | 135.4 | – | |
per 1 mol of | 935.43 | 854.81 | 270.8 | – |
| 467.71 | 427.40 | 135.4 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous rubidium acetate with water as reducing agent◆
ΔrG 854.8 kJ/mol K 0.18 × 10−149 pK 149.75
| 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 | 940.5 | 854.8 | 287.4 | – |
per 1 mol of | 940.5 | 854.8 | 287.4 | – |
per 1 mol of | 313.5 | 284.9 | 95.80 | – |
| 470.3 | 427.4 | 143.7 | – | |
per 1 mol of | 940.5 | 854.8 | 287.4 | – |
| 470.3 | 427.4 | 143.7 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous rubidium acetate with water as reducing agent◆
ΔrG 887.6 kJ/mol K 0.32 × 10−155 pK 155.50
| 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 | 912.0 | 887.6 | 82.3 | – |
per 1 mol of | 912.0 | 887.6 | 82.3 | – |
per 1 mol of | 304.0 | 295.9 | 27.4 | – |
| 456.0 | 443.8 | 41.1 | – | |
per 1 mol of | 912.0 | 887.6 | 82.3 | – |
| 456.0 | 443.8 | 41.1 | – |
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 |
|---|---|---|---|---|
| CH3COORb (ai) | -737.18[1] | -653.29[1] | 207.9[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] |
* (ai):Ionized aqueous solution, (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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
| RbOH (cr) | -418.19[1] | – | – | – |
| RbOH (g) | -238[1] | – | – | – |
| RbOH (ai) | -481.16[1] | -441.21[1] | 110.75[1] | – |
| RbOH (cr) 1 hydrate | -748.85[1] | – | – | – |
| RbOH (cr) 2 hydrate | -1053.24[1] | – | – | – |
| (g) | -74.81[1] | -50.72[1] | 186.264[1] | 35.309[1] |
| (ao) | -89.04[1] | -34.33[1] | 83.7[1] | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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°, -737.18 kJ · mol−1
- ^ ΔfG°, -653.29 kJ · mol−1
- ^ S°, 207.9 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°, 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°, -418.19 kJ · mol−1
- ^ ΔfH°, -238. kJ · mol−1
- ^ ΔfH°, -481.16 kJ · mol−1
- ^ ΔfG°, -441.21 kJ · mol−1
- ^ S°, 110.75 J · K−1 · mol−1
- ^ ΔfH°, -748.85 kJ · mol−1
- ^ ΔfH°, -1053.24 kJ · mol−1
- ^ ΔfH°, -74.81 kJ · mol−1
- ^ ΔfG°, -50.72 kJ · mol−1
- ^ S°, 186.264 J · K−1 · mol−1
- ^ Cp°, 35.309 J · K−1 · mol−1
- ^ ΔfH°, -89.04 kJ · mol−1
- ^ ΔfG°, -34.33 kJ · mol−1
- ^ S°, 83.7 J · K−1 · mol−1