2RbF 🔥⚡→ 2Rb + F2↑
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- Molten salt electrolysis of rubidium fluoride
Molten salt electrolysis of rubidium fluoride yields and . This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Molten salt electrolysis of rubidium fluoride
General equation
- Molten salt electrolysis
- SaltSelf redox agent🔥⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Molten salt electrolysis of rubidium fluoride
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| RbF | Rubidium fluoride | 2 | Self redox agent | Salt |
Products
Thermodynamic changes
Changes in standard condition
- Molten salt electrolysis of rubidium fluoride
| 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 | 1115.4 | – | – | – |
per 1 mol of | 557.70 | – | – | – |
| 557.70 | – | – | – | |
| 1115.4 | – | – | – |
Changes in aqueous solution
- Molten salt electrolysis of rubidium fluoride◆
ΔrG 1125.54 kJ/mol K 0.65 × 10−197 pK 197.19
| 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 | 1167.58 | 1125.54 | 141.3 | – |
per 1 mol of | 583.790 | 562.770 | 70.65 | – |
| 583.790 | 562.770 | 70.65 | – | |
| 1167.58 | 1125.54 | 141.3 | – |
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 |
|---|---|---|---|---|
| RbF (cr) | -557.7[1] | – | – | – |
| RbF (g) | -331.4[1] | -349.0[1] | 237.09[1] | 35.69[1] |
| RbF (ai) | -583.79[1] | -562.77[1] | 107.5[1] | – |
| RbF (cr) 1.5 hydrate | -1013.8[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution
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] | 76.78[1] | 31.062[1] |
| (g) | 80.88[1] | 53.06[1] | 170.089[1] | 20.786[1] |
| (g) | 0[1] | 0[1] | 202.78[1] | 31.30[1] |
* (cr):Crystalline solid, (g):Gas
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°, -557.7 kJ · mol−1
- ^ ΔfH°, -331.4 kJ · mol−1
- ^ ΔfG°, -349.0 kJ · mol−1
- ^ S°, 237.09 J · K−1 · mol−1
- ^ Cp°, 35.69 J · K−1 · mol−1
- ^ ΔfH°, -583.79 kJ · mol−1
- ^ ΔfG°, -562.77 kJ · mol−1
- ^ S°, 107.5 J · K−1 · mol−1
- ^ ΔfH°, -1013.8 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 76.78 J · K−1 · mol−1
- ^ Cp°, 31.062 J · K−1 · mol−1
- ^ ΔfH°, 80.88 kJ · mol−1
- ^ ΔfG°, 53.06 kJ · mol−1
- ^ S°, 170.089 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 202.78 J · K−1 · mol−1
- ^ Cp°, 31.30 J · K−1 · mol−1