3K2SiO3 + 4e− → 3K2O + Si + 2SiO32−
Last updated:
- Reduction of potassium metasilicate
Reduction of potassium metasilicate yields potassium oxide, , and metasilicate ion (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reduction of potassium metasilicate
General equation
- Reduction of reducible species
- ReactantOxidizing agent + e− ⟶ ProductReduction product
Oxidation state of each atom
- Reduction of potassium metasilicate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2SiO3 | Potassium metasilicate | 3 | Oxidizing | – |
| e− | Electron | 4 | – | Electron |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2O | Potassium oxide | 3 | – | – |
| 1 | Reduced | – | ||
| SiO32− | Metasilicate ion | 2 | – | – |
Thermodynamic changes
Changes in standard condition
- Reduction of potassium metasilicate
| 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 | – | – | −329.3 | – |
per 1 mol of | – | – | −109.8 | – |
per 1 mol of Electron | – | – | −82.33 | – |
per 1 mol of | – | – | −109.8 | – |
| – | – | −329.3 | – | |
per 1 mol of Metasilicate ion | – | – | −164.7 | – |
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 |
|---|---|---|---|---|
| K2SiO3 (cr) | – | – | 146.0[1] | 118.4[1] |
| e− | – | – | – | – |
* (cr):Crystalline solid
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 |
|---|---|---|---|---|
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[1] | – | – | – |
| (cr) | 0[1] | 0[1] | 18.83[1] | 20.00[1] |
| (am) | 4.2[1] | – | – | – |
| (g) | 455.6[1] | 411.3[1] | 167.97[1] | 22.251[1] |
| SiO32− (ao) | -1104.576[3] | -939.764[3] | -96.232[3] | – |
* (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)
- ^ S°, 146.0 J · K−1 · mol−1
- ^ Cp°, 118.4 J · K−1 · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 18.83 J · K−1 · mol−1
- ^ Cp°, 20.00 J · K−1 · mol−1
- ^ ΔfH°, 4.2 kJ · mol−1
- ^ ΔfH°, 455.6 kJ · mol−1
- ^ ΔfG°, 411.3 kJ · mol−1
- ^ S°, 167.97 J · K−1 · mol−1
- ^ Cp°, 22.251 J · K−1 · mol−1
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfG°, -322.1 kJ · mol−1 - p.280
- ^ S°, 94.1 J · K−1 · mol−1 - p.280
- ^ Cp°, 83.7 J · K−1 · mol−1 - p.280
- 3Colin Stuart Walker, Anraku Sohtaro, Oda Chie, Mitsui Seiichiro, Mihara MorihiroThermodynamic properties of SiO2(aq), HSiO3– and SiO3-2Japan Atomic Energy Agency