K2SiO3 🔥→ K2O + Si + O2↑
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- Decomposition of potassium metasilicate
Decomposition of potassium metasilicate yields potassium oxide, , and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Decomposition of potassium metasilicate
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
- Thermal decomposition of oxoacid salt with redox
- Oxoacid saltSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of potassium metasilicate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
K2SiO3 | Potassium metasilicate | 1 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
K2O | Potassium oxide | 1 | – | – |
1 | Reduced | – | ||
1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Decomposition 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 | – | – | 172.1 | 14.7 |
per 1 mol of | – | – | 172.1 | 14.7 |
per 1 mol of | – | – | 172.1 | 14.7 |
– | – | 172.1 | 14.7 | |
– | – | 172.1 | 14.7 |
Changes in standard condition (2)
- Decomposition 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
– | – | – | – | |
– | – | – | – |
Changes in aqueous solution (1)
- Decomposition 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 | – | – | 172.1 | 14.7 |
per 1 mol of | – | – | 172.1 | 14.7 |
per 1 mol of | – | – | 172.1 | 14.7 |
– | – | 172.1 | 14.7 | |
– | – | 172.1 | 14.7 |
Changes in aqueous solution (2)
- Decomposition 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 | – | – | 77.8 | – |
per 1 mol of | – | – | 77.8 | – |
per 1 mol of | – | – | 77.8 | – |
– | – | 77.8 | – | |
– | – | 77.8 | – |
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] |
* (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] |
(g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
(ao) | -11.7[1] | 16.4[1] | 110.9[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)
- ^ 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
- ^ 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
- 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