2LiHCO3 + 2K2SiO3 💧→ Li2SiO3↓ + H2SiO3↓ + 2K2CO3
Last updated:
The reaction of lithium hydrogencarbonate and potassium metasilicate yields lithium metasilicate, metasilicic acid, and potassium carbonate (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of lithium hydrogencarbonate and potassium metasilicate
General equation
- Precipitation reaction
- Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base💧⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)
Oxidation state of each atom
- Reaction of lithium hydrogencarbonate and potassium metasilicate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| LiHCO3 | Lithium hydrogencarbonate | 2 | Lewis acid | Soluble in water |
| K2SiO3 | Potassium metasilicate | 2 | Lewis base | Soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Li2SiO3 | Lithium metasilicate | 1 | Lewis conjugate | Insoluble in water |
| H2SiO3 | Metasilicic acid | 1 | Lewis conjugate | Very slightly soluble in water |
| K2CO3 | Potassium carbonate | 2 | Non-redox product | – |
Thermodynamic changes
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 |
|---|---|---|---|---|
| LiHCO3 | – | – | – | – |
| 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 |
|---|---|---|---|---|
| Li2SiO3 (cr) | -1648.1[1] | -1557.2[1] | 79.83[1] | 99.08[1] |
| Li2SiO3 (vit) | -1628[1] | – | – | – |
| H2SiO3 (cr) | -1188.7[1] | -1092.4[1] | 134[1] | – |
| H2SiO3 (ao) | -1182.8[1] | -1079.4[1] | 109[1] | – |
| K2CO3 (cr) | -1151.02[1] | -1063.5[1] | 155.52[1] | 114.43[1] |
| K2CO3 (ai) | -1181.90[1] | -1094.36[1] | 148.1[1] | – |
| K2CO3 (cr) 1.5 hydrate | -1609.2[1] | -1432.5[1] | 203.3[1] | – |
* (cr):Crystalline solid, (vit):Vitreous liquid, (ao):Un-ionized aqueous solution, (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)
- ^ S°, 146.0 J · K−1 · mol−1
- ^ Cp°, 118.4 J · K−1 · mol−1
- ^ ΔfH°, -1648.1 kJ · mol−1
- ^ ΔfG°, -1557.2 kJ · mol−1
- ^ S°, 79.83 J · K−1 · mol−1
- ^ Cp°, 99.08 J · K−1 · mol−1
- ^ ΔfH°, -1628. kJ · mol−1
- ^ ΔfH°, -1188.7 kJ · mol−1
- ^ ΔfG°, -1092.4 kJ · mol−1
- ^ S°, 134. J · K−1 · mol−1
- ^ ΔfH°, -1182.8 kJ · mol−1
- ^ ΔfG°, -1079.4 kJ · mol−1
- ^ S°, 109. J · K−1 · mol−1
- ^ ΔfH°, -1151.02 kJ · mol−1
- ^ ΔfG°, -1063.5 kJ · mol−1
- ^ S°, 155.52 J · K−1 · mol−1
- ^ Cp°, 114.43 J · K−1 · mol−1
- ^ ΔfH°, -1181.90 kJ · mol−1
- ^ ΔfG°, -1094.36 kJ · mol−1
- ^ S°, 148.1 J · K−1 · mol−1
- ^ ΔfH°, -1609.2 kJ · mol−1
- ^ ΔfG°, -1432.5 kJ · mol−1
- ^ S°, 203.3 J · K−1 · mol−1