FeOH+ + HSiO3− → FeSiO3↓ + H2O
Last updated:
- Reaction of iron(II) hydroxide ion and hydrogenmetasilicate ion
- FeOH+Iron(II) hydroxide ion + HSiO3−Hydrogenmetasilicate ionFeSiO3↓Iron(II) metasilicate + H2OWater⟶
The reaction of iron(II) hydroxide ion and hydrogenmetasilicate ion yields iron(II) metasilicate and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(II) hydroxide ion and hydrogenmetasilicate ion
- FeOH+Iron(II) hydroxide ion + HSiO3−Hydrogenmetasilicate ionFeSiO3↓Iron(II) metasilicate + H2OWater⟶
General equation
- Reaction of cation and anion
- CationLewis acid + AnionLewis base ⟶ ProductLewis conjugate + (H2O)
- Precipitation reaction of cation and anion
- CationLewis acid + AnionLewis base ⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + (H2O)
Oxidation state of each atom
- Reaction of iron(II) hydroxide ion and hydrogenmetasilicate ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeOH+ | Iron(II) hydroxide ion | 1 | Lewis acid | Cation |
| HSiO3− | Hydrogenmetasilicate ion | 1 | Lewis base | Anion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeSiO3 | Iron(II) metasilicate | 1 | Lewis conjugate | – Insoluble in water |
| H2O | Water | 1 | – | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of iron(II) hydroxide ion and hydrogenmetasilicate ion
| 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 | −19 | – | – | – |
per 1 mol of Iron(II) hydroxide ion | −19 | – | – | – |
per 1 mol of Hydrogenmetasilicate ion | −19 | – | – | – |
per 1 mol of | −19 | – | – | – |
per 1 mol of | −19 | – | – | – |
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 |
|---|---|---|---|---|
| FeOH+ (ao) | -324.7[1] | -277.4[1] | -29[1] | – |
| HSiO3− (ao) | -1147.253[2] | -1016.026[2] | 16.74[2] | – |
* (ao):Un-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 |
|---|---|---|---|---|
| FeSiO3 (cr) | -1205[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] |
* (cr):Crystalline solid, (l):Liquid, (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°, -324.7 kJ · mol−1
- ^ ΔfG°, -277.4 kJ · mol−1
- ^ S°, -29. J · K−1 · mol−1
- ^ ΔfH°, -1205. kJ · 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
- 2Colin Stuart Walker, Anraku Sohtaro, Oda Chie, Mitsui Seiichiro, Mihara MorihiroThermodynamic properties of SiO2(aq), HSiO3– and SiO3-2Japan Atomic Energy Agency