2Na + 2Sn(OH)4 → Na2SnO3 + Sn(OH)2 + 3H2O
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- Reaction of and tin(IV) hydroxide
The reaction of and tin(IV) hydroxide yields sodium metastannate, tin(II) hydroxide, and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and tin(IV) hydroxide
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and tin(IV) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 2 | Reducing | Reducing | ||
| Sn(OH)4 | Tin(IV) hydroxide | 2 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2SnO3 | Sodium metastannate | 1 | Oxidized | – |
| Sn(OH)2 | Tin(II) hydroxide | 1 | Reduced | – |
| H2O | Water | 3 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and tin(IV) hydroxide
| 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 | −354 | – | – | – |
| −177 | – | – | – | |
per 1 mol of | −177 | – | – | – |
per 1 mol of | −354 | – | – | – |
per 1 mol of | −354 | – | – | – |
per 1 mol of | −118 | – | – | – |
Changes in aqueous solution
- Reaction of and tin(IV) hydroxide
| 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 | −354 | – | – | – |
| −177 | – | – | – | |
per 1 mol of | −177 | – | – | – |
per 1 mol of | −354 | – | – | – |
per 1 mol of | −354 | – | – | – |
per 1 mol of | −118 | – | – | – |
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 51.21[1] | 28.24[1] |
| (g) | 107.32[1] | 76.761[1] | 153.712[1] | 20.786[1] |
| Sn(OH)4 (cr) precipitated | -1110.0[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas
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 |
|---|---|---|---|---|
| Na2SnO3 (cr) | -1155[1] | – | – | – |
| Sn(OH)2 (cr) precipitated | -561.1[1] | -491.6[1] | 155[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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 51.21 J · K−1 · mol−1
- ^ Cp°, 28.24 J · K−1 · mol−1
- ^ ΔfH°, 107.32 kJ · mol−1
- ^ ΔfG°, 76.761 kJ · mol−1
- ^ S°, 153.712 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -1110.0 kJ · mol−1
- ^ ΔfH°, -1155. kJ · mol−1
- ^ ΔfH°, -561.1 kJ · mol−1
- ^ ΔfG°, -491.6 kJ · mol−1
- ^ S°, 155. J · K−1 · 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