6Na + 4K2SeO3 → 3Na2SeO3 + K2Se + 3K2O
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- Reaction of and potassium selenite
The reaction of and potassium selenite yields sodium selenite, potassium selenide, and potassium oxide (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 potassium selenite
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 potassium selenite
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
6 | Reducing | Reducing | ||
K2SeO3 | Potassium selenite | 4 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2SeO3 | Sodium selenite | 3 | Oxidized | – |
K2Se | Potassium selenide | 1 | Reduced | – |
K2O | Potassium oxide | 3 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and potassium selenite
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 | −427.3 | – | – | – |
−71.22 | – | – | – | |
per 1 mol of | −106.8 | – | – | – |
per 1 mol of | −142.4 | – | – | – |
per 1 mol of | −427.3 | – | – | – |
per 1 mol of | −142.4 | – | – | – |
Changes in aqueous solution
- Reaction of and potassium selenite◆
ΔrG −339.4 kJ/mol K 2.89 × 1059 pK −59.46
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 | – | −339.4 | – | – |
– | −56.57 | – | – | |
per 1 mol of | – | −84.85 | – | – |
per 1 mol of | – | −113.1 | – | – |
per 1 mol of | – | −339.4 | – | – |
per 1 mol of | – | −113.1 | – | – |
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] |
K2SeO3 (cr) | -982.0[1] | – | – | – |
K2SeO3 (ai) | -1013.8[1] | -936.3[1] | 218.0[1] | – |
* (cr):Crystalline solid, (g):Gas, (ai):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 |
---|---|---|---|---|
Na2SeO3 (cr) | -958.6[1] | – | – | – |
Na2SeO3 (ai) | -989.5[1] | -893.7[1] | 130[1] | – |
Na2SeO3 (cr) 5 hydrate | -2404.13[1] | – | – | – |
K2Se (cr) | -395.0[1] | – | – | – |
K2Se (ai) | – | -437.2[1] | – | – |
K2Se (cr) 9 hydrate | -3087.0[1] | – | – | – |
K2Se (cr) 14 hydrate | -4524.2[1] | – | – | – |
K2Se (cr) 19 hydrate | -5991.9[1] | – | – | – |
K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
K2O (g) | -63[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, -982.0 kJ · mol−1
- ^ ΔfH°, -1013.8 kJ · mol−1
- ^ ΔfG°, -936.3 kJ · mol−1
- ^ S°, 218.0 J · K−1 · mol−1
- ^ ΔfH°, -958.6 kJ · mol−1
- ^ ΔfH°, -989.5 kJ · mol−1
- ^ ΔfG°, -893.7 kJ · mol−1
- ^ S°, 130. J · K−1 · mol−1
- ^ ΔfH°, -2404.13 kJ · mol−1
- ^ ΔfH°, -395.0 kJ · mol−1
- ^ ΔfG°, -437.2 kJ · mol−1
- ^ ΔfH°, -3087.0 kJ · mol−1
- ^ ΔfH°, -4524.2 kJ · mol−1
- ^ ΔfH°, -5991.9 kJ · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · 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