2Na2SeO3 + O2 → 2Na2SeO4
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- Reaction of sodium selenite and
The reaction of sodium selenite and yields sodium selenate. This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of sodium selenite and
General equation
- Reaction of oxidizable species and oxidizing species
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of sodium selenite and
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2SeO3 | Sodium selenite | 2 | Reducing | Oxidizable |
1 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2SeO4 | Sodium selenate | 2 | Redoxed product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of sodium selenite and
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 | −220.8 | – | – | – |
per 1 mol of | −110.4 | – | – | – |
−220.8 | – | – | – | |
per 1 mol of | −110.4 | – | – | – |
Changes in aqueous solution
- Reaction of sodium selenite and ◆
ΔrG −159.4 kJ/mol K 8.43 × 1027 pK −27.93
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 | −168.3 | −159.4 | −27 | – |
per 1 mol of | −84.15 | −79.70 | −14 | – |
−168.3 | −159.4 | −27 | – | |
per 1 mol of | −84.15 | −79.70 | −14 | – |
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 |
---|---|---|---|---|
Na2SeO3 (cr) | -958.6[1] | – | – | – |
Na2SeO3 (ai) | -989.5[1] | -893.7[1] | 130[1] | – |
Na2SeO3 (cr) 5 hydrate | -2404.13[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, (ai):Ionized aqueous solution, (g):Gas, (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 |
---|---|---|---|---|
Na2SeO4 (cr) | -1069.0[1] | – | – | – |
Na2SeO4 (ai) | -1079.5[1] | -965.2[1] | 172.0[1] | – |
Na2SeO4 (cr) 10 hydrate | -4006.6[1] | – | – | – |
* (cr):Crystalline solid, (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)
- ^ 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°, 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
- ^ ΔfH°, -1069.0 kJ · mol−1
- ^ ΔfH°, -1079.5 kJ · mol−1
- ^ ΔfG°, -965.2 kJ · mol−1
- ^ S°, 172.0 J · K−1 · mol−1
- ^ ΔfH°, -4006.6 kJ · mol−1