3H2 + H2SeO3 → H2Se + 3H2O
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- Reaction of and selenous acid
The reaction of and selenous acid yields hydrogen selenide 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 selenous acid
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 selenous acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 3 | Reducing | Reducing | ||
| H2SeO3 | Selenous acid | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2Se | Hydrogen selenide | 1 | Reduced | – |
| H2O | Water | 3 | Oxidized | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and selenous acid
| 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 | −303.3 | – | – | – |
| −101.1 | – | – | – | |
per 1 mol of | −303.3 | – | – | – |
per 1 mol of | −303.3 | – | – | – |
per 1 mol of | −101.1 | – | – | – |
Changes in aqueous solution (1)
- Reaction of and selenous acid◆
ΔrG −322.1 kJ/mol K 2.69 × 1056 pK −56.43
| 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 | −307.7 | −322.1 | −1510 | – |
| −102.6 | −107.4 | −503.3 | – | |
per 1 mol of | −307.7 | −322.1 | −1510 | – |
per 1 mol of | −307.7 | −322.1 | −1510 | – |
per 1 mol of | −102.6 | −107.4 | −503.3 | – |
Changes in aqueous solution (2)
- Reaction of and selenous acid◆
ΔrG −315.8 kJ/mol K 2.12 × 1055 pK −55.33
| 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 | −318.2 | −315.8 | −1566 | – |
| −106.1 | −105.3 | −522.0 | – | |
per 1 mol of | −318.2 | −315.8 | −1566 | – |
per 1 mol of | −318.2 | −315.8 | −1566 | – |
per 1 mol of | −106.1 | −105.3 | −522.0 | – |
Changes in aqueous solution (3)
- Reaction of and selenous acid
| 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 | −307.9 | – | – | – |
| −102.6 | – | – | – | |
per 1 mol of | −307.9 | – | – | – |
per 1 mol of | −307.9 | – | – | – |
per 1 mol of | −102.6 | – | – | – |
Changes in aqueous solution (4)
- Reaction of and selenous acid
| 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 | −318.4 | – | – | – |
| −106.1 | – | – | – | |
per 1 mol of | −318.4 | – | – | – |
per 1 mol of | −318.4 | – | – | – |
per 1 mol of | −106.1 | – | – | – |
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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
| H2SeO3 (cr) | -524.46[1] | – | – | – |
| H2SeO3 (ao) | -507.48[1] | -426.14[1] | 207.9[1] | – |
| H2SeO3 (aq) | -507.27[1] | – | – | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (aq):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 |
|---|---|---|---|---|
| H2Se (g) | 29.7[1] | 15.9[1] | 219.02[1] | 34.73[1] |
| H2Se (ao) | 19.2[1] | 22.2[1] | 163.6[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] |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid
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°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1
- ^ ΔfH°, -524.46 kJ · mol−1
- ^ ΔfH°, -507.48 kJ · mol−1
- ^ ΔfG°, -426.14 kJ · mol−1
- ^ S°, 207.9 J · K−1 · mol−1
- ^ ΔfH°, -507.27 kJ · mol−1
- ^ ΔfH°, 29.7 kJ · mol−1
- ^ ΔfG°, 15.9 kJ · mol−1
- ^ S°, 219.02 J · K−1 · mol−1
- ^ Cp°, 34.73 J · K−1 · mol−1
- ^ ΔfH°, 19.2 kJ · mol−1
- ^ ΔfG°, 22.2 kJ · mol−1
- ^ S°, 163.6 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