6H2S + 11K2SeO3 → 6KHSO4 + 8K2Se + 3H2SeO3
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The reaction of hydrogen sulfide and potassium selenite yields potassium hydrogensulfate, potassium selenide, and selenous acid (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 hydrogen sulfide 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 hydrogen sulfide and potassium selenite
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2S | Hydrogen sulfide | 6 | Reducing | Reducing |
| K2SeO3 | Potassium selenite | 11 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KHSO4 | Potassium hydrogensulfate | 6 | Oxidized | – |
| K2Se | Potassium selenide | 8 | Reduced | – |
| H2SeO3 | Selenous acid | 3 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen sulfide 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 | −771.2 | – | – | – |
per 1 mol of | −128.5 | – | – | – |
per 1 mol of | −70.11 | – | – | – |
per 1 mol of | −128.5 | – | – | – |
per 1 mol of | −96.40 | – | – | – |
per 1 mol of | −257.1 | – | – | – |
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and potassium selenite◆
ΔrG −544.8 kJ/mol K 2.79 × 1095 pK −95.44
| 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 | – | −544.8 | – | – |
per 1 mol of | – | −90.80 | – | – |
per 1 mol of | – | −49.53 | – | – |
per 1 mol of | – | −90.80 | – | – |
per 1 mol of | – | −68.10 | – | – |
per 1 mol of | – | −181.6 | – | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
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 |
|---|---|---|---|---|
| H2S (g) | -20.63[1] | -33.56[1] | 205.79[1] | 34.23[1] |
| H2S (ao) | -39.7[1] | -27.83[1] | 121[1] | – |
| K2SeO3 (cr) | -982.0[1] | – | – | – |
| K2SeO3 (ai) | -1013.8[1] | -936.3[1] | 218.0[1] | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| KHSO4 (cr) | -1160.6[1] | -1031.3[1] | 138.1[1] | – |
| KHSO4 (ai) | -1139.72[1] | -1039.18[1] | 234.3[1] | -63[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] | – | – | – |
| H2SeO3 (cr) | -524.46[1] | – | – | – |
| H2SeO3 (ao) | -507.48[1] | -426.14[1] | 207.9[1] | – |
| H2SeO3 (aq) | -507.27[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (aq):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°, -20.63 kJ · mol−1
- ^ ΔfG°, -33.56 kJ · mol−1
- ^ S°, 205.79 J · K−1 · mol−1
- ^ Cp°, 34.23 J · K−1 · mol−1
- ^ ΔfH°, -39.7 kJ · mol−1
- ^ ΔfG°, -27.83 kJ · mol−1
- ^ S°, 121. 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°, -1160.6 kJ · mol−1
- ^ ΔfG°, -1031.3 kJ · mol−1
- ^ S°, 138.1 J · K−1 · mol−1
- ^ ΔfH°, -1139.72 kJ · mol−1
- ^ ΔfG°, -1039.18 kJ · mol−1
- ^ S°, 234.3 J · K−1 · mol−1
- ^ Cp°, -63. J · K−1 · 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°, -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