H2S + SeO2 → SO2 + H2Se
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The reaction of hydrogen sulfide and selenium dioxide yields sulfur dioxide and hydrogen selenide (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 selenium dioxide
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 selenium dioxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
H2S | Hydrogen sulfide | 1 | Reducing | Reducing |
SeO2 | Selenium dioxide | 1 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
SO2 | Sulfur dioxide | 1 | Oxidized | – |
H2Se | Hydrogen selenide | 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen sulfide and selenium dioxide
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 | −21.2 | – | – | – |
per 1 mol of | −21.2 | – | – | – |
per 1 mol of | −21.2 | – | – | – |
per 1 mol of | −21.2 | – | – | – |
per 1 mol of | −21.2 | – | – | – |
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and selenium dioxide
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 | −5.8 | – | – | – |
per 1 mol of | −5.8 | – | – | – |
per 1 mol of | −5.8 | – | – | – |
per 1 mol of | −5.8 | – | – | – |
per 1 mol of | −5.8 | – | – | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and selenium dioxide
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 | −16.3 | – | – | – |
per 1 mol of | −16.3 | – | – | – |
per 1 mol of | −16.3 | – | – | – |
per 1 mol of | −16.3 | – | – | – |
per 1 mol of | −16.3 | – | – | – |
Changes in aqueous solution (3)
- Reaction of hydrogen sulfide and selenium dioxide
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 | −32.0 | – | – | – |
per 1 mol of | −32.0 | – | – | – |
per 1 mol of | −32.0 | – | – | – |
per 1 mol of | −32.0 | – | – | – |
per 1 mol of | −32.0 | – | – | – |
Changes in aqueous solution (4)
- Reaction of hydrogen sulfide and selenium dioxide
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 | −42.5 | – | – | – |
per 1 mol of | −42.5 | – | – | – |
per 1 mol of | −42.5 | – | – | – |
per 1 mol of | −42.5 | – | – | – |
per 1 mol of | −42.5 | – | – | – |
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] | – |
SeO2 (cr) | -225.35[1] | – | – | – |
SeO2 (aq) | -221.63[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 |
---|---|---|---|---|
SO2 (l) | -320.5[1] | – | – | – |
SO2 (g) | -296.830[1] | -300.194[1] | 248.22[1] | 39.87[1] |
SO2 (ao) | -322.980[1] | -300.676[1] | 161.9[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] | – |
* (l):Liquid, (g):Gas, (ao):Un-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°, -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°, -225.35 kJ · mol−1
- ^ ΔfH°, -221.63 kJ · mol−1
- ^ ΔfH°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 J · K−1 · 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