H2S + 5KClO2 → K2SO3 + 3KClO + 2HClO2
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The reaction of hydrogen sulfide and potassium chlorite yields potassium sulfite, potassium hypochlorite, and chlorous 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 chlorite
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of hydrogen sulfide and potassium chlorite
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2S | Hydrogen sulfide | 1 | Reducing | Reducing |
| KClO2 | Potassium chlorite | 5 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2SO3 | Potassium sulfite | 1 | Oxidized | – |
| KClO | Potassium hypochlorite | 3 | Reduced | – |
| HClO2 | Chlorous acid | 2 | – | – |
Thermodynamic changes
Changes in aqueous solution
- Reaction of hydrogen sulfide and potassium chlorite◆
ΔrG −643.0 kJ/mol K 4.45 × 10112 pK −112.65
| 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 | −688.4 | −643.0 | −149 | – |
per 1 mol of | −688.4 | −643.0 | −149 | – |
per 1 mol of | −137.7 | −128.6 | −29.8 | – |
per 1 mol of | −688.4 | −643.0 | −149 | – |
per 1 mol of | −229.5 | −214.3 | −49.7 | – |
per 1 mol of | −344.2 | −321.5 | −74.5 | – |
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] | – |
| KClO2 (ai) | -318.8[1] | -266.1[1] | 203.8[1] | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (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 |
|---|---|---|---|---|
| K2SO3 (cr) | -1125.5[1] | – | – | – |
| K2SO3 (ai) | -1140.1[1] | -1053.1[1] | 176[1] | – |
| KClO (ai) | -359.4[1] | -320.0[1] | 146[1] | – |
| HClO2 (ao) | -51.9[1] | 5.9[1] | 188.3[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, -318.8 kJ · mol−1
- ^ ΔfG°, -266.1 kJ · mol−1
- ^ S°, 203.8 J · K−1 · mol−1
- ^ ΔfH°, -1125.5 kJ · mol−1
- ^ ΔfH°, -1140.1 kJ · mol−1
- ^ ΔfG°, -1053.1 kJ · mol−1
- ^ S°, 176. J · K−1 · mol−1
- ^ ΔfH°, -359.4 kJ · mol−1
- ^ ΔfG°, -320.0 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1
- ^ ΔfH°, -51.9 kJ · mol−1
- ^ ΔfG°, 5.9 kJ · mol−1
- ^ S°, 188.3 J · K−1 · mol−1