4H2S + 3K2CO3 🔥→ SO2 + 3K2S + 3CO + 4H2O
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- Reaction of hydrogen sulfide and potassium carbonate
The reaction of hydrogen sulfide and potassium carbonate yields sulfur dioxide, potassium sulfide, carbon monoxide, 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 hydrogen sulfide and potassium carbonate
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 carbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2S | Hydrogen sulfide | 4 | Reducing | Reducing |
| K2CO3 | Potassium carbonate | 3 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SO2 | Sulfur dioxide | 1 | Oxidized | – |
| K2S | Potassium sulfide | 3 | – | – |
| CO | Carbon monoxide | 3 | Reduced | – |
| H2O | Water | 4 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen sulfide and potassium carbonate◆
ΔrG 572.5 kJ/mol K 0.50 × 10−100 pK 100.30
| 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 | 621.8 | 572.5 | 146 | – |
per 1 mol of | 155.4 | 143.1 | 36.5 | – |
per 1 mol of | 207.3 | 190.8 | 48.7 | – |
per 1 mol of | 621.8 | 572.5 | 146 | – |
per 1 mol of | 207.3 | 190.8 | 48.7 | – |
per 1 mol of | 207.3 | 190.8 | 48.7 | – |
per 1 mol of | 155.4 | 143.1 | 36.5 | – |
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and potassium carbonate◆
ΔrG 292.1 kJ/mol K 0.67 × 10−51 pK 51.17
| 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 | 518.3 | 292.1 | 764 | – |
per 1 mol of | 129.6 | 73.03 | 191 | – |
per 1 mol of | 172.8 | 97.37 | 255 | – |
per 1 mol of | 518.3 | 292.1 | 764 | – |
per 1 mol of | 172.8 | 97.37 | 255 | – |
per 1 mol of | 172.8 | 97.37 | 255 | – |
per 1 mol of | 129.6 | 73.03 | 191 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and potassium carbonate◆
ΔrG 343.9 kJ/mol K 0.56 × 10−60 pK 60.25
| 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 | 487.0 | 343.9 | 485 | – |
per 1 mol of | 121.8 | 85.97 | 121 | – |
per 1 mol of | 162.3 | 114.6 | 162 | – |
per 1 mol of | 487.0 | 343.9 | 485 | – |
per 1 mol of | 162.3 | 114.6 | 162 | – |
per 1 mol of | 162.3 | 114.6 | 162 | – |
per 1 mol of | 121.8 | 85.97 | 121 | – |
Changes in aqueous solution (3)
- Reaction of hydrogen sulfide and potassium carbonate◆
ΔrG 291.6 kJ/mol K 0.82 × 10−51 pK 51.09
| 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 | 492.1 | 291.6 | 677 | – |
per 1 mol of | 123.0 | 72.90 | 169 | – |
per 1 mol of | 164.0 | 97.20 | 226 | – |
per 1 mol of | 492.1 | 291.6 | 677 | – |
per 1 mol of | 164.0 | 97.20 | 226 | – |
per 1 mol of | 164.0 | 97.20 | 226 | – |
per 1 mol of | 123.0 | 72.90 | 169 | – |
Changes in aqueous solution (4)
- Reaction of hydrogen sulfide and potassium carbonate◆
ΔrG 343.4 kJ/mol K 0.69 × 10−60 pK 60.16
| 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 | 460.8 | 343.4 | 398 | – |
per 1 mol of | 115.2 | 85.85 | 99.5 | – |
per 1 mol of | 153.6 | 114.5 | 133 | – |
per 1 mol of | 460.8 | 343.4 | 398 | – |
per 1 mol of | 153.6 | 114.5 | 133 | – |
per 1 mol of | 153.6 | 114.5 | 133 | – |
per 1 mol of | 115.2 | 85.85 | 99.5 | – |
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] | – |
| K2CO3 (cr) | -1151.02[1] | -1063.5[1] | 155.52[1] | 114.43[1] |
| K2CO3 (ai) | -1181.90[1] | -1094.36[1] | 148.1[1] | – |
| K2CO3 (cr) 1.5 hydrate | -1609.2[1] | -1432.5[1] | 203.3[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 |
|---|---|---|---|---|
| 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] | – |
| K2S (cr) | -380.7[1] | -364.0[1] | 105[1] | – |
| K2S (ai) | -471.5[1] | -480.7[1] | 190.4[1] | – |
| K2S (cr) 2 hydrate | -975.3[1] | – | – | – |
| K2S (cr) 5 hydrate | -1871.5[1] | – | – | – |
| CO (g) | -110.525[1] | -137.168[1] | 197.674[1] | 29.142[1] |
| CO (ao) | -120.96[1] | -119.90[1] | 104.6[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] |
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (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°, -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°, -1151.02 kJ · mol−1
- ^ ΔfG°, -1063.5 kJ · mol−1
- ^ S°, 155.52 J · K−1 · mol−1
- ^ Cp°, 114.43 J · K−1 · mol−1
- ^ ΔfH°, -1181.90 kJ · mol−1
- ^ ΔfG°, -1094.36 kJ · mol−1
- ^ S°, 148.1 J · K−1 · mol−1
- ^ ΔfH°, -1609.2 kJ · mol−1
- ^ ΔfG°, -1432.5 kJ · mol−1
- ^ S°, 203.3 J · K−1 · 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°, -380.7 kJ · mol−1
- ^ ΔfG°, -364.0 kJ · mol−1
- ^ S°, 105. J · K−1 · mol−1
- ^ ΔfH°, -471.5 kJ · mol−1
- ^ ΔfG°, -480.7 kJ · mol−1
- ^ S°, 190.4 J · K−1 · mol−1
- ^ ΔfH°, -975.3 kJ · mol−1
- ^ ΔfH°, -1871.5 kJ · mol−1
- ^ ΔfH°, -110.525 kJ · mol−1
- ^ ΔfG°, -137.168 kJ · mol−1
- ^ S°, 197.674 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -120.96 kJ · mol−1
- ^ ΔfG°, -119.90 kJ · mol−1
- ^ S°, 104.6 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