8H2S + 6CsClO3 → 5SO2 + 3Cl2 + 3Cs2S + 8H2O
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- Reaction of hydrogen sulfide and caesium chlorate
The reaction of hydrogen sulfide and caesium chlorate yields sulfur dioxide, , caesium sulfide, 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 caesium chlorate
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 caesium chlorate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2S | Hydrogen sulfide | 8 | Reducing | Reducing |
| CsClO3 | Caesium chlorate | 6 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SO2 | Sulfur dioxide | 5 | Oxidized | – |
| 3 | Reduced | – | ||
| Cs2S | Caesium sulfide | 3 | – | – |
| H2O | Water | 8 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen sulfide and caesium chlorate
| 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 | −2215.0 | – | – | – |
per 1 mol of | −276.88 | – | – | – |
per 1 mol of | −369.17 | – | – | – |
per 1 mol of | −443.00 | – | – | – |
| −738.33 | – | – | – | |
per 1 mol of | −738.33 | – | – | – |
per 1 mol of | −276.88 | – | – | – |
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and caesium chlorate◆
ΔrG −2870.4 kJ/mol K 7.45 × 10502 pK −502.87
| 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 | −2730.8 | −2870.4 | 484 | – |
per 1 mol of | −341.35 | −358.80 | 60.5 | – |
per 1 mol of | −455.13 | −478.40 | 80.7 | – |
per 1 mol of | −546.16 | −574.08 | 96.8 | – |
| −910.27 | −956.80 | 161 | – | |
per 1 mol of | −910.27 | −956.80 | 161 | – |
per 1 mol of | −341.35 | −358.80 | 60.5 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and caesium chlorate◆
ΔrG −2849.6 kJ/mol K 1.69 × 10499 pK −499.23
| 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 | −2801.0 | −2849.6 | 177 | – |
per 1 mol of | −350.13 | −356.20 | 22.1 | – |
per 1 mol of | −466.83 | −474.93 | 29.5 | – |
per 1 mol of | −560.20 | −569.92 | 35.4 | – |
| −933.67 | −949.87 | 59.0 | – | |
per 1 mol of | −933.67 | −949.87 | 59.0 | – |
per 1 mol of | −350.13 | −356.20 | 22.1 | – |
Changes in aqueous solution (3)
- Reaction of hydrogen sulfide and caesium chlorate◆
ΔrG −2872.9 kJ/mol K 2.04 × 10503 pK −503.31
| 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 | −2861.5 | −2872.9 | 52 | – |
per 1 mol of | −357.69 | −359.11 | 6.5 | – |
per 1 mol of | −476.92 | −478.82 | 8.7 | – |
per 1 mol of | −572.30 | −574.58 | 10 | – |
| −953.83 | −957.63 | 17 | – | |
per 1 mol of | −953.83 | −957.63 | 17 | – |
per 1 mol of | −357.69 | −359.11 | 6.5 | – |
Changes in aqueous solution (4)
- Reaction of hydrogen sulfide and caesium chlorate◆
ΔrG −2852.0 kJ/mol K 4.45 × 10499 pK −499.65
| 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 | −2931.7 | −2852.0 | −254 | – |
per 1 mol of | −366.46 | −356.50 | −31.8 | – |
per 1 mol of | −488.62 | −475.33 | −42.3 | – |
per 1 mol of | −586.34 | −570.40 | −50.8 | – |
| −977.23 | −950.67 | −84.7 | – | |
per 1 mol of | −977.23 | −950.67 | −84.7 | – |
per 1 mol of | −366.46 | −356.50 | −31.8 | – |
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] | – |
| CsClO3 (cr) | -411.7[1] | -307.9[1] | 156.1[1] | – |
| CsClO3 (ai) | -362.25[1] | -299.97[1] | 295.4[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] | – |
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[1] | – |
| Cs2S (cr) | -359.8[1] | – | – | – |
| Cs2S (ai) | -483.7[1] | -498.3[1] | 251.5[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°, -411.7 kJ · mol−1
- ^ ΔfG°, -307.9 kJ · mol−1
- ^ S°, 156.1 J · K−1 · mol−1
- ^ ΔfH°, -362.25 kJ · mol−1
- ^ ΔfG°, -299.97 kJ · mol−1
- ^ S°, 295.4 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ ΔfH°, -359.8 kJ · mol−1
- ^ ΔfH°, -483.7 kJ · mol−1
- ^ ΔfG°, -498.3 kJ · mol−1
- ^ S°, 251.5 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