23H2S + 6K3AsO4 🔥→ 5SO2 + 6As + 18KHS + 14H2O
Last updated:
- Reaction of hydrogen sulfide and potassium arsenate
The reaction of hydrogen sulfide and potassium arsenate yields sulfur dioxide, , potassium hydrogensulfide, 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 arsenate
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 arsenate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
H2S | Hydrogen sulfide | 23 | Reducing | Reducing |
K3AsO4 | Potassium arsenate | 6 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
SO2 | Sulfur dioxide | 5 | Oxidized | – |
6 | Reduced | – | ||
KHS | Potassium hydrogensulfide | 18 | – | – |
H2O | Water | 14 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and potassium arsenate◆
ΔrG −72.73 kJ/mol K 5.52 × 1012 pK −12.74
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 | 440.8 | −72.73 | 1754 | – |
per 1 mol of | 19.17 | −3.162 | 76.26 | – |
per 1 mol of | 73.47 | −12.12 | 292.3 | – |
per 1 mol of | 88.16 | −14.55 | 350.8 | – |
73.47 | −12.12 | 292.3 | – | |
per 1 mol of | 24.49 | −4.041 | 97.44 | – |
per 1 mol of | 31.49 | −5.195 | 125.3 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and potassium arsenate◆
ΔrG −75.14 kJ/mol K 1.46 × 1013 pK −13.16
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 | 310.0 | −75.14 | 1322 | – |
per 1 mol of | 13.48 | −3.267 | 57.48 | – |
per 1 mol of | 51.67 | −12.52 | 220.3 | – |
per 1 mol of | 62.00 | −15.03 | 264.4 | – |
51.67 | −12.52 | 220.3 | – | |
per 1 mol of | 17.22 | −4.174 | 73.44 | – |
per 1 mol of | 22.14 | −5.367 | 94.43 | – |
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] | – |
K3AsO4 (ai) | -1645.27[1] | -1498.23[1] | 144.8[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 |
---|---|---|---|---|
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] | – |
(cr) α, gray, metallic | 0[1] | 0[1] | 35.1[1] | 24.64[1] |
(cr) γ, yellow, cubic | 14.6[1] | – | – | – |
(am) β | 4.2[1] | – | – | – |
(g) | 302.5[1] | 261.0[1] | 174.21[1] | 20.786[1] |
KHS (cr) | -265.10[1] | – | – | 75.31[1] |
KHS (ai) | -269.9[1] | -271.19[1] | 165.3[1] | – |
KHS (cr) 0.25 hydrate | -337.2[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, (am):Amorphous 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°, -1645.27 kJ · mol−1
- ^ ΔfG°, -1498.23 kJ · mol−1
- ^ S°, 144.8 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°, 35.1 J · K−1 · mol−1
- ^ Cp°, 24.64 J · K−1 · mol−1
- ^ ΔfH°, 14.6 kJ · mol−1
- ^ ΔfH°, 4.2 kJ · mol−1
- ^ ΔfH°, 302.5 kJ · mol−1
- ^ ΔfG°, 261.0 kJ · mol−1
- ^ S°, 174.21 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -265.10 kJ · mol−1
- ^ Cp°, 75.31 J · K−1 · mol−1
- ^ ΔfH°, -269.9 kJ · mol−1
- ^ ΔfG°, -271.19 kJ · mol−1
- ^ S°, 165.3 J · K−1 · mol−1
- ^ ΔfH°, -337.2 kJ · 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