20H2S + 3Mg3(AsO4)2 → 2SO2 + 3As2S3 + 9MgS + 20H2O
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- Reaction of hydrogen sulfide and magnesium arsenate
The reaction of hydrogen sulfide and magnesium arsenate yields sulfur dioxide, , magnesium 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 magnesium 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 magnesium arsenate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2S | Hydrogen sulfide | 20 | Reducing | Reducing |
| Mg3(AsO4)2 | Magnesium arsenate | 3 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SO2 | Sulfur dioxide | 2 | Oxidized | – |
| 3 | Reduced | – | ||
| MgS | Magnesium sulfide | 9 | – | – |
| H2O | Water | 20 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen sulfide and magnesium arsenate
- 20H2SGas + 3Mg3(AsO4)2Crystalline solid2SO2Gas + 3Crystalline solid + 9MgSCrystalline solid + 20H2OLiquid⟶
| 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 | −240.3 | – | – | – |
per 1 mol of | −12.02 | – | – | – |
per 1 mol of | −80.10 | – | – | – |
per 1 mol of | −120.2 | – | – | – |
| −80.10 | – | – | – | |
per 1 mol of | −26.70 | – | – | – |
per 1 mol of | −12.02 | – | – | – |
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and magnesium arsenate
- 20H2SUn-ionized aqueous solution + 3Mg3(AsO4)2Crystalline solid2SO2Gas + 3Crystalline solid + 9MgSCrystalline solid + 20H2OLiquid⟶
| 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 | 141.1 | – | – | – |
per 1 mol of | 7.055 | – | – | – |
per 1 mol of | 47.03 | – | – | – |
per 1 mol of | 70.55 | – | – | – |
| 47.03 | – | – | – | |
per 1 mol of | 15.68 | – | – | – |
per 1 mol of | 7.055 | – | – | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and magnesium arsenate
- 20H2SUn-ionized aqueous solution + 3Mg3(AsO4)2Crystalline solid2SO2Un-ionized aqueous solution + 3Crystalline solid + 9MgSCrystalline solid + 20H2OLiquid⟶
| 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 | 88.8 | – | – | – |
per 1 mol of | 4.44 | – | – | – |
per 1 mol of | 29.6 | – | – | – |
per 1 mol of | 44.4 | – | – | – |
| 29.6 | – | – | – | |
per 1 mol of | 9.87 | – | – | – |
per 1 mol of | 4.44 | – | – | – |
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] | – |
| Mg3(AsO4)2 (cr) | -3092.8[1] | – | – | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid
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) | -169.0[1] | -168.6[1] | 163.6[1] | 116.3[1] |
| MgS (cr) | -346.0[1] | -341.8[1] | 50.33[1] | 45.56[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
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°, -3092.8 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°, -169.0 kJ · mol−1
- ^ ΔfG°, -168.6 kJ · mol−1
- ^ S°, 163.6 J · K−1 · mol−1
- ^ Cp°, 116.3 J · K−1 · mol−1
- ^ ΔfH°, -346.0 kJ · mol−1
- ^ ΔfG°, -341.8 kJ · mol−1
- ^ S°, 50.33 J · K−1 · mol−1
- ^ Cp°, 45.56 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