26H2S + 6(NH4)3AsO4 🔥→ 8H2SO3 + 3As2S3 + 9(NH4)2S + 18H2
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- Reaction of hydrogen sulfide and ammonium arsenate
- 26H2SHydrogen sulfide + 6(NH4)3AsO4Ammonium arsenate8H2SO3Sulfurous acid + 3 + 9(NH4)2SAmmonium sulfide + 18🔥⟶
The reaction of hydrogen sulfide and ammonium arsenate yields sulfurous acid, , ammonium sulfide, and (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 ammonium arsenate
- 26H2SHydrogen sulfide + 6(NH4)3AsO4Ammonium arsenate8H2SO3Sulfurous acid + 3 + 9(NH4)2SAmmonium sulfide + 18🔥⟶
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 ammonium arsenate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2S | Hydrogen sulfide | 26 | Reducing | Reducing |
| (NH4)3AsO4 | Ammonium arsenate | 6 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2SO3 | Sulfurous acid | 8 | Oxidized | – |
| 3 | Reduced | – | ||
| (NH4)2S | Ammonium sulfide | 9 | – | – |
| 18 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and ammonium arsenate◆
ΔrG 579.8 kJ/mol K 0.27 × 10−101 pK 101.58 - 26H2SUn-ionized aqueous solution + 6(NH4)3AsO4Ionized aqueous solution8H2SO3Un-ionized aqueous solution + 3Crystalline solid + 9(NH4)2SIonized aqueous solution + 18Gas🔥⟶
| 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 | 1282.5 | 579.8 | 2399 | – |
per 1 mol of | 49.327 | 22.30 | 92.27 | – |
per 1 mol of | 213.75 | 96.63 | 399.8 | – |
per 1 mol of | 160.31 | 72.47 | 299.9 | – |
| 427.50 | 193.3 | 799.7 | – | |
per 1 mol of | 142.50 | 64.42 | 266.6 | – |
| 71.250 | 32.21 | 133.3 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and ammonium arsenate◆
ΔrG 896.6 kJ/mol K 0.84 × 10−157 pK 157.08 - 26H2SUn-ionized aqueous solution + 6(NH4)3AsO4Ionized aqueous solution8H2SO3Un-ionized aqueous solution + 3Crystalline solid + 9(NH4)2SIonized aqueous solution + 18Un-ionized aqueous solution🔥⟶
| 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 | 1206.9 | 896.6 | 10433 | – |
per 1 mol of | 46.419 | 34.48 | 401.27 | – |
per 1 mol of | 201.15 | 149.4 | 1738.8 | – |
per 1 mol of | 150.86 | 112.1 | 1304.1 | – |
| 402.30 | 298.9 | 3477.7 | – | |
per 1 mol of | 134.10 | 99.62 | 1159.2 | – |
| 67.050 | 49.81 | 579.61 | – |
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] | – |
| (NH4)3AsO4 (cr) | -1286.2[1] | – | – | – |
| (NH4)3AsO4 (ai) | -1285.66[1] | -886.32[1] | 177.4[1] | – |
| (NH4)3AsO4 (cr) 3 hydrate | -2166.9[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 |
|---|---|---|---|---|
| H2SO3 (ao) | -608.81[1] | -537.81[1] | 232.2[1] | – |
| (cr) | -169.0[1] | -168.6[1] | 163.6[1] | 116.3[1] |
| (NH4)2S (ai) | -231.8[1] | -72.6[1] | 212.1[1] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas
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°, -1286.2 kJ · mol−1
- ^ ΔfH°, -1285.66 kJ · mol−1
- ^ ΔfG°, -886.32 kJ · mol−1
- ^ S°, 177.4 J · K−1 · mol−1
- ^ ΔfH°, -2166.9 kJ · mol−1
- ^ ΔfH°, -608.81 kJ · mol−1
- ^ ΔfG°, -537.81 kJ · mol−1
- ^ S°, 232.2 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°, -231.8 kJ · mol−1
- ^ ΔfG°, -72.6 kJ · mol−1
- ^ S°, 212.1 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1