5H2S + Zn3(AsO4)2 → 2S + As2O3 + 3ZnS + 5H2O
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- Reaction of hydrogen sulfide and zinc arsenate
The reaction of hydrogen sulfide and zinc arsenate yields , diarsenic trioxide, zinc 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 zinc 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 zinc arsenate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
H2S | Hydrogen sulfide | 5 | Reducing | Reducing |
Zn3(AsO4)2 | Zinc arsenate | 1 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
2 | Oxidized | – | ||
As2O3 | Diarsenic trioxide | 1 | Reduced | – |
ZnS | Zinc sulfide | 3 | – | – |
H2O | Water | 5 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen sulfide and zinc arsenate◆
ΔrG −303 kJ/mol K 1.21 × 1053 pK −53.08 - 5H2SGas + Zn3(AsO4)2Crystalline solid2Crystalline solidrhombic + As2O3Crystalline solidoctahedral + 3ZnSCrystalline solid + 5H2OLiquid⟶
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 | – | −303 | – | – |
per 1 mol of | – | −60.6 | – | – |
per 1 mol of | – | −303 | – | – |
– | −152 | – | – | |
per 1 mol of | – | −303 | – | – |
per 1 mol of | – | −101 | – | – |
per 1 mol of | – | −60.6 | – | – |
Changes in standard condition (2)
- Reaction of hydrogen sulfide and zinc arsenate◆
ΔrG −304 kJ/mol K 1.81 × 1053 pK −53.26 - 5H2SGas + Zn3(AsO4)2Crystalline solid2Crystalline solidrhombic + As2O3Crystalline solidmonoclinic + 3ZnSCrystalline solid + 5H2OLiquid⟶
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 | – | −304 | – | – |
per 1 mol of | – | −60.8 | – | – |
per 1 mol of | – | −304 | – | – |
– | −152 | – | – | |
per 1 mol of | – | −304 | – | – |
per 1 mol of | – | −101 | – | – |
per 1 mol of | – | −60.8 | – | – |
Changes in standard condition (3)
- Reaction of hydrogen sulfide and zinc arsenate
- 5H2SGas + Zn3(AsO4)2Crystalline solid2Crystalline solidmonoclinic + As2O3Crystalline solidoctahedral + 3ZnSCrystalline solid + 5H2OLiquid⟶
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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
– | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in standard condition (4)
- Reaction of hydrogen sulfide and zinc arsenate
- 5H2SGas + Zn3(AsO4)2Crystalline solid2Crystalline solidmonoclinic + As2O3Crystalline solidmonoclinic + 3ZnSCrystalline solid + 5H2OLiquid⟶
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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
– | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution
- Reaction of hydrogen sulfide and zinc arsenate
- 5H2SUn-ionized aqueous solution + Zn3(AsO4)2Crystalline solid2Crystalline solidrhombic + As2O3Aqueous solution + 3ZnSCrystalline solid + 5H2OLiquid⟶
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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
– | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
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] | – |
Zn3(AsO4)2 (cr) | – | -1895[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 |
---|---|---|---|---|
(cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
(cr) monoclinic | 0.33[1] | – | – | – |
(g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
As2O3 (cr) octahedral | -656.97[1] | -576.22[1] | 107.1[1] | 95.65[1] |
As2O3 (cr) monoclinic | -654.8[1] | -576.97[1] | 117[1] | – |
As2O3 (g) | -604.6[1] | -548.9[1] | 191[1] | – |
As2O3 (aq) | -626.8[1] | – | – | – |
ZnS (cr) | -205.98[1] | -201.29[1] | 57.7[1] | 46.0[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] |
* (cr):Crystalline solid, (g):Gas, (aq):Aqueous solution, (l):Liquid
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
- ^ ΔfG°, -1895. kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, -656.97 kJ · mol−1
- ^ ΔfG°, -576.22 kJ · mol−1
- ^ S°, 107.1 J · K−1 · mol−1
- ^ Cp°, 95.65 J · K−1 · mol−1
- ^ ΔfH°, -654.8 kJ · mol−1
- ^ ΔfG°, -576.97 kJ · mol−1
- ^ S°, 117 J · K−1 · mol−1
- ^ ΔfH°, -604.6 kJ · mol−1
- ^ ΔfG°, -548.9 kJ · mol−1
- ^ S°, 191 J · K−1 · mol−1
- ^ ΔfH°, -626.8 kJ · mol−1
- ^ ΔfH°, -205.98 kJ · mol−1
- ^ ΔfG°, -201.29 kJ · mol−1
- ^ S°, 57.7 J · K−1 · mol−1
- ^ Cp°, 46.0 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