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5H2S + Zn3(AsO4)2 → 2S + As2O3 + 3ZnS + 5H2O

The reaction of hydrogen sulfide and zinc arsenate yields sulfur, 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
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide5
Reducing
Reducing
Zn3(AsO4)2Zinc arsenate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
SSulfur2
Oxidized
As2O3Diarsenic trioxide1
Reduced
ZnSZinc sulfide3
H2OWater5

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and zinc arsenate
ΔrG−303 kJ/mol
K1.21 × 1053
pK−53.08
5H2SGas + Zn3(AsO4)2Crystalline solid
2SCrystalline 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
per 1 mol of
−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
K1.81 × 1053
pK−53.26
5H2SGas + Zn3(AsO4)2Crystalline solid
2SCrystalline 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
per 1 mol of
−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 solid
2SCrystalline 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
per 1 mol of

Changes in standard condition (4)

Reaction of hydrogen sulfide and zinc arsenate
5H2SGas + Zn3(AsO4)2Crystalline solid
2SCrystalline 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
per 1 mol of

Changes in aqueous solution

Reaction of hydrogen sulfide and zinc arsenate
5H2SUn-ionized aqueous solution + Zn3(AsO4)2Crystalline solid
2SCrystalline 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
per 1 mol of

Thermodynamic data of reactants

Chemical formulaStandard 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 formulaStandard 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
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]
S (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

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)