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23H2S + 6K3AsO4 🔥→ 5SO2 + 6As + 18KHS + 14H2O

The reaction of hydrogen sulfide and potassium arsenate yields sulfur dioxide, arsenic, potassium hydrogensulfide, 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 sulfide23
Reducing
Reducing
K3AsO4Potassium arsenate6
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide5
Oxidized
AsArsenic6
Reduced
KHSPotassium hydrogensulfide18
H2OWater14

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and potassium arsenate
ΔrG−72.73 kJ/mol
K5.52 × 1012
pK−12.74
23H2SUn-ionized aqueous solution + 6K3AsO4Ionized aqueous solution
🔥
5SO2Gas + 6AsCrystalline solidα, gray, metallic + 18KHSIonized aqueous solution + 14H2OLiquid
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
440.8−72.731754
per 1 mol of
19.17−3.16276.26
per 1 mol of
73.47−12.12292.3
per 1 mol of
88.16−14.55350.8
per 1 mol of
73.47−12.12292.3
24.49−4.04197.44
per 1 mol of
31.49−5.195125.3

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and potassium arsenate
ΔrG−75.14 kJ/mol
K1.46 × 1013
pK−13.16
23H2SUn-ionized aqueous solution + 6K3AsO4Ionized aqueous solution
🔥
5SO2Un-ionized aqueous solution + 6AsCrystalline solidα, gray, metallic + 18KHSIonized aqueous solution + 14H2OLiquid
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
310.0−75.141322
per 1 mol of
13.48−3.26757.48
per 1 mol of
51.67−12.52220.3
per 1 mol of
62.00−15.03264.4
per 1 mol of
51.67−12.52220.3
17.22−4.17473.44
per 1 mol of
22.14−5.36794.43

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]
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 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
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]
As (cr)
α, gray, metallic
0[1]0[1]35.1[1]24.64[1]
As (cr)
γ, yellow, cubic
14.6[1]
As (am)
β
4.2[1]
As (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

  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)