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4S + 3H2SeO3 → H2S2O3 + 2H2S↑ + 3SeO2

The reaction of sulfur and selenous acid yields thiosulfuric acid, hydrogen sulfide, and selenium dioxide (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 self redoxing species and acid
Self-redoxing speciesSelf redox agent + AcidNon-redox agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of sulfur and selenous acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
SSulfur4
Self redoxing
H2SeO3Selenous acid3
Acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
H2S2O3Thiosulfuric acid1
Redoxed product
H2SHydrogen sulfide2
Reduced
SeO2Selenium dioxide3

Thermodynamic changes

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
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]
H2SeO3 (cr)-524.46[1]
H2SeO3 (ao)-507.48[1]-426.14[1]207.9[1]
H2SeO3 (aq)-507.27[1]
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (aq):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
H2S2O3
H2S (g)-20.63[1]-33.56[1]205.79[1]34.23[1]
H2S (ao)-39.7[1]-27.83[1]121[1]
SeO2 (cr)-225.35[1]
SeO2 (aq)-221.63[1]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (aq):Aqueous solution

References

List of references

  1. 1