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H2S + 2SeO2 → H2SO4 + 2Se

The reaction of hydrogen sulfide and selenium dioxide yields sulfuric acid and selenium (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 sulfide1
Reducing
Reducing
SeO2Selenium dioxide2
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
H2SO4Sulfuric acid1
Oxidized
SeSelenium2
Reduced

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and selenium dioxide
H2SGas + 2SeO2Crystalline solid
H2SO4Liquid + 2SeCrystalline solidhexagonal, gray
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
−342.66
per 1 mol of
−342.66
per 1 mol of
−171.33
per 1 mol of
−342.66
per 1 mol of
−171.33

Changes in standard condition (2)

Reaction of hydrogen sulfide and selenium dioxide
H2SGas + 2SeO2Crystalline solid
H2SO4Liquid + 2SeCrystalline solidmonoclinic, red
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
−329.3
per 1 mol of
−329.3
per 1 mol of
−164.7
per 1 mol of
−329.3
per 1 mol of
−164.7

Changes in aqueous solution

Reaction of hydrogen sulfide and selenium dioxide
H2SUn-ionized aqueous solution + 2SeO2Aqueous solution
H2SO4Ionized aqueous solution + 2SeCrystalline solidhexagonal, gray
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
−426.3
per 1 mol of
−426.3
per 1 mol of
−213.2
per 1 mol of
−426.3
per 1 mol of
−213.2

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]
SeO2 (cr)-225.35[1]
SeO2 (aq)-221.63[1]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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
H2SO4 (cr)
H2SO4 (l)-813.989[1]-690.003[1]156.904[1]138.91[1]
H2SO4 (ai)-909.27[1]-744.53[1]20.1[1]-293[1]
H2SO4 (l)
1 hydrate
-1127.621[1]-950.383[1]211.54[1]214.85[1]
H2SO4 (l)
2 hydrate
-1427.100[1]-1199.650[1]276.40[1]260.83[1]
H2SO4 (l)
3 hydrate
-1720.402[1]-1443.980[1]345.39[1]318.95[1]
H2SO4 (l)
4 hydrate
-2011.199[1]-1685.863[1]414.59[1]382.21[1]
H2SO4 (l)
6.5 hydrate
-2733.256[1]-2285.734[1]587.89[1]570.28[1]
Se (cr)
hexagonal, gray
0[1]0[1]42.442[1]25.363[1]
Se (cr)
monoclinic, red
6.7[1]
Se (vit)5.0[1]
Se (g)227.07[1]187.03[1]176.72[1]20.820[1]
* (cr):Crystalline solid, (l):Liquid, (ai):Ionized aqueous solution, (vit):Vitreous liquid, (g):Gas

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)