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4H2S + Fe3O4 → S + 3FeS + 4H2O

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Reaction of hydrogen sulfide and iron(II,III) oxide
4H2SHydrogen sulfide + Fe3O4Iron(II,III) oxide
⟶
SSulfur + 3FeSIron(II) sulfide + 4H2OWater

The reaction of hydrogen sulfide and iron(II,III) oxide yields sulfur, iron(II) 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

Reaction of hydrogen sulfide and iron(II,III) oxide
4H2SHydrogen sulfide + Fe3O4Iron(II,III) oxide
⟶
SSulfur + 3FeSIron(II) sulfide + 4H2OWater

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 iron(II,III) oxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide4
Reducing
Reducing
Fe3O4Iron(II,III) oxide1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
SSulfur1
Oxidized
–
FeSIron(II) sulfide3
Reduced
–
H2OWater4
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and iron(II,III) oxide
◆
ΔrG−100.1 kJ/mol
K3.44 × 1017
pK−17.54
4H2SGas + Fe3O4Crystalline solid
⟶
SCrystalline solidrhombic + 3FeSCrystalline solidiron-rich pyrrhotite, α + 4H2OLiquid
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
−242.4−100.1−477.3195.07
per 1 mol of
−60.60−25.02−119.348.767
per 1 mol of
−242.4−100.1−477.3195.07
per 1 mol of
−242.4−100.1−477.3195.07
per 1 mol of
−80.80−33.37−159.165.023
per 1 mol of
−60.60−25.02−119.348.767

Changes in standard condition (2)

Reaction of hydrogen sulfide and iron(II,III) oxide
4H2SGas + Fe3O4Crystalline solid
⟶
SCrystalline solidmonoclinic + 3FeSCrystalline solidiron-rich pyrrhotite, α + 4H2OLiquid
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
−242.1–––
per 1 mol of
−60.52–––
per 1 mol of
−242.1–––
per 1 mol of
−242.1–––
per 1 mol of
−80.70–––
per 1 mol of
−60.52–––

Changes in aqueous solution

Reaction of hydrogen sulfide and iron(II,III) oxide
◆
ΔrG−123.0 kJ/mol
K3.54 × 1021
pK−21.55
4H2SUn-ionized aqueous solution + Fe3O4Crystalline solid
⟶
SCrystalline solidrhombic + 3FeSCrystalline solidiron-rich pyrrhotite, α + 4H2OLiquid
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
−166.1−123.0−138–
per 1 mol of
−41.52−30.75−34.5–
per 1 mol of
−166.1−123.0−138–
per 1 mol of
−166.1−123.0−138–
per 1 mol of
−55.37−41.00−46.0–
per 1 mol of
−41.52−30.75−34.5–

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]–
Fe3O4 (cr)-1118.4[1]-1015.4[1]146.4[1]143.43[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]
FeS (cr)
iron-rich pyrrhotite, α
-100.0[1]-100.4[1]60.29[1]50.54[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, (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)