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4Fe + 4SO3 → FeS + 3FeSO4

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Reaction of iron and sulfur trioxide
4FeIron + 4SO3Sulfur trioxide
⟶
FeSIron(II) sulfide + 3FeSO4Iron(II) sulfate

The reaction of iron and sulfur trioxide yields iron(II) sulfide and iron(II) sulfate (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 iron and sulfur trioxide
4FeIron + 4SO3Sulfur trioxide
⟶
FeSIron(II) sulfide + 3FeSO4Iron(II) sulfate

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 iron and sulfur trioxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeIron4
Reducing
Reducing
SO3Sulfur trioxide4
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
FeSIron(II) sulfide1
Redoxed product
–
FeSO4Iron(II) sulfate3
Oxidized
–

Thermodynamic changes

Changes in standard condition

Reaction of iron and sulfur trioxide
◆
ΔrG−1067.8 kJ/mol
K1.18 × 10187
pK−187.07
4FeCrystalline solid + 4SO3Liquid
⟶
FeSCrystalline solidiron-rich pyrrhotite, α + 3FeSO4Crystalline solid
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
−1121.0−1067.8−181.5–
per 1 mol of
−280.25−266.95−45.38–
per 1 mol of
−280.25−266.95−45.38–
per 1 mol of
−1121.0−1067.8−181.5–
per 1 mol of
−373.67−355.93−60.50–

Changes in aqueous solution

Reaction of iron and sulfur trioxide
◆
ΔrG−1066.0 kJ/mol
K5.69 × 10186
pK−186.76
4FeCrystalline solid + 4SO3Crystalline solidβ
⟶
FeSCrystalline solidiron-rich pyrrhotite, α + 3FeSO4Crystalline solid
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
−1067.2−1066.0−9.1–
per 1 mol of
−266.80−266.50−2.3–
per 1 mol of
−266.80−266.50−2.3–
per 1 mol of
−1067.2−1066.0−9.1–
per 1 mol of
−355.73−355.33−3.0–

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
Fe (cr)0[1]0[1]27.28[1]25.10[1]
Fe (g)416.3[1]370.7[1]180.490[1]25.677[1]
SO3 (cr)
β
-454.51[1]-374.21[1]70.7[1]–
SO3 (l)-441.04[1]-373.75[1]113.8[1]–
SO3 (g)-395.72[1]-371.06[1]256.76[1]50.67[1]
* (cr):Crystalline solid, (g):Gas, (l):Liquid

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
FeS (cr)
iron-rich pyrrhotite, α
-100.0[1]-100.4[1]60.29[1]50.54[1]
FeSO4 (cr)-928.4[1]-820.8[1]107.5[1]100.58[1]
FeSO4 (ai)-998.3[1]-823.43[1]-117.6[1]–
FeSO4 (cr)
1 hydrate
-1243.69[1]–––
FeSO4 (cr)
4 hydrate
-2129.2[1]–––
FeSO4 (cr)
7 hydrate
-3014.57[1]-2509.87[1]409.2[1]394.47[1]
* (cr):Crystalline 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)