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3Zn + Fe2O3 → 3ZnO + 2Fe

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Reaction of zinc and iron(III) oxide
3ZnZinc + Fe2O3Iron(III) oxide
⟶
3ZnOZinc oxide + 2FeIron

The reaction of zinc and iron(III) oxide yields zinc oxide and iron (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 zinc and iron(III) oxide
3ZnZinc + Fe2O3Iron(III) oxide
⟶
3ZnOZinc oxide + 2FeIron

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 zinc and iron(III) oxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
ZnZinc3
Reducing
Reducing
Fe2O3Iron(III) oxide1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
ZnOZinc oxide3
Oxidized
–
FeIron2
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of zinc and iron(III) oxide
◆
ΔrG−212.7 kJ/mol
K1.83 × 1037
pK−37.26
3ZnCrystalline solid + Fe2O3Crystalline solid
⟶
3ZnOCrystalline solid + 2FeCrystalline 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
−220.6−212.7−26.81−9.10
per 1 mol of
−73.53−70.90−8.937−3.03
per 1 mol of
−220.6−212.7−26.81−9.10
per 1 mol of
−73.53−70.90−8.937−3.03
per 1 mol of
−110.3−106.3−13.40−4.55

Changes in aqueous solution

Reaction of zinc and iron(III) oxide
◆
ΔrG−212.7 kJ/mol
K1.83 × 1037
pK−37.26
3ZnCrystalline solid + Fe2O3Crystalline solid
⟶
3ZnOCrystalline solid + 2FeCrystalline 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
−220.6−212.7−26.81−9.10
per 1 mol of
−73.53−70.90−8.937−3.03
per 1 mol of
−220.6−212.7−26.81−9.10
per 1 mol of
−73.53−70.90−8.937−3.03
per 1 mol of
−110.3−106.3−13.40−4.55

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
Zn (cr)0[1]0[1]41.63[1]25.40[1]
Zn (g)130.729[1]95.145[1]160.984[1]20.786[1]
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[1]
* (cr):Crystalline solid, (g):Gas

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
ZnO (cr)-348.28[1]-318.30[1]43.64[1]40.25[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]
* (cr):Crystalline solid, (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)