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CaH2 + 3Fe2O3 → CaO + 2Fe3O4 + H2↑

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Reaction of calcium hydride and iron(III) oxide
CaH2Calcium hydride + 3Fe2O3Iron(III) oxide
⟶
CaOCalcium oxide + 2Fe3O4Iron(II,III) oxide + H2↑Hydrogen

The reaction of calcium hydride and iron(III) oxide yields calcium oxide, iron(II,III) oxide, and hydrogen (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 calcium hydride and iron(III) oxide
CaH2Calcium hydride + 3Fe2O3Iron(III) oxide
⟶
CaOCalcium oxide + 2Fe3O4Iron(II,III) oxide + H2↑Hydrogen

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 calcium hydride and iron(III) oxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CaH2Calcium hydride1
Reducing
Reducing
Fe2O3Iron(III) oxide3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
CaOCalcium oxide1
–
–
Fe3O4Iron(II,III) oxide2
Reduced
–
H2Hydrogen1
Oxidized
–

Thermodynamic changes

Changes in standard condition

Reaction of calcium hydride and iron(III) oxide
◆
ΔrG−261.0 kJ/mol
K5.31 × 1045
pK−45.73
CaH2Crystalline solid + 3Fe2O3Crystalline solid
⟶
CaOCrystalline solid + 2Fe3O4Crystalline solid + H2↑Gas
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
−213.1−261.0159–
per 1 mol of
−213.1−261.0159–
per 1 mol of
−71.03−87.0053.0–
per 1 mol of
−213.1−261.0159–
per 1 mol of
−106.5−130.579.5–
per 1 mol of
−213.1−261.0159–

Changes in aqueous solution (1)

Reaction of calcium hydride and iron(III) oxide
◆
ΔrG−261.0 kJ/mol
K5.31 × 1045
pK−45.73
CaH2Crystalline solid + 3Fe2O3Crystalline solid
⟶
CaOCrystalline solid + 2Fe3O4Crystalline solid + H2↑Gas
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
−213.1−261.0159–
per 1 mol of
−213.1−261.0159–
per 1 mol of
−71.03−87.0053.0–
per 1 mol of
−213.1−261.0159–
per 1 mol of
−106.5−130.579.5–
per 1 mol of
−213.1−261.0159–

Changes in aqueous solution (2)

Reaction of calcium hydride and iron(III) oxide
◆
ΔrG−243.4 kJ/mol
K4.38 × 1042
pK−42.64
CaH2Crystalline solid + 3Fe2O3Crystalline solid
⟶
CaOCrystalline solid + 2Fe3O4Crystalline solid + H2↑Un-ionized aqueous solution
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
−217.3−243.4605–
per 1 mol of
−217.3−243.4605–
per 1 mol of
−72.43−81.13202–
per 1 mol of
−217.3−243.4605–
per 1 mol of
−108.7−121.7303–
per 1 mol of
−217.3−243.4605–

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
CaH2 (cr)-186.2[1]-147.2[1]42[1]–
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[1]
* (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
CaO (cr)-635.09[1]-604.03[1]39.75[1]42.80[1]
CaO (g)––––
Fe3O4 (cr)-1118.4[1]-1015.4[1]146.4[1]143.43[1]
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
* (cr):Crystalline solid, (g):Gas, (ao):Un-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)