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2PH3 + 6Fe2O3 → 2P + 3Fe(OH)2 + 3Fe3O4

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Reaction of phosphine and iron(III) oxide
2PH3Phosphine + 6Fe2O3Iron(III) oxide
⟶
2PPhosphorus + 3Fe(OH)2Iron(II) hydroxide + 3Fe3O4Iron(II,III) oxide

The reaction of phosphine and iron(III) oxide yields phosphorus, iron(II) hydroxide, and iron(II,III) oxide (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 phosphine and iron(III) oxide
2PH3Phosphine + 6Fe2O3Iron(III) oxide
⟶
2PPhosphorus + 3Fe(OH)2Iron(II) hydroxide + 3Fe3O4Iron(II,III) oxide

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 phosphine and iron(III) oxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
PH3Phosphine2
Reducing
Reducing
Fe2O3Iron(III) oxide6
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
PPhosphorus2
Oxidized
–
Fe(OH)2Iron(II) hydroxide3
Reduced
–
Fe3O4Iron(II,III) oxide3
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of phosphine and iron(III) oxide
◆
ΔrG−79.3 kJ/mol
K7.81 × 1013
pK−13.89
2PH3Gas + 6Fe2O3Crystalline solid
⟶
2PCrystalline solidwhite + 3Fe(OH)2Crystalline solidprecipitated + 3Fe3O4Crystalline 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
−127.8−79.3−159–
per 1 mol of
−63.90−39.6−79.5–
per 1 mol of
−21.30−13.2−26.5–
per 1 mol of
−63.90−39.6−79.5–
per 1 mol of
−42.60−26.4−53.0–
per 1 mol of
−42.60−26.4−53.0–

Changes in standard condition (2)

Reaction of phosphine and iron(III) oxide
◆
ΔrG−103.5 kJ/mol
K1.36 × 1018
pK−18.13
2PH3Gas + 6Fe2O3Crystalline solid
⟶
2PCrystalline solidred, triclinic + 3Fe(OH)2Crystalline solidprecipitated + 3Fe3O4Crystalline 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
−163.0−103.5−196–
per 1 mol of
−81.50−51.75−98.0–
per 1 mol of
−27.17−17.25−32.7–
per 1 mol of
−81.50−51.75−98.0–
per 1 mol of
−54.33−34.50−65.3–
per 1 mol of
−54.33−34.50−65.3–

Changes in standard condition (3)

Reaction of phosphine and iron(III) oxide
2PH3Gas + 6Fe2O3Crystalline solid
⟶
2PCrystalline solidblack + 3Fe(OH)2Crystalline solidprecipitated + 3Fe3O4Crystalline 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
−206.4–––
per 1 mol of
−103.2–––
per 1 mol of
−34.40–––
per 1 mol of
−103.2–––
per 1 mol of
−68.80–––
per 1 mol of
−68.80–––

Changes in standard condition (4)

Reaction of phosphine and iron(III) oxide
2PH3Gas + 6Fe2O3Crystalline solid
⟶
2PAmorphous solidred + 3Fe(OH)2Crystalline solidprecipitated + 3Fe3O4Crystalline 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
−142.8–––
per 1 mol of
−71.40–––
per 1 mol of
−23.80–––
per 1 mol of
−71.40–––
per 1 mol of
−47.60–––
per 1 mol of
−47.60–––

Changes in aqueous solution

Reaction of phosphine and iron(III) oxide
◆
ΔrG−103.2 kJ/mol
K1.20 × 1018
pK−18.08
2PH3Un-ionized aqueous solution + 6Fe2O3Crystalline solid
⟶
2PCrystalline solidwhite + 3Fe(OH)2Crystalline solidprecipitated + 3Fe3O4Crystalline 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
−98.0−103.221–
per 1 mol of
−49.0−51.6011–
per 1 mol of
−16.3−17.203.5–
per 1 mol of
−49.0−51.6011–
per 1 mol of
−32.7−34.407.0–
per 1 mol of
−32.7−34.407.0–

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
PH3 (g)5.4[1]13.4[1]210.23[1]37.11[1]
PH3 (ao)-9.50[1]25.36[1]120.1[1]–
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[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
P (cr)
white
0[1]0[1]41.09[1]23.84[1]
P (cr)
red, triclinic
-17.6[1]-12.1[1]22.80[1]21.21[1]
P (cr)
black
-39.3[1]–––
P (am)
red
-7.5[1]–––
P (g)314.64[1]278.25[1]163.193[1]20.786[1]
Fe(OH)2 (cr)
precipitated
-569.0[1]-486.5[1]88[1]–
Fe(OH)2 (g)-372[1]–––
Fe3O4 (cr)-1118.4[1]-1015.4[1]146.4[1]143.43[1]
* (cr):Crystalline solid, (am):Amorphous 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)