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6Na + 2Fe(OH)3 → 3Na2O + 2Fe + 3H2O

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Reaction of sodium and iron(III) hydroxide
6NaSodium + 2Fe(OH)3Iron(III) hydroxide
⟶
3Na2OSodium oxide + 2FeIron + 3H2OWater

The reaction of sodium and iron(III) hydroxide yields sodium oxide, iron, 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 sodium and iron(III) hydroxide
6NaSodium + 2Fe(OH)3Iron(III) hydroxide
⟶
3Na2OSodium oxide + 2FeIron + 3H2OWater

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 sodium and iron(III) hydroxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium6
Reducing
Reducing
Fe(OH)3Iron(III) hydroxide2
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2OSodium oxide3
Oxidized
–
FeIron2
Reduced
–
H2OWater3
–
–

Thermodynamic changes

Changes in standard condition

Reaction of sodium and iron(III) hydroxide
◆
ΔrG−444.8 kJ/mol
K8.43 × 1077
pK−77.93
6NaCrystalline solid + 2Fe(OH)3Crystalline solidprecipitated
⟶
3Na2OCrystalline solid + 2FeCrystalline solid + 3H2OLiquid
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
−454.2−444.8−31.2–
per 1 mol of
−75.70−74.13−5.20–
−227.1−222.4−15.6–
per 1 mol of
−151.4−148.3−10.4–
per 1 mol of
−227.1−222.4−15.6–
per 1 mol of
−151.4−148.3−10.4–

Changes in aqueous solution

Reaction of sodium and iron(III) hydroxide
◆
ΔrG−519.2 kJ/mol
K9.12 × 1090
pK−90.96
6NaCrystalline solid + 2Fe(OH)3Un-ionized aqueous solution
⟶
3Na2OCrystalline solid + 2FeCrystalline solid + 3H2OLiquid
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
–−519.2––
per 1 mol of
–−86.53––
–−259.6––
per 1 mol of
–−173.1––
per 1 mol of
–−259.6––
per 1 mol of
–−173.1––

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
Na (cr)0[1]0[1]51.21[1]28.24[1]
Na (g)107.32[1]76.761[1]153.712[1]20.786[1]
Fe(OH)3 (cr)
precipitated
-823.0[1]-696.5[1]106.7[1]–
Fe(OH)3 (ao)–-659.3[1]––
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution

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
Na2O (cr)-414.22[1]-375.46[1]75.06[1]69.12[1]
Na2O (g)-35.6[1]-52.3[1]261.2[1]55.2[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]
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)