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3Na + FeF3 → 3NaF + Fe

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Reaction of sodium and iron(III) fluoride
3NaSodium + FeF3Iron(III) fluoride
⟶
3NaFSodium fluoride + FeIron

The reaction of sodium and iron(III) fluoride yields sodium fluoride 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 sodium and iron(III) fluoride
3NaSodium + FeF3Iron(III) fluoride
⟶
3NaFSodium fluoride + FeIron

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) fluoride

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium3
Reducing
Reducing
FeF3Iron(III) fluoride1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaFSodium fluoride3
Oxidized
–
FeIron1
Reduced
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of sodium and iron(III) fluoride
3NaCrystalline solid + FeF3Aqueous solution
⟶
3NaFIonized aqueous solution + FeCrystalline 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
−702.0–––
per 1 mol of
−234.0–––
per 1 mol of
−702.0–––
per 1 mol of
−234.0–––
per 1 mol of
−702.0–––

Changes in aqueous solution (2)

Reaction of sodium and iron(III) fluoride
◆
ΔrG−781.1 kJ/mol
K6.96 × 10136
pK−136.84
3NaCrystalline solid + FeF3Ionized aqueous solution
⟶
3NaFIonized aqueous solution + FeCrystalline 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
−671.9−781.1366.6–
per 1 mol of
−224.0−260.4122.2–
per 1 mol of
−671.9−781.1366.6–
per 1 mol of
−224.0−260.4122.2–
per 1 mol of
−671.9−781.1366.6–

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]
FeF3 (ai)-1046.4[1]-840.9[1]-357.3[1]–
FeF3 (aq)-1016.3[1]–––
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (aq):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
NaF (cr)-573.647[1]-543.494[1]51.46[1]46.86[1]
NaF (g)-291.2[1]-310.5[1]217.59[1]34.221[1]
NaF (ai)-572.75[1]-540.68[1]45.2[1]-60.2[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]
* (cr):Crystalline solid, (g):Gas, (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)