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Na + FeCl3 → NaCl + FeCl2

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Reaction of sodium and iron(III) chloride
NaSodium + FeCl3Iron(III) chloride
⟶
NaClSodium chloride + FeCl2Iron(II) chloride

The reaction of sodium and iron(III) chloride yields sodium chloride and iron(II) chloride (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) chloride
NaSodium + FeCl3Iron(III) chloride
⟶
NaClSodium chloride + FeCl2Iron(II) chloride

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) chloride

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium1
Reducing
Reducing
FeCl3Iron(III) chloride1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaClSodium chloride1
Oxidized
–
FeCl2Iron(II) chloride1
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of sodium and iron(III) chloride
◆
ΔrG−352.44 kJ/mol
K5.56 × 1061
pK−61.74
NaCrystalline solid + FeCl3Crystalline solid
⟶
NaClCrystalline solid + FeCl2Crystalline 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
−353.45−352.44−3.42.26
per 1 mol of
−353.45−352.44−3.42.26
per 1 mol of
−353.45−352.44−3.42.26
per 1 mol of
−353.45−352.44−3.42.26
per 1 mol of
−353.45−352.44−3.42.26

Changes in aqueous solution (1)

Reaction of sodium and iron(III) chloride
◆
ΔrG−267.7 kJ/mol
K7.93 × 1046
pK−46.90
NaCrystalline solid + FeCl3Un-ionized aqueous solution
⟶
NaClIonized aqueous solution + FeCl2Un-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
–−267.7––
per 1 mol of
–−267.7––
per 1 mol of
–−267.7––
per 1 mol of
–−267.7––
per 1 mol of
–−267.7––

Changes in aqueous solution (2)

Reaction of sodium and iron(III) chloride
◆
ΔrG−330.0 kJ/mol
K6.51 × 1057
pK−57.81
NaCrystalline solid + FeCl3Un-ionized aqueous solution
⟶
NaClIonized aqueous solution + FeCl2Ionized 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
–−330.0––
per 1 mol of
–−330.0––
per 1 mol of
–−330.0––
per 1 mol of
–−330.0––
per 1 mol of
–−330.0––

Changes in aqueous solution (3)

Reaction of sodium and iron(III) chloride
◆
ΔrG−273.9 kJ/mol
K9.67 × 1047
pK−47.99
NaCrystalline solid + FeCl3Ionized aqueous solution
⟶
NaClIonized aqueous solution + FeCl2Un-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
–−273.9––
per 1 mol of
–−273.9––
per 1 mol of
–−273.9––
per 1 mol of
–−273.9––
per 1 mol of
–−273.9––

Changes in aqueous solution (4)

Reaction of sodium and iron(III) chloride
◆
ΔrG−336.2 kJ/mol
K7.94 × 1058
pK−58.90
NaCrystalline solid + FeCl3Ionized aqueous solution
⟶
NaClIonized aqueous solution + FeCl2Ionized 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
−280.5−336.2186.0–
per 1 mol of
−280.5−336.2186.0–
per 1 mol of
−280.5−336.2186.0–
per 1 mol of
−280.5−336.2186.0–
per 1 mol of
−280.5−336.2186.0–

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
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]
FeCl3 (cr)-399.49[1]-334.00[1]142.3[1]96.65[1]
FeCl3 (g)-254.0[1]–––
FeCl3 (ai)-550.2[1]-398.3[1]-146.4[1]–
FeCl3 (ao)–-404.5[1]––
FeCl3 (cr)
6 hydrate
-2223.8[1]–––
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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
NaCl (cr)-411.153[1]-384.138[1]72.13[1]50.50[1]
NaCl (g)-176.65[1]-196.66[1]229.81[1]35.77[1]
NaCl (ai)-407.27[1]-393.133[1]115.5[1]-90.0[1]
FeCl2 (cr)-341.79[1]-302.30[1]117.95[1]76.65[1]
FeCl2 (g)-148.5[1]–––
FeCl2 (ai)-423.4[1]-341.34[1]-24.7[1]–
FeCl2 (ao)–-279.1[1]––
FeCl2 (cr)
2 hydrate
-953.1[1]–––
FeCl2 (cr)
4 hydrate
-1549.3[1]–––
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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)