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FeI2 + Na2S 💧→ FeS↓ + 2NaI

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Reaction of iron(II) iodide and sodium sulfide
FeI2Iron(II) iodide + Na2SSodium sulfide
💧
⟶
FeS↓Iron(II) sulfide + 2NaISodium iodide

The reaction of iron(II) iodide and sodium sulfide yields iron(II) sulfide and sodium iodide. This reaction is an acid-base reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

Reaction of iron(II) iodide and sodium sulfide
FeI2Iron(II) iodide + Na2SSodium sulfide
💧
⟶
FeS↓Iron(II) sulfide + 2NaISodium iodide

General equation

Precipitation reaction
Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base
💧
⟶
Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)

Oxidation state of each atom

Reaction of iron(II) iodide and sodium sulfide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeI2Iron(II) iodide1
Lewis acid
Soluble in water
Na2SSodium sulfide1
Lewis base
Soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
FeSIron(II) sulfide1
Lewis conjugate
Insoluble in water
NaISodium iodide2
Non-redox product
–

Thermodynamic changes

Changes in standard condition

Reaction of iron(II) iodide and sodium sulfide
FeI2Crystalline solid + Na2SCrystalline solid
💧
⟶
FeS↓Crystalline solidiron-rich pyrrhotite, α + 2NaICrystalline 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
−197.8–––
per 1 mol of
−197.8–––
per 1 mol of
−197.8–––
per 1 mol of
−197.8–––
per 1 mol of
−98.90–––

Changes in aqueous solution

Reaction of iron(II) iodide and sodium sulfide
◆
ΔrG−107.2 kJ/mol
K6.03 × 1018
pK−18.78
FeI2Ionized aqueous solution + Na2SIonized aqueous solution
💧
⟶
FeS↓Crystalline solidiron-rich pyrrhotite, α + 2NaIIonized 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
−43.7−107.2212.7–
per 1 mol of
−43.7−107.2212.7–
per 1 mol of
−43.7−107.2212.7–
per 1 mol of
−43.7−107.2212.7–
per 1 mol of
−21.9−53.60106.3–

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
FeI2 (cr)-113.0[1]–––
FeI2 (g)60.7[1]–––
FeI2 (ai)-199.6[1]-182.05[1]84.9[1]–
Na2S (cr)-364.8[1]-349.8[1]83.7[1]–
Na2S (ai)-447.3[1]-438.1[1]103.3[1]–
Na2S (cr)
4.5 hydrate
-1725.9[1]–––
Na2S (cr)
5 hydrate
-1886.6[1]–––
Na2S (cr)
9 hydrate
-3074.0[1]–––
* (cr):Crystalline solid, (g):Gas, (ai):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
FeS (cr)
iron-rich pyrrhotite, α
-100.0[1]-100.4[1]60.29[1]50.54[1]
NaI (cr)-287.78[1]-286.06[1]98.53[1]52.09[1]
NaI (g)-79.5[1]-121.0[1]248.978[1]36.65[1]
NaI (ai)-295.31[1]-313.47[1]170.3[1]-95.8[1]
NaI (cr)
1 hydrate
-883.096[1]-771.10[1]196.2[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)