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FeSO4 + K2S 💧→ FeS↓ + K2SO4

The reaction of iron(II) sulfate and potassium sulfide yields iron(II) sulfide and potassium sulfate. 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

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeSO4Iron(II) sulfate1
Lewis acid
Soluble in water
K2SPotassium sulfide1
Lewis base
Soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
FeSIron(II) sulfide1
Lewis conjugate
Insoluble in water
K2SO4Potassium sulfate1
Non-redox product

Thermodynamic changes

Changes in standard condition

Reaction of iron(II) sulfate and potassium sulfide
ΔrG−237.0 kJ/mol
K3.32 × 1041
pK−41.52
FeSO4Crystalline solid + K2SCrystalline solid
💧
FeSCrystalline solidiron-rich pyrrhotite, α + K2SO4Crystalline 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
−228.7−237.023
per 1 mol of
−228.7−237.023
per 1 mol of
−228.7−237.023
per 1 mol of
−228.7−237.023
per 1 mol of
−228.7−237.023

Changes in aqueous solution

Reaction of iron(II) sulfate and potassium sulfide
ΔrG−110.0 kJ/mol
K1.87 × 1019
pK−19.27
FeSO4Crystalline solid + K2SIonized aqueous solution
💧
FeSCrystalline solidiron-rich pyrrhotite, α + K2SO4Ionized 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
−114.1−110.0−12.5
per 1 mol of
−114.1−110.0−12.5
per 1 mol of
−114.1−110.0−12.5
per 1 mol of
−114.1−110.0−12.5
per 1 mol of
−114.1−110.0−12.5

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
FeSO4 (cr)-928.4[1]-820.8[1]107.5[1]100.58[1]
FeSO4 (ai)-998.3[1]-823.43[1]-117.6[1]
FeSO4 (cr)
1 hydrate
-1243.69[1]
FeSO4 (cr)
4 hydrate
-2129.2[1]
FeSO4 (cr)
7 hydrate
-3014.57[1]-2509.87[1]409.2[1]394.47[1]
K2S (cr)-380.7[1]-364.0[1]105[1]
K2S (ai)-471.5[1]-480.7[1]190.4[1]
K2S (cr)
2 hydrate
-975.3[1]
K2S (cr)
5 hydrate
-1871.5[1]
* (cr):Crystalline solid, (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]
K2SO4 (cr)-1437.79[1]-1321.37[1]175.56[1]131.46[1]
K2SO4 (g)-1096[1]-1033[1]364[1]108.8[1]
K2SO4 (ai)-1414.02[1]-1311.07[1]225.1[1]-251[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

References

List of references

  1. 1