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FeSe + 2H2O → Fe(OH)2 + H2Se↑

The reaction of iron(II) selenide and water yields iron(II) hydroxide and hydrogen selenide. 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

Hydrolysis of salt
Salt of weak acid and weak baseBrønsted base + H2OBrønsted acid
Base/Basic saltConjugate base + Acid/Acid salt/HydrideConjugate acid

Oxidation state of each atom

Hydrolysis of iron(II) selenide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeSeIron(II) selenide1
Brønsted base
Salt of weak acid and weak base
H2OWater2
Brønsted acid
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe(OH)2Iron(II) hydroxide1
Conjugate base
Base
H2SeHydrogen selenide1
Conjugate acid
Acid

Thermodynamic changes

Changes in standard condition (1)

Hydrolysis of iron(II) selenide
FeSeCrystalline solid + 2H2OLiquid
Fe(OH)2Crystalline solidprecipitated + H2SeGas
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
107.7
per 1 mol of
107.7
per 1 mol of
53.85
per 1 mol of
107.7
per 1 mol of
107.7

Changes in standard condition (2)

Hydrolysis of iron(II) selenide
FeSeAmorphous solid + 2H2OLiquid
Fe(OH)2Crystalline solidprecipitated + H2SeGas
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
96.0
per 1 mol of
96.0
per 1 mol of
48.0
per 1 mol of
96.0
per 1 mol of
96.0

Changes in aqueous solution (1)

Hydrolysis of iron(II) selenide
FeSeCrystalline solid + 2H2OLiquid
Fe(OH)2Crystalline solidprecipitated + H2SeGas
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
107.7
per 1 mol of
107.7
per 1 mol of
53.85
per 1 mol of
107.7
per 1 mol of
107.7

Changes in aqueous solution (2)

Hydrolysis of iron(II) selenide
FeSeCrystalline solid + 2H2OLiquid
Fe(OH)2Crystalline solidprecipitated + H2SeUn-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
97.2
per 1 mol of
97.2
per 1 mol of
48.6
per 1 mol of
97.2
per 1 mol of
97.2

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
FeSe (cr)-75.3[1]
FeSe (am)-63.6[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, (am):Amorphous solid, (l):Liquid, (g):Gas

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
Fe(OH)2 (cr)
precipitated
-569.0[1]-486.5[1]88[1]
Fe(OH)2 (g)-372[1]
H2Se (g)29.7[1]15.9[1]219.02[1]34.73[1]
H2Se (ao)19.2[1]22.2[1]163.6[1]
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

  1. 1