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FeBr2 + Mg(OH)2 → MgBr2 + Fe(OH)2

The reaction of iron(II) bromide and magnesium hydroxide yields magnesium bromide and iron(II) hydroxide. 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
FeBr2Iron(II) bromide1
Brønsted acid
Salt of weak base
Mg(OH)2Magnesium hydroxide1
Brønsted base
Strong base

Products

Chemical formulaNameCoefficientTypeType in general
equation
MgBr2Magnesium bromide1
Conjugate acid
Salt of strong base
Fe(OH)2Iron(II) hydroxide1
Conjugate base
Weak base

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) bromide and magnesium hydroxide
ΔrG81.3 kJ/mol
K0.57 × 10−14
pK14.24
FeBr2Crystalline solid + Mg(OH)2Crystalline solid
MgBr2Crystalline solid + Fe(OH)2Crystalline solidprecipitated
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
81.081.31
per 1 mol of
81.081.31
81.081.31
per 1 mol of
81.081.31
per 1 mol of
81.081.31

Changes in standard condition (2)

Reaction of iron(II) bromide and magnesium hydroxide
FeBr2Crystalline solid + Mg(OH)2Amorphous solidprecipitated
MgBr2Crystalline solid + Fe(OH)2Crystalline solidprecipitated
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
77.0
per 1 mol of
77.0
77.0
per 1 mol of
77.0
per 1 mol of
77.0

Changes in aqueous solution (1)

Reaction of iron(II) bromide and magnesium hydroxide
ΔrG−28.9 kJ/mol
K1.16 × 105
pK−5.06
FeBr2Ionized aqueous solution + Mg(OH)2Crystalline solid
MgBr2Ionized aqueous solution + Fe(OH)2Crystalline solidprecipitated
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
−22.2−28.924
per 1 mol of
−22.2−28.924
−22.2−28.924
per 1 mol of
−22.2−28.924
per 1 mol of
−22.2−28.924

Changes in aqueous solution (2)

Reaction of iron(II) bromide and magnesium hydroxide
FeBr2Ionized aqueous solution + Mg(OH)2Amorphous solidprecipitated
MgBr2Ionized aqueous solution + Fe(OH)2Crystalline solidprecipitated
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
−26.2
per 1 mol of
−26.2
−26.2
per 1 mol of
−26.2
per 1 mol of
−26.2

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
FeBr2 (cr)-249.8[1]-238.1[1]140.6[1]
FeBr2 (g)-46[1]
FeBr2 (ai)-332.2[1]-286.81[1]27.2[1]
Mg(OH)2 (cr)-924.54[1]-833.51[1]63.18[1]77.03[1]
Mg(OH)2 (am)
precipitated
-920.5[1]
Mg(OH)2 (g)-561[1]
Mg(OH)2 (ai)-926.84[1]-769.4[1]-159.4[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (am):Amorphous solid

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
MgBr2 (cr)-524.3[1]-503.8[1]117.2[1]
MgBr2 (g)-309.6[1]
MgBr2 (ai)-709.94[1]-662.7[1]26.8[1]
MgBr2 (cr)
6 hydrate
-2410.0[1]-2055.7[1]397[1]
Fe(OH)2 (cr)
precipitated
-569.0[1]-486.5[1]88[1]
Fe(OH)2 (g)-372[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

References

List of references

  1. 1