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3FeO + Mg(OH)2 ๐Ÿ”ฅโ†’ Fe3O4 + MgO + H2โ†‘

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Reaction of iron(II) oxide and magnesium hydroxide
3FeOIron(II) oxide + Mg(OH)2Magnesium hydroxide
๐Ÿ”ฅ
โŸถ
Fe3O4Iron(II,III) oxide + MgOMagnesium oxide + H2โ†‘Hydrogen

The reaction of iron(II) oxide and magnesium hydroxide yields iron(II,III) oxide, magnesium oxide, and hydrogen (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 iron(II) oxide and magnesium hydroxide
3FeOIron(II) oxide + Mg(OH)2Magnesium hydroxide
๐Ÿ”ฅ
โŸถ
Fe3O4Iron(II,III) oxide + MgOMagnesium oxide + H2โ†‘Hydrogen

General equation

Reaction of oxidizable species and reducible species
Oxidizable speciesReducing agent + Reducible speciesOxidizing agent
๐Ÿ”ฅ
โŸถ
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of iron(II) oxide and magnesium hydroxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeOIron(II) oxide3
Reducing
Oxidizable
Mg(OH)2Magnesium hydroxide1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe3O4Iron(II,III) oxide1
Oxidized
โ€“
MgOMagnesium oxide1
โ€“
โ€“
H2Hydrogen1
Reduced
โ€“

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) oxide and magnesium hydroxide
3FeOCrystalline solid + Mg(OH)2Crystalline solid
๐Ÿ”ฅ
โŸถ
Fe3O4Crystalline solid + MgOCrystalline solid + H2โ†‘Gas
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
24.2โ€“โ€“โ€“
per 1 mol of
8.07โ€“โ€“โ€“
24.2โ€“โ€“โ€“
per 1 mol of
24.2โ€“โ€“โ€“
per 1 mol of
24.2โ€“โ€“โ€“
per 1 mol of
24.2โ€“โ€“โ€“

Changes in standard condition (2)

Reaction of iron(II) oxide and magnesium hydroxide
3FeOCrystalline solid + Mg(OH)2Amorphous solidprecipitated
๐Ÿ”ฅ
โŸถ
Fe3O4Crystalline solid + MgOCrystalline solid + H2โ†‘Gas
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
20.1โ€“โ€“โ€“
per 1 mol of
6.70โ€“โ€“โ€“
20.1โ€“โ€“โ€“
per 1 mol of
20.1โ€“โ€“โ€“
per 1 mol of
20.1โ€“โ€“โ€“
per 1 mol of
20.1โ€“โ€“โ€“

Changes in aqueous solution (1)

Reaction of iron(II) oxide and magnesium hydroxide
3FeOCrystalline solid + Mg(OH)2Crystalline solid
๐Ÿ”ฅ
โŸถ
Fe3O4Crystalline solid + MgOCrystalline solid + H2โ†‘Gas
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
24.2โ€“โ€“โ€“
per 1 mol of
8.07โ€“โ€“โ€“
24.2โ€“โ€“โ€“
per 1 mol of
24.2โ€“โ€“โ€“
per 1 mol of
24.2โ€“โ€“โ€“
per 1 mol of
24.2โ€“โ€“โ€“

Changes in aqueous solution (2)

Reaction of iron(II) oxide and magnesium hydroxide
3FeOCrystalline solid + Mg(OH)2Crystalline solid
๐Ÿ”ฅ
โŸถ
Fe3O4Crystalline solid + MgOCrystalline solid + H2โ†‘Un-ionized aqueous solution
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
20.0โ€“โ€“โ€“
per 1 mol of
6.67โ€“โ€“โ€“
20.0โ€“โ€“โ€“
per 1 mol of
20.0โ€“โ€“โ€“
per 1 mol of
20.0โ€“โ€“โ€“
per 1 mol of
20.0โ€“โ€“โ€“

Changes in aqueous solution (3)

Reaction of iron(II) oxide and magnesium hydroxide
3FeOCrystalline solid + Mg(OH)2Amorphous solidprecipitated
๐Ÿ”ฅ
โŸถ
Fe3O4Crystalline solid + MgOCrystalline solid + H2โ†‘Gas
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
20.1โ€“โ€“โ€“
per 1 mol of
6.70โ€“โ€“โ€“
20.1โ€“โ€“โ€“
per 1 mol of
20.1โ€“โ€“โ€“
per 1 mol of
20.1โ€“โ€“โ€“
per 1 mol of
20.1โ€“โ€“โ€“

Changes in aqueous solution (4)

Reaction of iron(II) oxide and magnesium hydroxide
3FeOCrystalline solid + Mg(OH)2Amorphous solidprecipitated
๐Ÿ”ฅ
โŸถ
Fe3O4Crystalline solid + MgOCrystalline solid + H2โ†‘Un-ionized aqueous solution
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
15.9โ€“โ€“โ€“
per 1 mol of
5.30โ€“โ€“โ€“
15.9โ€“โ€“โ€“
per 1 mol of
15.9โ€“โ€“โ€“
per 1 mol of
15.9โ€“โ€“โ€“
per 1 mol of
15.9โ€“โ€“โ€“

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ฮ”fHยฐ
kJ ยท molโˆ’1		Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1		Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
FeO (cr)-272.0[1]โ€“โ€“โ€“
Mg(OH)2 (cr)-924.54[1]-833.51[1]63.18[1]77.03[1]
Mg(OH)2 (am)
precipitated
-920.5[1]โ€“โ€“โ€“
Mg(OH)2 (g)-561[1]โ€“โ€“โ€“
Mg(OH)2 (ai)-926.84[1]-769.4[1]-159.4[1]โ€“
* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (ai):Ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ฮ”fHยฐ
kJ ยท molโˆ’1		Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1		Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
Fe3O4 (cr)-1118.4[1]-1015.4[1]146.4[1]143.43[1]
MgO (cr)-597.98[1]-565.95[1]27.91[1]37.66[1]
MgO (g)17[1]โ€“โ€“โ€“
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]โ€“
* (cr):Crystalline solid, (g):Gas, (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)