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6NH4F + 6Fe2O3 ๐Ÿ”ฅโ†’ 2N2โ†‘ + 3FeF2 + 9Fe(OH)2 + 2NH3โ†‘

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Reaction of ammonium fluoride and iron(III) oxide
6NH4FAmmonium fluoride + 6Fe2O3Iron(III) oxide
๐Ÿ”ฅ
โŸถ
2N2โ†‘Nitrogen + 3FeF2Iron(II) fluoride + 9Fe(OH)2Iron(II) hydroxide + 2NH3โ†‘Ammonia

The reaction of ammonium fluoride and iron(III) oxide yields nitrogen, iron(II) fluoride, iron(II) hydroxide, and ammonia (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 ammonium fluoride and iron(III) oxide
6NH4FAmmonium fluoride + 6Fe2O3Iron(III) oxide
๐Ÿ”ฅ
โŸถ
2N2โ†‘Nitrogen + 3FeF2Iron(II) fluoride + 9Fe(OH)2Iron(II) hydroxide + 2NH3โ†‘Ammonia

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
โŸถ
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of ammonium fluoride and iron(III) oxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4FAmmonium fluoride6
Reducing
Reducing
Fe2O3Iron(III) oxide6
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
N2Nitrogen2
Oxidized
โ€“
FeF2Iron(II) fluoride3
Reduced
โ€“
Fe(OH)2Iron(II) hydroxide9
Reduced
โ€“
NH3Ammonia2
โ€“
โ€“

Thermodynamic changes

Changes in standard condition

Reaction of ammonium fluoride and iron(III) oxide
โ—†
ฮ”rG128.1 kJ/mol
K0.36 ร— 10โˆ’22
pK22.44
6NH4FCrystalline solid + 6Fe2O3Crystalline solid
๐Ÿ”ฅ
โŸถ
2N2โ†‘Gas + 3FeF2Crystalline solid + 9Fe(OH)2Crystalline solidprecipitated + 2NH3โ†‘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
381.8128.1865โ€“
per 1 mol of
63.6321.35144โ€“
per 1 mol of
63.6321.35144โ€“
per 1 mol of
190.964.05433โ€“
per 1 mol of
127.342.70288โ€“
per 1 mol of
42.4214.2396.1โ€“
per 1 mol of
190.964.05433โ€“

Changes in aqueous solution (1)

Reaction of ammonium fluoride and iron(III) oxide
6NH4FIonized aqueous solution + 6Fe2O3Crystalline solid
๐Ÿ”ฅ
โŸถ
2N2โ†‘Gas + 3FeF2Aqueous solution + 9Fe(OH)2Crystalline solidprecipitated + 2NH3โ†‘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
287.2โ€“โ€“โ€“
per 1 mol of
47.87โ€“โ€“โ€“
per 1 mol of
47.87โ€“โ€“โ€“
per 1 mol of
143.6โ€“โ€“โ€“
per 1 mol of
95.73โ€“โ€“โ€“
per 1 mol of
31.91โ€“โ€“โ€“
per 1 mol of
143.6โ€“โ€“โ€“

Changes in aqueous solution (2)

Reaction of ammonium fluoride and iron(III) oxide
6NH4FIonized aqueous solution + 6Fe2O3Crystalline solid
๐Ÿ”ฅ
โŸถ
2N2โ†‘Gas + 3FeF2Aqueous solution + 9Fe(OH)2Crystalline solidprecipitated + 2NH3โ†‘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
218.9โ€“โ€“โ€“
per 1 mol of
36.48โ€“โ€“โ€“
per 1 mol of
36.48โ€“โ€“โ€“
per 1 mol of
109.5โ€“โ€“โ€“
per 1 mol of
72.97โ€“โ€“โ€“
per 1 mol of
24.32โ€“โ€“โ€“
per 1 mol of
109.5โ€“โ€“โ€“

Changes in aqueous solution (3)

Reaction of ammonium fluoride and iron(III) oxide
โ—†
ฮ”rG184.5 kJ/mol
K0.48 ร— 10โˆ’32
pK32.32
6NH4FIonized aqueous solution + 6Fe2O3Crystalline solid
๐Ÿ”ฅ
โŸถ
2N2โ†‘Gas + 3FeF2Crystalline solid + 9Fe(OH)2Crystalline solidprecipitated + 2NH3โ†‘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
388.9184.5699โ€“
per 1 mol of
64.8230.75117โ€“
per 1 mol of
64.8230.75117โ€“
per 1 mol of
194.492.25350โ€“
per 1 mol of
129.661.50233โ€“
per 1 mol of
43.2120.5077.7โ€“
per 1 mol of
194.492.25350โ€“

Changes in aqueous solution (4)

Reaction of ammonium fluoride and iron(III) oxide
โ—†
ฮ”rG164.4 kJ/mol
K0.16 ร— 10โˆ’28
pK28.80
6NH4FIonized aqueous solution + 6Fe2O3Crystalline solid
๐Ÿ”ฅ
โŸถ
2N2โ†‘Gas + 3FeF2Crystalline solid + 9Fe(OH)2Crystalline solidprecipitated + 2NH3โ†‘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
320.6164.4537โ€“
per 1 mol of
53.4327.4089.5โ€“
per 1 mol of
53.4327.4089.5โ€“
per 1 mol of
160.382.20269โ€“
per 1 mol of
106.954.80179โ€“
per 1 mol of
35.6218.2759.7โ€“
per 1 mol of
160.382.20269โ€“

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
NH4F (cr)-463.96[1]-348.68[1]71.96[1]65.27[1]
NH4F (ai)-465.14[1]-358.09[1]99.6[1]-26.8[1]
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[1]
* (cr):Crystalline solid, (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
N2 (g)0[1]0[1]191.61[1]29.125[1]
FeF2 (cr)-711.3[1]-668.6[1]86.99[1]68.12[1]
FeF2 (ai)-754.4[1]-636.48[1]-165.3[1]โ€“
FeF2 (aq)-745.2[1]โ€“โ€“โ€“
Fe(OH)2 (cr)
precipitated
-569.0[1]-486.5[1]88[1]โ€“
Fe(OH)2 (g)-372[1]โ€“โ€“โ€“
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[1]โ€“
* (g):Gas, (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (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)