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6FeF2 + 9HNO3 ๐Ÿ”ฅโ†’ 4FeF3 + 2Fe(NO3)3 + 3HNO2 + 3H2O

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Reaction of iron(II) fluoride and nitric acid
6FeF2Iron(II) fluoride + 9HNO3Nitric acid
๐Ÿ”ฅ
โŸถ
4FeF3Iron(III) fluoride + 2Fe(NO3)3Iron(III) nitrate + 3HNO2Nitrous acid + 3H2OWater

The reaction of iron(II) fluoride and nitric acid yields iron(III) fluoride, iron(III) nitrate, nitrous acid, and water (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) fluoride and nitric acid
6FeF2Iron(II) fluoride + 9HNO3Nitric acid
๐Ÿ”ฅ
โŸถ
4FeF3Iron(III) fluoride + 2Fe(NO3)3Iron(III) nitrate + 3HNO2Nitrous acid + 3H2OWater

General equation

Reaction of oxidizable species and oxidizing species
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
โŸถ
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of iron(II) fluoride and nitric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeF2Iron(II) fluoride6
Reducing
Oxidizable
HNO3Nitric acid9
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
FeF3Iron(III) fluoride4
Oxidized
โ€“
Fe(NO3)3Iron(III) nitrate2
Oxidized
โ€“
HNO2Nitrous acid3
Reduced
โ€“
H2OWater3
โ€“
โ€“

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of iron(II) fluoride and nitric acid
6FeF2Aqueous solution + 9HNO3Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
4FeF3Aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
โˆ’284.3โ€“โ€“โ€“
per 1 mol of
โˆ’47.38โ€“โ€“โ€“
per 1 mol of
โˆ’31.59โ€“โ€“โ€“
per 1 mol of
โˆ’71.08โ€“โ€“โ€“
per 1 mol of
โˆ’142.2โ€“โ€“โ€“
per 1 mol of
โˆ’94.77โ€“โ€“โ€“
per 1 mol of
โˆ’94.77โ€“โ€“โ€“

Changes in aqueous solution (2)

Reaction of iron(II) fluoride and nitric acid
6FeF2Aqueous solution + 9HNO3Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
4FeF3Aqueous solution + 2Fe(NO3)3Aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
โˆ’292.7โ€“โ€“โ€“
per 1 mol of
โˆ’48.78โ€“โ€“โ€“
per 1 mol of
โˆ’32.52โ€“โ€“โ€“
per 1 mol of
โˆ’73.17โ€“โ€“โ€“
per 1 mol of
โˆ’146.3โ€“โ€“โ€“
per 1 mol of
โˆ’97.57โ€“โ€“โ€“
per 1 mol of
โˆ’97.57โ€“โ€“โ€“

Changes in aqueous solution (3)

Reaction of iron(II) fluoride and nitric acid
6FeF2Aqueous solution + 9HNO3Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
4FeF3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
โˆ’404.7โ€“โ€“โ€“
per 1 mol of
โˆ’67.45โ€“โ€“โ€“
per 1 mol of
โˆ’44.97โ€“โ€“โ€“
per 1 mol of
โˆ’101.2โ€“โ€“โ€“
per 1 mol of
โˆ’202.3โ€“โ€“โ€“
per 1 mol of
โˆ’134.9โ€“โ€“โ€“
per 1 mol of
โˆ’134.9โ€“โ€“โ€“

Changes in aqueous solution (4)

Reaction of iron(II) fluoride and nitric acid
6FeF2Aqueous solution + 9HNO3Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
4FeF3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
โˆ’413.1โ€“โ€“โ€“
per 1 mol of
โˆ’68.85โ€“โ€“โ€“
per 1 mol of
โˆ’45.90โ€“โ€“โ€“
per 1 mol of
โˆ’103.3โ€“โ€“โ€“
per 1 mol of
โˆ’206.6โ€“โ€“โ€“
per 1 mol of
โˆ’137.7โ€“โ€“โ€“
per 1 mol of
โˆ’137.7โ€“โ€“โ€“

Changes in aqueous solution (5)

Reaction of iron(II) fluoride and nitric acid
6FeF2Crystalline solid + 9HNO3Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
4FeF3Aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
โˆ’487.7โ€“โ€“โ€“
per 1 mol of
โˆ’81.28โ€“โ€“โ€“
per 1 mol of
โˆ’54.19โ€“โ€“โ€“
per 1 mol of
โˆ’121.9โ€“โ€“โ€“
per 1 mol of
โˆ’243.8โ€“โ€“โ€“
per 1 mol of
โˆ’162.6โ€“โ€“โ€“
per 1 mol of
โˆ’162.6โ€“โ€“โ€“

Changes in aqueous solution (6)

Reaction of iron(II) fluoride and nitric acid
6FeF2Crystalline solid + 9HNO3Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
4FeF3Aqueous solution + 2Fe(NO3)3Aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
โˆ’496.1โ€“โ€“โ€“
per 1 mol of
โˆ’82.68โ€“โ€“โ€“
per 1 mol of
โˆ’55.12โ€“โ€“โ€“
per 1 mol of
โˆ’124.0โ€“โ€“โ€“
per 1 mol of
โˆ’248.1โ€“โ€“โ€“
per 1 mol of
โˆ’165.4โ€“โ€“โ€“
per 1 mol of
โˆ’165.4โ€“โ€“โ€“

Changes in aqueous solution (7)

Reaction of iron(II) fluoride and nitric acid
โ—†
ฮ”rG109.5 kJ/mol
K0.66 ร— 10โˆ’19
pK19.18
6FeF2Crystalline solid + 9HNO3Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
4FeF3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
โˆ’608.1109.5โˆ’2405.4โ€“
per 1 mol of
โˆ’101.418.25โˆ’400.90โ€“
per 1 mol of
โˆ’67.5712.17โˆ’267.27โ€“
per 1 mol of
โˆ’152.027.38โˆ’601.35โ€“
per 1 mol of
โˆ’304.154.75โˆ’1202.7โ€“
per 1 mol of
โˆ’202.736.50โˆ’801.80โ€“
per 1 mol of
โˆ’202.736.50โˆ’801.80โ€“

Changes in aqueous solution (8)

Reaction of iron(II) fluoride and nitric acid
6FeF2Crystalline solid + 9HNO3Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
4FeF3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
โˆ’616.5โ€“โ€“โ€“
per 1 mol of
โˆ’102.8โ€“โ€“โ€“
per 1 mol of
โˆ’68.50โ€“โ€“โ€“
per 1 mol of
โˆ’154.1โ€“โ€“โ€“
per 1 mol of
โˆ’308.3โ€“โ€“โ€“
per 1 mol of
โˆ’205.5โ€“โ€“โ€“
per 1 mol of
โˆ’205.5โ€“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
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€“
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (l):Liquid, (g):Gas

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
FeF3 (ai)-1046.4[1]-840.9[1]-357.3[1]โ€“
FeF3 (aq)-1016.3[1]โ€“โ€“โ€“
Fe(NO3)3 (ai)-670.7[1]-338.3[1]123.4[1]โ€“
Fe(NO3)3 (aq)-674.9[1]โ€“โ€“โ€“
Fe(NO3)3 (cr)
9 hydrate
-3285.3[1]โ€“โ€“โ€“
HNO2 (g)
cis
-77.99[1]-42.94[1]248.76[1]44.77[1]
HNO2 (g)
trans
-80.12[1]-45.24[1]249.22[1]46.07[1]
HNO2 (g)-79.5[1]-46.0[1]254.1[1]45.6[1]
HNO2 (ao)-119.2[1]-50.6[1]135.6[1]โ€“
H2O (cr)โ€“โ€“โ€“โ€“
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]
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid

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)