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2FeSe + 12HNO3 → 2Fe(NO3)3 + 2Se + 3N2O4 + 6H2O

The reaction of iron(II) selenide and nitric acid yields iron(III) nitrate, selenium, dinitrogen tetraoxide, 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

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeSeIron(II) selenide2
Reducing
Reducing
HNO3Nitric acid12
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe(NO3)3Iron(III) nitrate2
Oxidized
SeSelenium2
Oxidized
N2O4Dinitrogen tetraoxide3
Reduced
H2OWater6

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of iron(II) selenide and nitric acid
2FeSeCrystalline solid + 12HNO3Ionized aqueous solution
2Fe(NO3)3Ionized aqueous solution + 2SeCrystalline solidhexagonal, gray + 3N2O4Liquid + 6H2OLiquid
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
−476.0
per 1 mol of
−238.0
per 1 mol of
−39.67
per 1 mol of
−238.0
per 1 mol of
−238.0
−158.7
per 1 mol of
−79.33

Changes in aqueous solution (2)

Reaction of iron(II) selenide and nitric acid
2FeSeCrystalline solid + 12HNO3Ionized aqueous solution
2Fe(NO3)3Aqueous solution + 2SeCrystalline solidhexagonal, gray + 3N2O4Liquid + 6H2OLiquid
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
−484.4
per 1 mol of
−242.2
per 1 mol of
−40.37
per 1 mol of
−242.2
per 1 mol of
−242.2
−161.5
per 1 mol of
−80.73

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]
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, (am):Amorphous solid, (l):Liquid, (g):Gas, (ai):Ionized aqueous solution

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(NO3)3 (ai)-670.7[1]-338.3[1]123.4[1]
Fe(NO3)3 (aq)-674.9[1]
Fe(NO3)3 (cr)
9 hydrate
-3285.3[1]
Se (cr)
hexagonal, gray
0[1]0[1]42.442[1]25.363[1]
Se (cr)
monoclinic, red
6.7[1]
Se (vit)5.0[1]
Se (g)227.07[1]187.03[1]176.72[1]20.820[1]
N2O4 (l)-19.50[1]97.54[1]209.2[1]142.7[1]
N2O4 (g)9.16[1]97.89[1]304.29[1]77.28[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]
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (cr):Crystalline solid, (vit):Vitreous liquid, (g):Gas, (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)