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4FeSe + 26HNO3 → 4Fe(NO3)3 + 4SeO2 + 7N2O3↑ + 13H2O

The reaction of iron(II) selenide and nitric acid yields iron(III) nitrate, selenium dioxide, dinitrogen trioxide, 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) selenide4
Reducing
Reducing
HNO3Nitric acid26
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe(NO3)3Iron(III) nitrate4
Oxidized
SeO2Selenium dioxide4
Oxidized
N2O3Dinitrogen trioxide7
Reduced
H2OWater13

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of iron(II) selenide and nitric acid
4FeSeCrystalline solid + 26HNO3Ionized aqueous solution
4Fe(NO3)3Ionized aqueous solution + 4SeO2Aqueous solution + 7N2O3Gas + 13H2OLiquid
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
−1006.5
per 1 mol of
−251.63
per 1 mol of
−38.712
per 1 mol of
−251.63
per 1 mol of
−251.63
−143.79
per 1 mol of
−77.423

Changes in aqueous solution (2)

Reaction of iron(II) selenide and nitric acid
4FeSeCrystalline solid + 26HNO3Ionized aqueous solution
4Fe(NO3)3Aqueous solution + 4SeO2Aqueous solution + 7N2O3Gas + 13H2OLiquid
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
−1023.3
per 1 mol of
−255.82
per 1 mol of
−39.358
per 1 mol of
−255.82
per 1 mol of
−255.82
−146.19
per 1 mol of
−78.715

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]
SeO2 (cr)-225.35[1]
SeO2 (aq)-221.63[1]
N2O3 (l)50.29[1]
N2O3 (g)83.72[1]139.46[1]312.28[1]65.61[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, (l):Liquid, (g):Gas

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)