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FeS + 12HNO3 → Fe(NO3)3 + SO3 + 9NO2↑ + 6H2O

The reaction of iron(II) sulfide and nitric acid yields iron(III) nitrate, sulfur trioxide, nitrogen dioxide, 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
FeSIron(II) sulfide1
Reducing
Reducing
HNO3Nitric acid12
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe(NO3)3Iron(III) nitrate1
Oxidized
SO3Sulfur trioxide1
Oxidized
NO2Nitrogen dioxide9
Reduced
H2OWater6

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of iron(II) sulfide and nitric acid
ΔrG−238.1 kJ/mol
K5.17 × 1041
pK−41.71
FeSCrystalline solidiron-rich pyrrhotite, α + 12HNO3Ionized aqueous solution
Fe(NO3)3Ionized aqueous solution + SO3Crystalline solidβ + 9NO2Gas + 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
46.8−238.1957.0
per 1 mol of
46.8−238.1957.0
per 1 mol of
3.90−19.8479.75
per 1 mol of
46.8−238.1957.0
per 1 mol of
46.8−238.1957.0
per 1 mol of
5.20−26.46106.3
per 1 mol of
7.80−39.68159.5

Changes in aqueous solution (2)

Reaction of iron(II) sulfide and nitric acid
FeSCrystalline solidiron-rich pyrrhotite, α + 12HNO3Ionized aqueous solution
Fe(NO3)3Aqueous solution + SO3Crystalline solidβ + 9NO2Gas + 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
42.6
per 1 mol of
42.6
per 1 mol of
3.55
per 1 mol of
42.6
per 1 mol of
42.6
per 1 mol of
4.73
per 1 mol of
7.10

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
FeS (cr)
iron-rich pyrrhotite, α
-100.0[1]-100.4[1]60.29[1]50.54[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, (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]
SO3 (cr)
β
-454.51[1]-374.21[1]70.7[1]
SO3 (l)-441.04[1]-373.75[1]113.8[1]
SO3 (g)-395.72[1]-371.06[1]256.76[1]50.67[1]
NO2 (g)33.18[1]51.31[1]240.06[1]37.20[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)