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2NH4SCN + 6Fe2O3 → N2↑ + 2FeS + FeCO3 + 3Fe3O4 + (NH4)2CO3

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Reaction of ammonium thiocyanate and iron(III) oxide
2NH4SCNAmmonium thiocyanate + 6Fe2O3Iron(III) oxide
⟶
N2↑Nitrogen + 2FeSIron(II) sulfide + FeCO3Iron(II) carbonate + 3Fe3O4Iron(II,III) oxide + (NH4)2CO3Ammonium carbonate

The reaction of ammonium thiocyanate and iron(III) oxide yields nitrogen, iron(II) sulfide, iron(II) carbonate, iron(II,III) oxide, and ammonium carbonate (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 thiocyanate and iron(III) oxide
2NH4SCNAmmonium thiocyanate + 6Fe2O3Iron(III) oxide
⟶
N2↑Nitrogen + 2FeSIron(II) sulfide + FeCO3Iron(II) carbonate + 3Fe3O4Iron(II,III) oxide + (NH4)2CO3Ammonium carbonate

General equation

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

Oxidation state of each atom

Reaction of ammonium thiocyanate and iron(III) oxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4SCNAmmonium thiocyanate2
Reducing
Reducing
Fe2O3Iron(III) oxide6
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
N2Nitrogen1
Oxidized
–
FeSIron(II) sulfide2
Reduced
–
FeCO3Iron(II) carbonate1
Reduced
–
Fe3O4Iron(II,III) oxide3
Reduced
–
(NH4)2CO3Ammonium carbonate1
–
–

Thermodynamic changes

Changes in aqueous solution

Reaction of ammonium thiocyanate and iron(III) oxide
◆
ΔrG−173.7 kJ/mol
K2.70 × 1030
pK−30.43
2NH4SCNIonized aqueous solution + 6Fe2O3Crystalline solid
⟶
N2↑Gas + 2FeSCrystalline solidiron-rich pyrrhotite, α + FeCO3Crystalline solidsiderite + 3Fe3O4Crystalline solid + (NH4)2CO3Ionized aqueous solution
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
−180.6−173.7−25.6–
−90.30−86.85−12.8–
per 1 mol of
−30.10−28.95−4.27–
per 1 mol of
−180.6−173.7−25.6–
per 1 mol of
−90.30−86.85−12.8–
per 1 mol of
−180.6−173.7−25.6–
per 1 mol of
−60.20−57.90−8.53–
per 1 mol of
−180.6−173.7−25.6–

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
NH4SCN (cr)-78.7[1]–––
NH4SCN (ai)-56.07[1]13.40[1]257.7[1]39.7[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
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
N2 (g)0[1]0[1]191.61[1]29.125[1]
FeS (cr)
iron-rich pyrrhotite, α
-100.0[1]-100.4[1]60.29[1]50.54[1]
FeCO3 (cr)
siderite
-740.57[1]-666.67[1]92.9[1]82.13[1]
Fe3O4 (cr)-1118.4[1]-1015.4[1]146.4[1]143.43[1]
(NH4)2CO3 (ai)-942.15[1]-686.42[1]169.9[1]–
* (g):Gas, (cr):Crystalline solid, (ai):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)