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2NH4SCN + 4Fe2O3 → N2O↑ + FeS + 2FeCO3 + 5FeO + (NH4)2S

The reaction of ammonium thiocyanate and iron(III) oxide yields dinitrotgen monoxide, iron(II) sulfide, iron(II) carbonate, iron(II) oxide, and ammonium sulfide (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 reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4SCNAmmonium thiocyanate2
Reducing
Reducing
Fe2O3Iron(III) oxide4
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
N2ODinitrotgen monoxide1
Oxidized
FeSIron(II) sulfide1
Reduced
FeCO3Iron(II) carbonate2
Reduced
FeOIron(II) oxide5
Reduced
(NH4)2SAmmonium sulfide1

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of ammonium thiocyanate and iron(III) oxide
2NH4SCNIonized aqueous solution + 4Fe2O3Crystalline solid
N2OGas + FeSCrystalline solidiron-rich pyrrhotite, α + 2FeCO3Crystalline solidsiderite + 5FeOCrystalline solid + (NH4)2SIonized 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
318.1
159.1
per 1 mol of
79.53
318.1
per 1 mol of
318.1
per 1 mol of
159.1
per 1 mol of
63.62
per 1 mol of
318.1

Changes in aqueous solution (2)

Reaction of ammonium thiocyanate and iron(III) oxide
2NH4SCNIonized aqueous solution + 4Fe2O3Crystalline solid
N2OAqueous solution + FeSCrystalline solidiron-rich pyrrhotite, α + 2FeCO3Crystalline solidsiderite + 5FeOCrystalline solid + (NH4)2SIonized 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
292.1
146.1
per 1 mol of
73.03
292.1
per 1 mol of
292.1
per 1 mol of
146.1
per 1 mol of
58.42
per 1 mol of
292.1

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
N2O (g)82.05[1]104.20[1]219.85[1]38.45[1]
N2O (aq)56.1[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]
FeO (cr)-272.0[1]
(NH4)2S (ai)-231.8[1]-72.6[1]212.1[1]
* (g):Gas, (aq):Aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution

References

List of references

  1. 1