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6NH4NO3 + 4Fe2O3 🔥→ 3N2H4 + 6Fe(OH)2 + 2Fe(NO3)3

The reaction of ammonium nitrate and iron(III) oxide yields hydrazine, iron(II) hydroxide, and iron(III) nitrate (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
NH4NO3Ammonium nitrate6
Reducing
Reducing
Fe2O3Iron(III) oxide4
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
N2H4Hydrazine3
Oxidized
Fe(OH)2Iron(II) hydroxide6
Reduced
Fe(NO3)3Iron(III) nitrate2

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of ammonium nitrate and iron(III) oxide
ΔrG900.9 kJ/mol
K0.15 × 10−157
pK157.83
6NH4NO3Ionized aqueous solution + 4Fe2O3Crystalline solid
🔥
3N2H4Un-ionized aqueous solution + 6Fe(OH)2Crystalline solidprecipitated + 2Fe(NO3)3Ionized 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
683.6900.9−720
per 1 mol of
113.9150.2−120
per 1 mol of
170.9225.2−180
per 1 mol of
227.9300.3−240
per 1 mol of
113.9150.2−120
per 1 mol of
341.8450.4−360

Changes in aqueous solution (2)

Reaction of ammonium nitrate and iron(III) oxide
6NH4NO3Ionized aqueous solution + 4Fe2O3Crystalline solid
🔥
3N2H4Un-ionized aqueous solution + 6Fe(OH)2Crystalline solidprecipitated + 2Fe(NO3)3Aqueous 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
675.2
per 1 mol of
112.5
per 1 mol of
168.8
per 1 mol of
225.1
per 1 mol of
112.5
per 1 mol of
337.6

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
NH4NO3 (cr)-365.56[1]-183.87[1]151.08[1]139.3[1]
NH4NO3 (ai)-339.87[1]-190.56[1]259.8[1]-6.7[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
N2H4 (l)50.63[1]149.34[1]121.21[1]98.87[1]
N2H4 (g)95.40[1]159.35[1]238.47[1]49.58[1]
N2H4 (ao)34.31[1]128.1[1]138[1]
Fe(OH)2 (cr)
precipitated
-569.0[1]-486.5[1]88[1]
Fe(OH)2 (g)-372[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]
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution

References

List of references

  1. 1