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(NH4)3PO4 + 39Fe2O3 → Fe(NO3)3 + 24Fe3O4 + FePO4 + 4Fe(OH)3

The reaction of ammonium phosphate and iron(III) oxide yields iron(III) nitrate, iron(II,III) oxide, iron(III) phosphate, and iron(III) hydroxide (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
(NH4)3PO4Ammonium phosphate1
Reducing
Reducing
Fe2O3Iron(III) oxide39
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe(NO3)3Iron(III) nitrate1
Oxidized
Fe3O4Iron(II,III) oxide24
Reduced
FePO4Iron(III) phosphate1
Fe(OH)3Iron(III) hydroxide4

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of ammonium phosphate and iron(III) oxide
(NH4)3PO4Ionized aqueous solution + 39Fe2O3Crystalline solid
Fe(NO3)3Ionized aqueous solution + 24Fe3O4Crystalline solid + FePO4Crystalline solid + 4Fe(OH)3Un-ionized 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution (2)

Reaction of ammonium phosphate and iron(III) oxide
(NH4)3PO4Ionized aqueous solution + 39Fe2O3Crystalline solid
Fe(NO3)3Aqueous solution + 24Fe3O4Crystalline solid + FePO4Crystalline solid + 4Fe(OH)3Un-ionized 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

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
(NH4)3PO4 (cr)-1671.9[1]
(NH4)3PO4 (ai)-1674.9[1]-1256.6[1]117[1]
(NH4)3PO4 (cr)
3 hydrate
-2555.6[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
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]
Fe3O4 (cr)-1118.4[1]-1015.4[1]146.4[1]143.43[1]
FePO4 (cr)-1297.5[1]
FePO4 (cr)
2 hydrate
strengite
-1888.2[1]-1657.5[1]171.25[1]180.54[1]
Fe(OH)3 (cr)
precipitated
-823.0[1]-696.5[1]106.7[1]
Fe(OH)3 (ao)-659.3[1]
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (cr):Crystalline solid, (ao):Un-ionized aqueous solution

References

List of references

  1. 1