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8(NH4)3PO4 → 3N2↑ + 8H3PO4 + 18NH4+ + 18e−

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Oxidation of ammonium phosphate
8(NH4)3PO4Ammonium phosphate
⟶
3N2↑Nitrogen + 8H3PO4Phosphoric acid + 18NH4+Ammonium ion + 18e−Electron

Oxidation of ammonium phosphate yields nitrogen, phosphoric acid, ammonium ion (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

Oxidation of ammonium phosphate
8(NH4)3PO4Ammonium phosphate
⟶
3N2↑Nitrogen + 8H3PO4Phosphoric acid + 18NH4+Ammonium ion + 18e−Electron

General equation

Oxidation of oxidizable species
ReactantReducing agent
⟶
ProductOxidation product + e−

Oxidation state of each atom

Oxidation of ammonium phosphate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)3PO4Ammonium phosphate8
Reducing
–

Products

Chemical formulaNameCoefficientTypeType in general
equation
N2Nitrogen3
Oxidized
–
H3PO4Phosphoric acid8
–
–
NH4+Ammonium ion18
–
–
e−Electron18
–
Electron

Thermodynamic changes

Changes in standard condition (1)

Oxidation of ammonium phosphate
◆
ΔrG−515.1 kJ/mol
K1.74 × 1090
pK−90.24
8(NH4)3PO4Ionized aqueous solution
⟶
3N2↑Gas + 8H3PO4Un-ionized aqueous solution + 18NH4+Un-ionized aqueous solution + 18e−
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
707.3−515.12946–
per 1 mol of
88.41−64.39368.3–
per 1 mol of
235.8−171.7982.0–
per 1 mol of
88.41−64.39368.3–
per 1 mol of
Ammonium ion
39.29−28.62163.7–
per 1 mol of
Electron
39.29−28.62163.7–

Changes in standard condition (2)

Oxidation of ammonium phosphate
◆
ΔrG−515.1 kJ/mol
K1.74 × 1090
pK−90.24
8(NH4)3PO4Ionized aqueous solution
⟶
3N2↑Gas + 8H3PO4Un-ionized aqueous solution + 18NH4+Un-ionized aqueous solution + 18e−
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
707.3−515.12946–
per 1 mol of
88.41−64.39368.3–
per 1 mol of
235.8−171.7982.0–
per 1 mol of
88.41−64.39368.3–
per 1 mol of
Ammonium ion
39.29−28.62163.7–
per 1 mol of
Electron
39.29−28.62163.7–

Changes in standard condition (3)

Oxidation of ammonium phosphate
◆
ΔrG475.6 kJ/mol
K0.48 × 10−83
pK83.32
8(NH4)3PO4Ionized aqueous solution
⟶
3N2↑Gas + 8H3PO4Ionized aqueous solution + 18NH4+Un-ionized aqueous solution + 18e−
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
794.8475.6−82–
per 1 mol of
99.3559.45−10–
per 1 mol of
264.9158.5−27–
per 1 mol of
99.3559.45−10–
per 1 mol of
Ammonium ion
44.1626.42−4.6–
per 1 mol of
Electron
44.1626.42−4.6–

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
(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]–––
* (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]
H3PO4 (cr)-1279.0[1]-1119.1[1]110.50[1]106.06[1]
H3PO4 (l)-1266.9[1]–––
H3PO4 (ai)-1277.4[1]-1018.7[1]-220.3[1]–
H3PO4 (ao)-1288.34[1]-1142.54[1]158.2[1]–
H3PO4 (cr)
0.5 hydrate
-1431.3[1]-1242.1[1]129.16[1]126.02[1]
H3PO4 (cr)
1 hydrate
-1568.83[1]–––
NH4+ (ao)-132.51[1]-79.31[1]113.4[1]79.9[1]
e−––––
* (g):Gas, (cr):Crystalline solid, (l):Liquid, (ai):Ionized aqueous solution, (ao):Un-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)