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2NH4NO3 + 2e− → 2NH3↑ + 2NO3− + H2↑

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Reduction of ammonium nitrate
2NH4NO3Ammonium nitrate + 2e−Electron
⟶
2NH3↑Ammonia + 2NO3−Nitrate ion + H2↑Hydrogen

Reduction of ammonium nitrate yields ammonia, nitrate ion, and hydrogen (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

Reduction of ammonium nitrate
2NH4NO3Ammonium nitrate + 2e−Electron
⟶
2NH3↑Ammonia + 2NO3−Nitrate ion + H2↑Hydrogen

General equation

Reduction of reducible species
ReactantOxidizing agent + e−
⟶
ProductReduction product

Oxidation state of each atom

Reduction of ammonium nitrate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4NO3Ammonium nitrate2
Oxidizing
–
e−Electron2
–
Electron

Products

Chemical formulaNameCoefficientTypeType in general
equation
NH3Ammonia2
–
–
NO3−Nitrate ion2
–
–
H2Hydrogen1
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reduction of ammonium nitrate
◆
ΔrG125.72 kJ/mol
K0.94 × 10−22
pK22.03
2NH4NO3Ionized aqueous solution + 2e−
⟶
2NH3↑Gas + 2NO3−Un-ionized aqueous solution + H2↑Gas
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
172.80125.72288.8−60.9
per 1 mol of
86.40062.860144.4−30.4
per 1 mol of
Electron
86.40062.860144.4−30.4
per 1 mol of
86.40062.860144.4−30.4
per 1 mol of
Nitrate ion
86.40062.860144.4−30.4
per 1 mol of
172.80125.72288.8−60.9

Changes in standard condition (2)

Reduction of ammonium nitrate
◆
ΔrG143.3 kJ/mol
K0.79 × 10−25
pK25.11
2NH4NO3Ionized aqueous solution + 2e−
⟶
2NH3↑Gas + 2NO3−Un-ionized aqueous solution + H2↑Un-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
168.6143.3735–
per 1 mol of
84.3071.65368–
per 1 mol of
Electron
84.3071.65368–
per 1 mol of
84.3071.65368–
per 1 mol of
Nitrate ion
84.3071.65368–
per 1 mol of
168.6143.3735–

Changes in standard condition (3)

Reduction of ammonium nitrate
◆
ΔrG105.62 kJ/mol
K0.31 × 10−18
pK18.50
2NH4NO3Ionized aqueous solution + 2e−
⟶
2NH3↑Un-ionized aqueous solution + 2NO3−Un-ionized aqueous solution + H2↑Gas
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
104.44105.62126.5–
per 1 mol of
52.22052.81063.25–
per 1 mol of
Electron
52.22052.81063.25–
per 1 mol of
52.22052.81063.25–
per 1 mol of
Nitrate ion
52.22052.81063.25–
per 1 mol of
104.44105.62126.5–

Changes in standard condition (4)

Reduction of ammonium nitrate
◆
ΔrG123.2 kJ/mol
K0.26 × 10−21
pK21.58
2NH4NO3Ionized aqueous solution + 2e−
⟶
2NH3↑Un-ionized aqueous solution + 2NO3−Un-ionized aqueous solution + H2↑Un-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
100.2123.2573–
per 1 mol of
50.1061.60287–
per 1 mol of
Electron
50.1061.60287–
per 1 mol of
50.1061.60287–
per 1 mol of
Nitrate ion
50.1061.60287–
per 1 mol of
100.2123.2573–

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]
e−––––
* (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
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[1]–
NO3− (ao)-207.36[1]-111.25[1]146.4[1]-86.6[1]
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
* (g):Gas, (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)