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6NH4NO3 + 8e− → 7NH3↑ + 3OH− + 5NO3−

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Reduction of ammonium nitrate
6NH4NO3Ammonium nitrate + 8e−Electron
⟶
7NH3↑Ammonia + 3OH−Hydroxide ion + 5NO3−Nitrate ion

Reduction of ammonium nitrate yields ammonia, hydroxide ion, and nitrate 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

Reduction of ammonium nitrate
6NH4NO3Ammonium nitrate + 8e−Electron
⟶
7NH3↑Ammonia + 3OH−Hydroxide ion + 5NO3−Nitrate ion

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 nitrate6
Oxidizing
–
e−Electron8
–
Electron

Products

Chemical formulaNameCoefficientTypeType in general
equation
NH3Ammonia7
Reduced
–
OH−Hydroxide ion3
–
–
NO3−Nitrate ion5
–
–

Thermodynamic changes

Changes in standard condition (1)

Reduction of ammonium nitrate
◆
ΔrG0.23 kJ/mol
K0.91 × 100
pK0.04
6NH4NO3Ionized aqueous solution + 8e−
⟶
7NH3↑Gas + 3OH−Un-ionized aqueous solution + 5NO3−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
−10.330.23488.1−592.9
per 1 mol of
−1.7220.038381.35−98.82
per 1 mol of
Electron
−1.2910.028861.01−74.11
per 1 mol of
−1.4760.032969.73−84.70
per 1 mol of
Hydroxide ion
−3.4430.0767162.7−197.6
per 1 mol of
Nitrate ion
−2.0660.046097.62−118.6

Changes in standard condition (2)

Reduction of ammonium nitrate
◆
ΔrG−70.12 kJ/mol
K1.93 × 1012
pK−12.28
6NH4NO3Ionized aqueous solution + 8e−
⟶
7NH3↑Un-ionized aqueous solution + 3OH−Un-ionized aqueous solution + 5NO3−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
−249.59−70.12−79.9–
per 1 mol of
−41.598−11.69−13.3–
per 1 mol of
Electron
−31.199−8.765−9.99–
per 1 mol of
−35.656−10.02−11.4–
per 1 mol of
Hydroxide ion
−83.197−23.37−26.6–
per 1 mol of
Nitrate ion
−49.918−14.02−16.0–

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]–
OH− (g)-143.5[1]–––
OH− (ao)-229.994[1]-157.244[1]-10.75[1]-148.5[1]
NO3− (ao)-207.36[1]-111.25[1]146.4[1]-86.6[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)