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CH3COONH4 + HNO3 → (NH4)2CO3 + CO2↑

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Reaction of ammonium acetate and nitric acid
CH3COONH4Ammonium acetate + HNO3Nitric acid
⟶
(NH4)2CO3Ammonium carbonate + CO2↑Carbon dioxide

The reaction of ammonium acetate and nitric acid yields ammonium carbonate and carbon dioxide (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

Reaction of ammonium acetate and nitric acid
CH3COONH4Ammonium acetate + HNO3Nitric acid
⟶
(NH4)2CO3Ammonium carbonate + CO2↑Carbon dioxide

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of ammonium acetate and nitric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CH3COONH4Ammonium acetate1
Reducing
Reducing
HNO3Nitric acid1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2CO3Ammonium carbonate1
Redoxed product
–
CO2Carbon dioxide1
Oxidized
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of ammonium acetate and nitric acid
◆
ΔrG−520.92 kJ/mol
K1.82 × 1091
pK−91.26
CH3COONH4Ionized aqueous solution + HNO3Ionized aqueous solution
⟶
(NH4)2CO3Ionized aqueous solution + CO2↑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
−509.78−520.9237.2–
per 1 mol of
−509.78−520.9237.2–
per 1 mol of
−509.78−520.9237.2–
per 1 mol of
−509.78−520.9237.2–
per 1 mol of
−509.78−520.9237.2–

Changes in aqueous solution (2)

Reaction of ammonium acetate and nitric acid
◆
ΔrG−512.54 kJ/mol
K6.21 × 1089
pK−89.79
CH3COONH4Ionized aqueous solution + HNO3Ionized aqueous solution
⟶
(NH4)2CO3Ionized aqueous solution + CO2↑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
−530.07−512.54−58.9–
per 1 mol of
−530.07−512.54−58.9–
per 1 mol of
−530.07−512.54−58.9–
per 1 mol of
−530.07−512.54−58.9–
per 1 mol of
−530.07−512.54−58.9–

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
CH3COONH4 (cr)-616.14[1]–––
CH3COONH4 (ai)-618.52[1]-448.61[1]200.0[1]73.6[1]
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas

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
(NH4)2CO3 (ai)-942.15[1]-686.42[1]169.9[1]–
CO2 (g)-393.509[1]-394.359[1]213.74[1]37.11[1]
CO2 (ao)-413.80[1]-385.98[1]117.6[1]–
* (ai):Ionized aqueous solution, (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)