You-iggy
  1. Home
  2. Chemical reactions
  3. 4NH4HCO3 + 7O2 → 4NO2 + 4CO2 + 10H2O

4NH4HCO3 + 7O2 → 4NO2 + 4CO2 + 10H2O

Last updated:
Reaction of ammonium hydrogencarbonate and oxygen
4NH4HCO3Ammonium hydrogencarbonate + 7O2Oxygen
⟶
4NO2Nitrogen dioxide + 4CO2Carbon dioxide + 10H2OWater

The reaction of ammonium hydrogencarbonate and oxygen yields nitrogen dioxide, carbon dioxide, and water (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 hydrogencarbonate and oxygen
4NH4HCO3Ammonium hydrogencarbonate + 7O2Oxygen
⟶
4NO2Nitrogen dioxide + 4CO2Carbon dioxide + 10H2OWater

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 hydrogencarbonate and oxygen

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4HCO3Ammonium hydrogencarbonate4
Reducing
Reducing
O2Oxygen7
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NO2Nitrogen dioxide4
Redoxed product
–
CO2Carbon dioxide4
–
–
H2OWater10
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of ammonium hydrogencarbonate and oxygen
◆
ΔrG−1079.9 kJ/mol
K1.55 × 10189
pK−189.19
4NH4HCO3Crystalline solid + 7O2Gas
⟶
4NO2Gas + 4CO2Gas + 10H2OLiquid
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
−902.0−1079.9594.7–
−225.5−269.98148.7–
per 1 mol of
−128.9−154.2784.96–
per 1 mol of
−225.5−269.98148.7–
per 1 mol of
−225.5−269.98148.7–
per 1 mol of
−90.20−107.9959.47–

Changes in aqueous solution (1)

Reaction of ammonium hydrogencarbonate and oxygen
◆
ΔrG−1194.0 kJ/mol
K1.51 × 10209
pK−209.18
4NH4HCO3Ionized aqueous solution + 7O2Un-ionized aqueous solution
⟶
4NO2Gas + 4CO2Gas + 10H2OLiquid
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
−919.7−1194.0919.6–
−229.9−298.50229.9–
per 1 mol of
−131.4−170.57131.4–
per 1 mol of
−229.9−298.50229.9–
per 1 mol of
−229.9−298.50229.9–
per 1 mol of
−91.97−119.4091.96–

Changes in aqueous solution (2)

Reaction of ammonium hydrogencarbonate and oxygen
◆
ΔrG−1160.5 kJ/mol
K2.05 × 10203
pK−203.31
4NH4HCO3Ionized aqueous solution + 7O2Un-ionized aqueous solution
⟶
4NO2Gas + 4CO2Un-ionized aqueous solution + 10H2OLiquid
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
−1000.9−1160.5535.0–
−250.22−290.13133.8–
per 1 mol of
−142.99−165.7976.43–
per 1 mol of
−250.22−290.13133.8–
per 1 mol of
−250.22−290.13133.8–
per 1 mol of
−100.09−116.0553.50–

Changes in aqueous solution (3)

Reaction of ammonium hydrogencarbonate and oxygen
4NH4HCO3Aqueous solution + 7O2Un-ionized aqueous solution
⟶
4NO2Gas + 4CO2Gas + 10H2OLiquid
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
−930.9–––
−232.7–––
per 1 mol of
−133.0–––
per 1 mol of
−232.7–––
per 1 mol of
−232.7–––
per 1 mol of
−93.09–––

Changes in aqueous solution (4)

Reaction of ammonium hydrogencarbonate and oxygen
4NH4HCO3Aqueous solution + 7O2Un-ionized aqueous solution
⟶
4NO2Gas + 4CO2Un-ionized aqueous solution + 10H2OLiquid
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
−1012.1–––
−253.03–––
per 1 mol of
−144.59–––
per 1 mol of
−253.03–––
per 1 mol of
−253.03–––
per 1 mol of
−101.21–––

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
NH4HCO3 (cr)-849.4[1]-665.9[1]120.9[1]–
NH4HCO3 (ai)-824.50[1]-666.07[1]204.6[1]–
NH4HCO3 (aq)-821.7[1]–––
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (g):Gas, (ao):Un-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
NO2 (g)33.18[1]51.31[1]240.06[1]37.20[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]–
H2O (cr)––––
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid

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)