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  3. 13NH4HCO3 + 8e^− → 13NH4^+ + 3H3O^+ + 12CO3^2− + CH4↑

13NH4HCO3 + 8e− → 13NH4+ + 3H3O+ + 12CO32− + CH4↑

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Reduction of ammonium hydrogencarbonate
13NH4HCO3Ammonium hydrogencarbonate + 8e−Electron
⟶
13NH4+Ammonium ion + 3H3O+Hydronium ion + 12CO32−Carbonate ion + CH4↑Methane

Reduction of ammonium hydrogencarbonate yields ammonium ion, hydronium ion, carbonate ion, and methane (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 hydrogencarbonate
13NH4HCO3Ammonium hydrogencarbonate + 8e−Electron
⟶
13NH4+Ammonium ion + 3H3O+Hydronium ion + 12CO32−Carbonate ion + CH4↑Methane

General equation

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

Oxidation state of each atom

Reduction of ammonium hydrogencarbonate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4HCO3Ammonium hydrogencarbonate13
Oxidizing
–
e−Electron8
–
Electron

Products

Chemical formulaNameCoefficientTypeType in general
equation
NH4+Ammonium ion13
–
–
H3O+Hydronium ion3
–
–
CO32−Carbonate ion12
–
–
CH4Methane1
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reduction of ammonium hydrogencarbonate
◆
ΔrG532.05 kJ/mol
K0.61 × 10−93
pK93.21
13NH4HCO3Ionized aqueous solution + 8e−
⟶
13NH4+Un-ionized aqueous solution + 3H3O+Un-ionized aqueous solution + 12CO32−Un-ionized aqueous solution + CH4↑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
−62.11532.05−1472.4–
−4.77840.927−113.26–
per 1 mol of
Electron
−7.76466.506−184.05–
per 1 mol of
Ammonium ion
−4.77840.927−113.26–
per 1 mol of
Hydronium ion
−20.70177.35−490.80–
per 1 mol of
Carbonate ion
−5.17644.337−122.70–
per 1 mol of
−62.11532.05−1472.4–

Changes in standard condition (2)

Reduction of ammonium hydrogencarbonate
◆
ΔrG548.44 kJ/mol
K0.83 × 10−96
pK96.08
13NH4HCO3Ionized aqueous solution + 8e−
⟶
13NH4+Un-ionized aqueous solution + 3H3O+Un-ionized aqueous solution + 12CO32−Un-ionized aqueous solution + CH4↑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
−76.34548.44−1575.0–
−5.87242.188−121.15–
per 1 mol of
Electron
−9.54368.555−196.88–
per 1 mol of
Ammonium ion
−5.87242.188−121.15–
per 1 mol of
Hydronium ion
−25.45182.81−525.00–
per 1 mol of
Carbonate ion
−6.36245.703−131.25–
per 1 mol of
−76.34548.44−1575.0–

Changes in standard condition (3)

Reduction of ammonium hydrogencarbonate
13NH4HCO3Aqueous solution + 8e−
⟶
13NH4+Un-ionized aqueous solution + 3H3O+Un-ionized aqueous solution + 12CO32−Un-ionized aqueous solution + CH4↑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
−98.5–––
−7.58–––
per 1 mol of
Electron
−12.3–––
per 1 mol of
Ammonium ion
−7.58–––
per 1 mol of
Hydronium ion
−32.8–––
per 1 mol of
Carbonate ion
−8.21–––
per 1 mol of
−98.5–––

Changes in standard condition (4)

Reduction of ammonium hydrogencarbonate
13NH4HCO3Aqueous solution + 8e−
⟶
13NH4+Un-ionized aqueous solution + 3H3O+Un-ionized aqueous solution + 12CO32−Un-ionized aqueous solution + CH4↑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
−112.7–––
−8.669–––
per 1 mol of
Electron
−14.09–––
per 1 mol of
Ammonium ion
−8.669–––
per 1 mol of
Hydronium ion
−37.57–––
per 1 mol of
Carbonate ion
−9.392–––
per 1 mol of
−112.7–––

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]–––
e−––––
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):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
NH4+ (ao)-132.51[1]-79.31[1]113.4[1]79.9[1]
H3O+ (ao)-285.830[1]-237.129[1]69.91[1]75.291[1]
CO32− (ao)-677.14[1]-527.81[1]-56.9[1]–
CH4 (g)-74.81[1]-50.72[1]186.264[1]35.309[1]
CH4 (ao)-89.04[1]-34.33[1]83.7[1]–
* (ao):Un-ionized aqueous solution, (g):Gas

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)