6NH4HCO3 + 2e− → 3(NH4)2CO3 + CO↑ + 2H3O+ + 2CO32−
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- Reduction of ammonium hydrogencarbonate
- 6NH4HCO3Ammonium hydrogencarbonate + 2e−Electron3(NH4)2CO3Ammonium carbonate + CO↑Carbon monoxide + 2H3O+Hydronium ion + 2CO32−Carbonate ion⟶
Reduction of ammonium hydrogencarbonate yields ammonium carbonate, carbon monoxide, hydronium ion, and carbonate ion (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reduction of ammonium hydrogencarbonate
- 6NH4HCO3Ammonium hydrogencarbonate + 2e−Electron3(NH4)2CO3Ammonium carbonate + CO↑Carbon monoxide + 2H3O+Hydronium ion + 2CO32−Carbonate ion⟶
General equation
- Reduction of reducible species
- ReactantOxidizing agent + e− ⟶ ProductReduction product
Oxidation state of each atom
- Reduction of ammonium hydrogencarbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4HCO3 | Ammonium hydrogencarbonate | 6 | Oxidizing | – |
| e− | Electron | 2 | – | Electron |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| (NH4)2CO3 | Ammonium carbonate | 3 | – | – |
| CO | Carbon monoxide | 1 | Reduced | – |
| H3O+ | Hydronium ion | 2 | – | – |
| CO32− | Carbonate ion | 2 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reduction of ammonium hydrogencarbonate◆
ΔrG 270.11 kJ/mol K 0.48 × 10−47 pK 47.32
| 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 | 84.09 | 270.11 | −494.2 | – |
per 1 mol of | 14.02 | 45.018 | −82.37 | – |
per 1 mol of Electron | 42.05 | 135.06 | −247.1 | – |
per 1 mol of | 28.03 | 90.037 | −164.7 | – |
per 1 mol of | 84.09 | 270.11 | −494.2 | – |
per 1 mol of Hydronium ion | 42.05 | 135.06 | −247.1 | – |
per 1 mol of Carbonate ion | 42.05 | 135.06 | −247.1 | – |
Changes in aqueous solution (2)
- Reduction of ammonium hydrogencarbonate◆
ΔrG 287.38 kJ/mol K 0.45 × 10−50 pK 50.35
| 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 | 73.65 | 287.38 | −587.3 | – |
per 1 mol of | 12.28 | 47.897 | −97.88 | – |
per 1 mol of Electron | 36.83 | 143.69 | −293.6 | – |
per 1 mol of | 24.55 | 95.793 | −195.8 | – |
per 1 mol of | 73.65 | 287.38 | −587.3 | – |
per 1 mol of Hydronium ion | 36.83 | 143.69 | −293.6 | – |
per 1 mol of Carbonate ion | 36.83 | 143.69 | −293.6 | – |
Changes in aqueous solution (3)
- Reduction of ammonium hydrogencarbonate
| 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 | 67.3 | – | – | – |
per 1 mol of | 11.2 | – | – | – |
per 1 mol of Electron | 33.6 | – | – | – |
per 1 mol of | 22.4 | – | – | – |
per 1 mol of | 67.3 | – | – | – |
per 1 mol of Hydronium ion | 33.6 | – | – | – |
per 1 mol of Carbonate ion | 33.6 | – | – | – |
Changes in aqueous solution (4)
- Reduction of ammonium hydrogencarbonate
| 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 | 56.9 | – | – | – |
per 1 mol of | 9.48 | – | – | – |
per 1 mol of Electron | 28.4 | – | – | – |
per 1 mol of | 19.0 | – | – | – |
per 1 mol of | 56.9 | – | – | – |
per 1 mol of Hydronium ion | 28.4 | – | – | – |
per 1 mol of Carbonate ion | 28.4 | – | – | – |
Thermodynamic data of reactants
| Chemical formula | Standard 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 formula | Standard 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] | – |
| CO (g) | -110.525[1] | -137.168[1] | 197.674[1] | 29.142[1] |
| CO (ao) | -120.96[1] | -119.90[1] | 104.6[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] | – |
* (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -849.4 kJ · mol−1
- ^ ΔfG°, -665.9 kJ · mol−1
- ^ S°, 120.9 J · K−1 · mol−1
- ^ ΔfH°, -824.50 kJ · mol−1
- ^ ΔfG°, -666.07 kJ · mol−1
- ^ S°, 204.6 J · K−1 · mol−1
- ^ ΔfH°, -821.7 kJ · mol−1
- ^ ΔfH°, -942.15 kJ · mol−1
- ^ ΔfG°, -686.42 kJ · mol−1
- ^ S°, 169.9 J · K−1 · mol−1
- ^ ΔfH°, -110.525 kJ · mol−1
- ^ ΔfG°, -137.168 kJ · mol−1
- ^ S°, 197.674 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -120.96 kJ · mol−1
- ^ ΔfG°, -119.90 kJ · mol−1
- ^ S°, 104.6 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -677.14 kJ · mol−1
- ^ ΔfG°, -527.81 kJ · mol−1
- ^ S°, -56.9 J · K−1 · mol−1