NH4HCO3 🔥→ NH3↑ + CO2↑ + H2O
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- Decomposition of ammonium hydrogencarbonate
Decomposition of ammonium hydrogencarbonate yields ammonia, carbon dioxide, and water (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Decomposition of ammonium hydrogencarbonate
General equation
- Thermal decomposition without redox
- Thermally decomposable substanceLewis conjugate🔥⟶ ProductLewis acid + ProductLewis base
Oxidation state of each atom
- Decomposition of ammonium hydrogencarbonate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NH4HCO3 | Ammonium hydrogencarbonate | 1 | Lewis conjugate | Thermally decomposable |
Products
Thermodynamic changes
Changes in standard condition
- Decomposition of ammonium hydrogencarbonate◆
ΔrG 18.0 kJ/mol K 0.70 × 10−3 pK 3.15
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 | 124.0 | 18.0 | 355.2 | – |
per 1 mol of | 124.0 | 18.0 | 355.2 | – |
per 1 mol of | 124.0 | 18.0 | 355.2 | – |
per 1 mol of | 124.0 | 18.0 | 355.2 | – |
per 1 mol of | 124.0 | 18.0 | 355.2 | – |
Changes in aqueous solution (1)
- Decomposition of ammonium hydrogencarbonate◆
ΔrG 18.13 kJ/mol K 0.67 × 10−3 pK 3.18
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 | 99.05 | 18.13 | 271.5 | – |
per 1 mol of | 99.05 | 18.13 | 271.5 | – |
per 1 mol of | 99.05 | 18.13 | 271.5 | – |
per 1 mol of | 99.05 | 18.13 | 271.5 | – |
per 1 mol of | 99.05 | 18.13 | 271.5 | – |
Changes in aqueous solution (2)
- Decomposition of ammonium hydrogencarbonate◆
ΔrG 26.51 kJ/mol K 0.23 × 10−4 pK 4.64
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 | 78.76 | 26.51 | 175.4 | – |
per 1 mol of | 78.76 | 26.51 | 175.4 | – |
per 1 mol of | 78.76 | 26.51 | 175.4 | – |
per 1 mol of | 78.76 | 26.51 | 175.4 | – |
per 1 mol of | 78.76 | 26.51 | 175.4 | – |
Changes in aqueous solution (3)
- Decomposition of ammonium hydrogencarbonate◆
ΔrG 8.08 kJ/mol K 0.38 × 10−1 pK 1.42
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 | 64.87 | 8.08 | 190.4 | – |
per 1 mol of | 64.87 | 8.08 | 190.4 | – |
per 1 mol of | 64.87 | 8.08 | 190.4 | – |
per 1 mol of | 64.87 | 8.08 | 190.4 | – |
per 1 mol of | 64.87 | 8.08 | 190.4 | – |
Changes in aqueous solution (4)
- Decomposition of ammonium hydrogencarbonate◆
ΔrG 16.46 kJ/mol K 0.13 × 10−2 pK 2.88
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 | 44.58 | 16.46 | 94.2 | – |
per 1 mol of | 44.58 | 16.46 | 94.2 | – |
per 1 mol of | 44.58 | 16.46 | 94.2 | – |
per 1 mol of | 44.58 | 16.46 | 94.2 | – |
per 1 mol of | 44.58 | 16.46 | 94.2 | – |
Changes in aqueous solution (5)
- Decomposition 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 | 96.3 | – | – | – |
per 1 mol of | 96.3 | – | – | – |
per 1 mol of | 96.3 | – | – | – |
per 1 mol of | 96.3 | – | – | – |
per 1 mol of | 96.3 | – | – | – |
Changes in aqueous solution (6)
- Decomposition 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 | 76.0 | – | – | – |
per 1 mol of | 76.0 | – | – | – |
per 1 mol of | 76.0 | – | – | – |
per 1 mol of | 76.0 | – | – | – |
per 1 mol of | 76.0 | – | – | – |
Changes in aqueous solution (7)
- Decomposition 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 | 62.1 | – | – | – |
per 1 mol of | 62.1 | – | – | – |
per 1 mol of | 62.1 | – | – | – |
per 1 mol of | 62.1 | – | – | – |
per 1 mol of | 62.1 | – | – | – |
Changes in aqueous solution (8)
- Decomposition 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 | 41.8 | – | – | – |
per 1 mol of | 41.8 | – | – | – |
per 1 mol of | 41.8 | – | – | – |
per 1 mol of | 41.8 | – | – | – |
per 1 mol of | 41.8 | – | – | – |
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] | – | – | – |
* (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 |
---|---|---|---|---|
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] | – |
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
- 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°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ ΔfH°, -393.509 kJ · mol−1
- ^ ΔfG°, -394.359 kJ · mol−1
- ^ S°, 213.74 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -413.80 kJ · mol−1
- ^ ΔfG°, -385.98 kJ · mol−1
- ^ S°, 117.6 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°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1