4(NH4)2CO3 🔥→ NH4NO3 + 4CO↑ + 5H2O + 6NH3↑
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- Decomposition of ammonium carbonate
Decomposition of ammonium carbonate yields ammonium nitrate, carbon monoxide, water, and ammonia (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Decomposition of ammonium carbonate
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
- Thermal decomposition of oxoacid salt with redox
- Oxoacid saltSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of ammonium carbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| (NH4)2CO3 | Ammonium carbonate | 4 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4NO3 | Ammonium nitrate | 1 | Oxidized | – |
| CO | Carbon monoxide | 4 | Reduced | – |
| H2O | Water | 5 | – | – |
| NH3 | Ammonia | 6 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Decomposition of ammonium carbonate◆
ΔrG 722.10 kJ/mol K 0.31 × 10−126 pK 126.51
| 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 | 1280.82 | 722.10 | 1875.1 | – |
per 1 mol of | 320.205 | 180.53 | 468.77 | – |
per 1 mol of | 1280.82 | 722.10 | 1875.1 | – |
per 1 mol of | 320.205 | 180.53 | 468.77 | – |
per 1 mol of | 256.164 | 144.42 | 375.02 | – |
per 1 mol of | 213.470 | 120.35 | 312.52 | – |
Changes in aqueous solution (2)
- Decomposition of ammonium carbonate◆
ΔrG 661.80 kJ/mol K 0.11 × 10−115 pK 115.94
| 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 | 1075.74 | 661.80 | 1388.2 | – |
per 1 mol of | 268.935 | 165.45 | 347.05 | – |
per 1 mol of | 1075.74 | 661.80 | 1388.2 | – |
per 1 mol of | 268.935 | 165.45 | 347.05 | – |
per 1 mol of | 215.148 | 132.36 | 277.64 | – |
per 1 mol of | 179.290 | 110.30 | 231.37 | – |
Changes in aqueous solution (3)
- Decomposition of ammonium carbonate◆
ΔrG 791.18 kJ/mol K 0.25 × 10−138 pK 138.61
| 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 | 1239.08 | 791.18 | 1502.9 | – |
per 1 mol of | 309.770 | 197.79 | 375.73 | – |
per 1 mol of | 1239.08 | 791.18 | 1502.9 | – |
per 1 mol of | 309.770 | 197.79 | 375.73 | – |
per 1 mol of | 247.816 | 158.24 | 300.58 | – |
per 1 mol of | 206.513 | 131.86 | 250.48 | – |
Changes in aqueous solution (4)
- Decomposition of ammonium carbonate◆
ΔrG 730.88 kJ/mol K 0.90 × 10−128 pK 128.04
| 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 | 1034.00 | 730.88 | 1016.0 | – |
per 1 mol of | 258.500 | 182.72 | 254.00 | – |
per 1 mol of | 1034.00 | 730.88 | 1016.0 | – |
per 1 mol of | 258.500 | 182.72 | 254.00 | – |
per 1 mol of | 206.800 | 146.18 | 203.20 | – |
per 1 mol of | 172.333 | 121.81 | 169.33 | – |
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 |
|---|---|---|---|---|
| (NH4)2CO3 (ai) | -942.15[1] | -686.42[1] | 169.9[1] | – |
* (ai):Ionized 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 |
|---|---|---|---|---|
| NH4NO3 (cr) | -365.56[1] | -183.87[1] | 151.08[1] | 139.3[1] |
| NH4NO3 (ai) | -339.87[1] | -190.56[1] | 259.8[1] | -6.7[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] | – |
| 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] |
| 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] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (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°, -942.15 kJ · mol−1
- ^ ΔfG°, -686.42 kJ · mol−1
- ^ S°, 169.9 J · K−1 · mol−1
- ^ ΔfH°, -365.56 kJ · mol−1
- ^ ΔfG°, -183.87 kJ · mol−1
- ^ S°, 151.08 J · K−1 · mol−1
- ^ Cp°, 139.3 J · K−1 · mol−1
- ^ ΔfH°, -339.87 kJ · mol−1
- ^ ΔfG°, -190.56 kJ · mol−1
- ^ S°, 259.8 J · K−1 · mol−1
- ^ Cp°, -6.7 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°, -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
- ^ 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