(NH4)2CO3 🔥→ N2H4 + CH4↑ + O3↑
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- Decomposition of ammonium carbonate
Decomposition of ammonium carbonate yields hydrazine, , and (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 | 1 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
Thermodynamic changes
Changes in aqueous solution (1)
- Decomposition of ammonium carbonate◆
ΔrG 927.0 kJ/mol K 0.40 × 10−162 pK 162.40
| 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 | 1044.4 | 927.0 | 393 | – |
per 1 mol of | 1044.4 | 927.0 | 393 | – |
per 1 mol of | 1044.4 | 927.0 | 393 | – |
| 1044.4 | 927.0 | 393 | – | |
| 1044.4 | 927.0 | 393 | – |
Changes in aqueous solution (2)
- Decomposition of ammonium carbonate◆
ΔrG 937.9 kJ/mol K 0.49 × 10−164 pK 164.31
| 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 | 1027.6 | 937.9 | 300 | – |
per 1 mol of | 1027.6 | 937.9 | 300 | – |
per 1 mol of | 1027.6 | 937.9 | 300 | – |
| 1027.6 | 937.9 | 300 | – | |
| 1027.6 | 937.9 | 300 | – |
Changes in aqueous solution (3)
- Decomposition of ammonium carbonate◆
ΔrG 943.4 kJ/mol K 0.53 × 10−165 pK 165.28
| 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 | 1030.1 | 943.4 | 291 | – |
per 1 mol of | 1030.1 | 943.4 | 291 | – |
per 1 mol of | 1030.1 | 943.4 | 291 | – |
| 1030.1 | 943.4 | 291 | – | |
| 1030.1 | 943.4 | 291 | – |
Changes in aqueous solution (4)
- Decomposition of ammonium carbonate◆
ΔrG 954.3 kJ/mol K 0.65 × 10−167 pK 167.19
| 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 | 1013.3 | 954.3 | 198 | – |
per 1 mol of | 1013.3 | 954.3 | 198 | – |
per 1 mol of | 1013.3 | 954.3 | 198 | – |
| 1013.3 | 954.3 | 198 | – | |
| 1013.3 | 954.3 | 198 | – |
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 |
|---|---|---|---|---|
| N2H4 (l) | 50.63[1] | 149.34[1] | 121.21[1] | 98.87[1] |
| N2H4 (g) | 95.40[1] | 159.35[1] | 238.47[1] | 49.58[1] |
| N2H4 (ao) | 34.31[1] | 128.1[1] | 138[1] | – |
| (g) | -74.81[1] | -50.72[1] | 186.264[1] | 35.309[1] |
| (ao) | -89.04[1] | -34.33[1] | 83.7[1] | – |
| (g) | 142.7[1] | 163.2[1] | 238.93[1] | 39.20[1] |
| (ao) | 125.9[1] | 174.1[1] | 146[1] | – |
* (l):Liquid, (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°, -942.15 kJ · mol−1
- ^ ΔfG°, -686.42 kJ · mol−1
- ^ S°, 169.9 J · K−1 · mol−1
- ^ ΔfH°, 50.63 kJ · mol−1
- ^ ΔfG°, 149.34 kJ · mol−1
- ^ S°, 121.21 J · K−1 · mol−1
- ^ Cp°, 98.87 J · K−1 · mol−1
- ^ ΔfH°, 95.40 kJ · mol−1
- ^ ΔfG°, 159.35 kJ · mol−1
- ^ S°, 238.47 J · K−1 · mol−1
- ^ Cp°, 49.58 J · K−1 · mol−1
- ^ ΔfH°, 34.31 kJ · mol−1
- ^ ΔfG°, 128.1 kJ · mol−1
- ^ S°, 138. J · K−1 · mol−1
- ^ ΔfH°, -74.81 kJ · mol−1
- ^ ΔfG°, -50.72 kJ · mol−1
- ^ S°, 186.264 J · K−1 · mol−1
- ^ Cp°, 35.309 J · K−1 · mol−1
- ^ ΔfH°, -89.04 kJ · mol−1
- ^ ΔfG°, -34.33 kJ · mol−1
- ^ S°, 83.7 J · K−1 · mol−1
- ^ ΔfH°, 142.7 kJ · mol−1
- ^ ΔfG°, 163.2 kJ · mol−1
- ^ S°, 238.93 J · K−1 · mol−1
- ^ Cp°, 39.20 J · K−1 · mol−1
- ^ ΔfH°, 125.9 kJ · mol−1
- ^ ΔfG°, 174.1 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1