8CH3COONH4 🔥→ 4N2H4 + 7CH3COOH + 2H2O + 2CH4↑
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- Decomposition of ammonium acetate
Decomposition of ammonium acetate yields hydrazine, acetic acid, water, 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 acetate
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 acetate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CH3COONH4 | Ammonium acetate | 8 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
Thermodynamic changes
Changes in standard condition
- Decomposition of ammonium acetate
| 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 | 1018.9 | – | – | – |
per 1 mol of | 127.36 | – | – | – |
per 1 mol of | 254.72 | – | – | – |
per 1 mol of | 145.56 | – | – | – |
per 1 mol of | 509.45 | – | – | – |
| 509.45 | – | – | – |
Changes in aqueous solution (1)
- Decomposition of ammonium acetate◆
ΔrG 750.4 kJ/mol K 0.34 × 10−131 pK 131.46
| 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 | 963.80 | 750.4 | 715 | – |
per 1 mol of | 120.47 | 93.80 | 89.4 | – |
per 1 mol of | 240.95 | 187.6 | 179 | – |
per 1 mol of | 137.69 | 107.2 | 102 | – |
per 1 mol of | 481.90 | 375.2 | 358 | – |
| 481.90 | 375.2 | 358 | – |
Changes in aqueous solution (2)
- Decomposition of ammonium acetate◆
ΔrG 783.1 kJ/mol K 0.64 × 10−137 pK 137.19
| 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 | 935.34 | 783.1 | 510 | – |
per 1 mol of | 116.92 | 97.89 | 63.8 | – |
per 1 mol of | 233.84 | 195.8 | 128 | – |
per 1 mol of | 133.62 | 111.9 | 72.9 | – |
per 1 mol of | 467.67 | 391.6 | 255 | – |
| 467.67 | 391.6 | 255 | – |
Changes in aqueous solution (3)
- Decomposition of ammonium acetate◆
ΔrG 940.4 kJ/mol K 0.18 × 10−164 pK 164.75
| 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 | 962.05 | 940.4 | 71 | – |
per 1 mol of | 120.26 | 117.5 | 8.9 | – |
per 1 mol of | 240.51 | 235.1 | 18 | – |
per 1 mol of | 137.44 | 134.3 | 10 | – |
per 1 mol of | 481.02 | 470.2 | 36 | – |
| 481.02 | 470.2 | 36 | – |
Changes in aqueous solution (4)
- Decomposition of ammonium acetate◆
ΔrG 973.2 kJ/mol K 0.32 × 10−170 pK 170.50
| 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 | 933.59 | 973.2 | −135 | – |
per 1 mol of | 116.70 | 121.7 | −16.9 | – |
per 1 mol of | 233.40 | 243.3 | −33.8 | – |
per 1 mol of | 133.37 | 139.0 | −19.3 | – |
per 1 mol of | 466.80 | 486.6 | −67.5 | – |
| 466.80 | 486.6 | −67.5 | – |
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 |
|---|---|---|---|---|
| CH3COONH4 (cr) | -616.14[1] | – | – | – |
| CH3COONH4 (ai) | -618.52[1] | -448.61[1] | 200.0[1] | 73.6[1] |
* (cr):Crystalline solid, (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] | – |
| CH3COOH (l) | -484.5[1] | -389.9[1] | 159.8[1] | 124.3[1] |
| CH3COOH (g) | -432.25[1] | -374.0[1] | 282.5[1] | 66.5[1] |
| CH3COOH (ai) | -486.01[1] | -369.31[1] | 86.6[1] | -6.3[1] |
| CH3COOH (ao) | -485.76[1] | -396.46[1] | 178.7[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) | -74.81[1] | -50.72[1] | 186.264[1] | 35.309[1] |
| (ao) | -89.04[1] | -34.33[1] | 83.7[1] | – |
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (ai):Ionized aqueous solution, (cr):Crystalline solid
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°, -616.14 kJ · mol−1
- ^ ΔfH°, -618.52 kJ · mol−1
- ^ ΔfG°, -448.61 kJ · mol−1
- ^ S°, 200.0 J · K−1 · mol−1
- ^ Cp°, 73.6 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°, -484.5 kJ · mol−1
- ^ ΔfG°, -389.9 kJ · mol−1
- ^ S°, 159.8 J · K−1 · mol−1
- ^ Cp°, 124.3 J · K−1 · mol−1
- ^ ΔfH°, -432.25 kJ · mol−1
- ^ ΔfG°, -374.0 kJ · mol−1
- ^ S°, 282.5 J · K−1 · mol−1
- ^ Cp°, 66.5 J · K−1 · mol−1
- ^ ΔfH°, -486.01 kJ · mol−1
- ^ ΔfG°, -369.31 kJ · mol−1
- ^ S°, 86.6 J · K−1 · mol−1
- ^ Cp°, -6.3 J · K−1 · mol−1
- ^ ΔfH°, -485.76 kJ · mol−1
- ^ ΔfG°, -396.46 kJ · mol−1
- ^ S°, 178.7 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°, -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