2CH3COOK 🔥→ K2O + 3CO↑ + C + 3H2↑
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- Decomposition of potassium acetate
Decomposition of potassium acetate yields potassium oxide, carbon monoxide, , 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 potassium 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 potassium acetate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CH3COOK | Potassium acetate | 2 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2O | Potassium oxide | 1 | – | – |
| CO | Carbon monoxide | 3 | Redoxed product | – |
| 1 | Oxidized | – | ||
| 3 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Decomposition of potassium 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 | 752.9 | – | – | – |
per 1 mol of | 376.4 | – | – | – |
per 1 mol of | 752.9 | – | – | – |
per 1 mol of | 251.0 | – | – | – |
| 752.9 | – | – | – | |
| 251.0 | – | – | – |
Changes in standard condition (2)
- Decomposition of potassium 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 | 754.8 | – | – | – |
per 1 mol of | 377.4 | – | – | – |
per 1 mol of | 754.8 | – | – | – |
per 1 mol of | 251.6 | – | – | – |
| 754.8 | – | – | – | |
| 251.6 | – | – | – |
Changes in aqueous solution (1)
- Decomposition of potassium acetate◆
ΔrG 571.6 kJ/mol K 0.72 × 10−100 pK 100.14
| 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 | 783.7 | 571.6 | 706.7 | 235.1 |
per 1 mol of | 391.9 | 285.8 | 353.4 | 117.5 |
per 1 mol of | 783.7 | 571.6 | 706.7 | 235.1 |
per 1 mol of | 261.2 | 190.5 | 235.6 | 78.37 |
| 783.7 | 571.6 | 706.7 | 235.1 | |
| 261.2 | 190.5 | 235.6 | 78.37 |
Changes in aqueous solution (2)
- Decomposition of potassium acetate◆
ΔrG 624.4 kJ/mol K 0.41 × 10−109 pK 109.39
| 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 | 771.1 | 624.4 | 2046 | – |
per 1 mol of | 385.6 | 312.2 | 1023 | – |
per 1 mol of | 771.1 | 624.4 | 2046 | – |
per 1 mol of | 257.0 | 208.1 | 682.0 | – |
| 771.1 | 624.4 | 2046 | – | |
| 257.0 | 208.1 | 682.0 | – |
Changes in aqueous solution (3)
- Decomposition of potassium acetate◆
ΔrG 623.4 kJ/mol K 0.61 × 10−109 pK 109.21
| 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 | 752.4 | 623.4 | 427.5 | – |
per 1 mol of | 376.2 | 311.7 | 213.8 | – |
per 1 mol of | 752.4 | 623.4 | 427.5 | – |
per 1 mol of | 250.8 | 207.8 | 142.5 | – |
| 752.4 | 623.4 | 427.5 | – | |
| 250.8 | 207.8 | 142.5 | – |
Changes in aqueous solution (4)
- Decomposition of potassium acetate◆
ΔrG 676.2 kJ/mol K 0.34 × 10−118 pK 118.47
| 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 | 739.8 | 676.2 | 1766 | – |
per 1 mol of | 369.9 | 338.1 | 883.0 | – |
per 1 mol of | 739.8 | 676.2 | 1766 | – |
per 1 mol of | 246.6 | 225.4 | 588.7 | – |
| 739.8 | 676.2 | 1766 | – | |
| 246.6 | 225.4 | 588.7 | – |
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 |
|---|---|---|---|---|
| CH3COOK (cr) | -723.0[1] | – | – | – |
| CH3COOK (ai) | -738.39[1] | -652.58[1] | 189.1[1] | 15.5[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 |
|---|---|---|---|---|
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[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] | – |
| (cr) graphite | 0[1] | 0[1] | 5.740[1] | 8.527[1] |
| (cr) diamond | 1.895[1] | 2.900[1] | 2.377[1] | 6.113[1] |
| (g) | 716.682[1] | 671.257[1] | 158.096[1] | 20.838[1] |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (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°, -723.0 kJ · mol−1
- ^ ΔfH°, -738.39 kJ · mol−1
- ^ ΔfG°, -652.58 kJ · mol−1
- ^ S°, 189.1 J · K−1 · mol−1
- ^ Cp°, 15.5 J · K−1 · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 5.740 J · K−1 · mol−1
- ^ Cp°, 8.527 J · K−1 · mol−1
- ^ ΔfH°, 1.895 kJ · mol−1
- ^ ΔfG°, 2.900 kJ · mol−1
- ^ S°, 2.377 J · K−1 · mol−1
- ^ Cp°, 6.113 J · K−1 · mol−1
- ^ ΔfH°, 716.682 kJ · mol−1
- ^ ΔfG°, 671.257 kJ · mol−1
- ^ S°, 158.096 J · K−1 · mol−1
- ^ Cp°, 20.838 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfG°, -322.1 kJ · mol−1 - p.280
- ^ S°, 94.1 J · K−1 · mol−1 - p.280
- ^ Cp°, 83.7 J · K−1 · mol−1 - p.280