2CH3COOLi 🔥→ O2↑ + 2LiOH + 3C + CH4↑
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- Decomposition of lithium acetate
Decomposition of lithium acetate yields , lithium hydroxide, , 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 lithium 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 lithium acetate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CH3COOLi | Lithium acetate | 2 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Oxidized | – | ||
| LiOH | Lithium hydroxide | 2 | – | – |
| 3 | Redoxed product | – | ||
| 1 | Reduced | – |
Thermodynamic changes
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 |
|---|---|---|---|---|
| CH3COOLi | – | – | – | – |
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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
| LiOH (cr) | -484.93[1] | -438.95[1] | 42.80[1] | 49.66[1] |
| LiOH (g) | -238.1[1] | -242.3[1] | 210.90[1] | 46.02[1] |
| LiOH (ai) | -508.48[1] | -450.58[1] | 2.80[1] | -79.9[1] |
| LiOH (ao) | -508.4[1] | -451.8[1] | 7.1[1] | – |
| LiOH (cr) 1 hydrate | -788.01[1] | -680.95[1] | 71.21[1] | 79.50[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) | -74.81[1] | -50.72[1] | 186.264[1] | 35.309[1] |
| (ao) | -89.04[1] | -34.33[1] | 83.7[1] | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 J · K−1 · mol−1
- ^ ΔfH°, -484.93 kJ · mol−1
- ^ ΔfG°, -438.95 kJ · mol−1
- ^ S°, 42.80 J · K−1 · mol−1
- ^ Cp°, 49.66 J · K−1 · mol−1
- ^ ΔfH°, -238.1 kJ · mol−1
- ^ ΔfG°, -242.3 kJ · mol−1
- ^ S°, 210.90 J · K−1 · mol−1
- ^ Cp°, 46.02 J · K−1 · mol−1
- ^ ΔfH°, -508.48 kJ · mol−1
- ^ ΔfG°, -450.58 kJ · mol−1
- ^ S°, 2.80 J · K−1 · mol−1
- ^ Cp°, -79.9 J · K−1 · mol−1
- ^ ΔfH°, -508.4 kJ · mol−1
- ^ ΔfG°, -451.8 kJ · mol−1
- ^ S°, 7.1 J · K−1 · mol−1
- ^ ΔfH°, -788.01 kJ · mol−1
- ^ ΔfG°, -680.95 kJ · mol−1
- ^ S°, 71.21 J · K−1 · mol−1
- ^ Cp°, 79.50 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°, -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