Li2CO3 🔥→ Li2O + CO2↑
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- Decomposition of lithium carbonate
Decomposition of lithium carbonate yields lithium oxide and carbon dioxide (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
- Thermal decomposition without redox
- Thermal decomposition of oxoacid salt without redox
- Thermal decomposition of salt of oxoacid and hydroxide base
Table of contents
Reaction data
Chemical equation
- Decomposition of lithium carbonate
General equation
- Thermal decomposition without redox
- Thermally decomposable substanceLewis conjugate🔥⟶ ProductLewis acid + ProductLewis base
- Thermal decomposition of oxoacid salt without redox
- Oxoacid saltLewis conjugate🔥⟶ Basic oxideLewis base + Acidic oxideLewis acid + (H2O)
- Thermal decomposition of salt of oxoacid and hydroxide base
- Salt of oxoacid and hydroxide baseLewis conjugate🔥⟶ Basic oxideLewis base + Acidic oxideLewis acid
Oxidation state of each atom
- Decomposition of lithium carbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Li2CO3 | Lithium carbonate | 1 | Lewis conjugate | Thermally decomposable Oxoacid salt Salt of oxoacid and hydroxide base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Li2O | Lithium oxide | 1 | Lewis acid Lewis base | – Basic oxide |
| CO2 | Carbon dioxide | 1 | Lewis acid | – Acidic oxide |
Thermodynamic changes
Changes in standard condition
- Decomposition of lithium carbonate◆
ΔrG 176.52 kJ/mol K 0.12 × 10−30 pK 30.92
| 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 | 224.5 | 176.52 | 160.94 | −7.91 |
per 1 mol of | 224.5 | 176.52 | 160.94 | −7.91 |
per 1 mol of | 224.5 | 176.52 | 160.94 | −7.91 |
per 1 mol of | 224.5 | 176.52 | 160.94 | −7.91 |
Changes in aqueous solution (1)
- Decomposition of lithium carbonate◆
ΔrG 176.52 kJ/mol K 0.12 × 10−30 pK 30.92
| 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 | 224.5 | 176.52 | 160.94 | −7.91 |
per 1 mol of | 224.5 | 176.52 | 160.94 | −7.91 |
per 1 mol of | 224.5 | 176.52 | 160.94 | −7.91 |
per 1 mol of | 224.5 | 176.52 | 160.94 | −7.91 |
Changes in aqueous solution (2)
- Decomposition of lithium carbonate◆
ΔrG 184.90 kJ/mol K 0.40 × 10−32 pK 32.39
| 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 | 204.2 | 184.90 | 64.8 | – |
per 1 mol of | 204.2 | 184.90 | 64.8 | – |
per 1 mol of | 204.2 | 184.90 | 64.8 | – |
per 1 mol of | 204.2 | 184.90 | 64.8 | – |
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 |
|---|---|---|---|---|
| Li2CO3 (cr) | -1215.9[1] | -1132.06[1] | 90.37[1] | 99.12[1] |
| Li2CO3 (ai) | -1234.11[1] | -1114.6[1] | -29.7[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 |
|---|---|---|---|---|
| Li2O (cr) | -597.94[1] | -561.18[1] | 37.57[1] | 54.10[1] |
| Li2O (g) | -160.7[1] | -181.6[1] | 231.48[1] | 49.83[1] |
| CO2 (g) | -393.509[1] | -394.359[1] | 213.74[1] | 37.11[1] |
| CO2 (ao) | -413.80[1] | -385.98[1] | 117.6[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°, -1215.9 kJ · mol−1
- ^ ΔfG°, -1132.06 kJ · mol−1
- ^ S°, 90.37 J · K−1 · mol−1
- ^ Cp°, 99.12 J · K−1 · mol−1
- ^ ΔfH°, -1234.11 kJ · mol−1
- ^ ΔfG°, -1114.6 kJ · mol−1
- ^ S°, -29.7 J · K−1 · mol−1
- ^ ΔfH°, -597.94 kJ · mol−1
- ^ ΔfG°, -561.18 kJ · mol−1
- ^ S°, 37.57 J · K−1 · mol−1
- ^ Cp°, 54.10 J · K−1 · mol−1
- ^ ΔfH°, -160.7 kJ · mol−1
- ^ ΔfG°, -181.6 kJ · mol−1
- ^ S°, 231.48 J · K−1 · mol−1
- ^ Cp°, 49.83 J · K−1 · mol−1
- ^ ΔfH°, -393.509 kJ · mol−1
- ^ ΔfG°, -394.359 kJ · mol−1
- ^ S°, 213.74 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -413.80 kJ · mol−1
- ^ ΔfG°, -385.98 kJ · mol−1
- ^ S°, 117.6 J · K−1 · mol−1