K2O + CO2 → K2CO3
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The reaction of potassium oxide and carbon dioxide yields potassium carbonate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of potassium oxide and carbon dioxide
General equation
- Reaction of basic oxide and acidic oxide
- Basic oxideLewis base + Acidic oxideLewis acid ⟶ Oxoacid saltLewis conjugate
- Reaction of strongly basic oxide and weakly acidic oxide
- Strongly basic oxideLewis base + Weakly acidic oxideLewis acid ⟶ Salt of weak acid and strong baseLewis conjugate
Oxidation state of each atom
- Reaction of potassium oxide and carbon dioxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2O | Potassium oxide | 1 | Lewis base | Basic oxide Strongly basic oxide |
| CO2 | Carbon dioxide | 1 | Lewis acid | Acidic oxide Weakly acidic oxide |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2CO3 | Potassium carbonate | 1 | Lewis conjugate | Oxoacid salt Salt of weak acid and strong base |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium oxide and carbon dioxide◆
ΔrG −347.0 kJ/mol K 6.19 × 1060 pK −60.79
| 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 | −396.0 | −347.0 | −152.3 | −6.4 |
per 1 mol of | −396.0 | −347.0 | −152.3 | −6.4 |
per 1 mol of | −396.0 | −347.0 | −152.3 | −6.4 |
per 1 mol of | −396.0 | −347.0 | −152.3 | −6.4 |
Changes in aqueous solution
- Reaction of potassium oxide and carbon dioxide◆
ΔrG −386.3 kJ/mol K 4.75 × 1067 pK −67.68
| 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 | −406.6 | −386.3 | −63.6 | – |
per 1 mol of | −406.6 | −386.3 | −63.6 | – |
per 1 mol of | −406.6 | −386.3 | −63.6 | – |
per 1 mol of | −406.6 | −386.3 | −63.6 | – |
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 |
|---|---|---|---|---|
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[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
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 |
|---|---|---|---|---|
| K2CO3 (cr) | -1151.02[1] | -1063.5[1] | 155.52[1] | 114.43[1] |
| K2CO3 (ai) | -1181.90[1] | -1094.36[1] | 148.1[1] | – |
| K2CO3 (cr) 1.5 hydrate | -1609.2[1] | -1432.5[1] | 203.3[1] | – |
* (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°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · 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
- ^ ΔfH°, -1151.02 kJ · mol−1
- ^ ΔfG°, -1063.5 kJ · mol−1
- ^ S°, 155.52 J · K−1 · mol−1
- ^ Cp°, 114.43 J · K−1 · mol−1
- ^ ΔfH°, -1181.90 kJ · mol−1
- ^ ΔfG°, -1094.36 kJ · mol−1
- ^ S°, 148.1 J · K−1 · mol−1
- ^ ΔfH°, -1609.2 kJ · mol−1
- ^ ΔfG°, -1432.5 kJ · mol−1
- ^ S°, 203.3 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