Rb2O + CO2 → Rb2CO3
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The reaction of rubidium oxide and carbon dioxide yields rubidium carbonate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of rubidium 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 rubidium oxide and carbon dioxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Rb2O | Rubidium 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 |
---|---|---|---|---|
Rb2CO3 | Rubidium carbonate | 1 | Lewis conjugate | Oxoacid salt Salt of weak acid and strong base |
Thermodynamic changes
Changes in standard condition
- Reaction of rubidium oxide and carbon dioxide
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 | −403 | – | – | – |
per 1 mol of | −403 | – | – | – |
per 1 mol of | −403 | – | – | – |
per 1 mol of | −403 | – | – | – |
Changes in aqueous solution
- Reaction of rubidium oxide and carbon dioxide
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 | −427 | – | – | – |
per 1 mol of | −427 | – | – | – |
per 1 mol of | −427 | – | – | – |
per 1 mol of | −427 | – | – | – |
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 |
---|---|---|---|---|
Rb2O (cr) | -339[1] | – | – | – |
Rb2O (g) | -50[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 |
---|---|---|---|---|
Rb2CO3 (cr) | -1136.0[1] | -1051.0[1] | 181.33[1] | 117.61[1] |
Rb2CO3 (ai) | -1179.47[1] | -1095.78[1] | 186.2[1] | – |
Rb2CO3 (cr) 1 hydrate | -1448.5[1] | – | – | – |
Rb2CO3 (cr) 1.5 hydrate | -1604.5[1] | – | – | – |
Rb2CO3 (cr) 3 hydrate | -2048.1[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°, -339. kJ · mol−1
- ^ ΔfH°, -50. 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°, -1136.0 kJ · mol−1
- ^ ΔfG°, -1051.0 kJ · mol−1
- ^ S°, 181.33 J · K−1 · mol−1
- ^ Cp°, 117.61 J · K−1 · mol−1
- ^ ΔfH°, -1179.47 kJ · mol−1
- ^ ΔfG°, -1095.78 kJ · mol−1
- ^ S°, 186.2 J · K−1 · mol−1
- ^ ΔfH°, -1448.5 kJ · mol−1
- ^ ΔfH°, -1604.5 kJ · mol−1
- ^ ΔfH°, -2048.1 kJ · mol−1