MgCO3 → Mg2+ + CO32−
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- Electrolytic dissociation of magnesium carbonate
Electrolytic dissociation of magnesium carbonate yields magnesium ion and carbonate ion. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolytic dissociation of magnesium carbonate
General equation
- Electrolytic dissociation of salt
- SaltLewis conjugate ⟶ CationLewis acid + AnionLewis base
Oxidation state of each atom
- Electrolytic dissociation of magnesium carbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgCO3 | Magnesium carbonate | 1 | Lewis conjugate | Salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mg2+ | Magnesium ion | 1 | Lewis acid | Cation |
| CO32− | Carbonate ion | 1 | Lewis base | Anion |
Thermodynamic changes
Changes in standard condition
- Electrolytic dissociation of magnesium carbonate◆
ΔrG 29.5 kJ/mol K 0.68 × 10−5 pK 5.17
| 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 | −48.2 | 29.5 | −260.7 | – |
per 1 mol of | −48.2 | 29.5 | −260.7 | – |
per 1 mol of Magnesium ion | −48.2 | 29.5 | −260.7 | – |
per 1 mol of Carbonate ion | −48.2 | 29.5 | −260.7 | – |
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 |
|---|---|---|---|---|
| MgCO3 (cr) | -1095.8[1] | -1012.1[1] | 65.7[1] | 75.52[1] |
| MgCO3 (cr) 3 hydrate | – | -1726.1[1] | – | – |
| MgCO3 (cr) 5 hydrate | – | -2199.2[1] | – | – |
* (cr):Crystalline solid
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 |
|---|---|---|---|---|
| Mg2+ (g) | 2348.504[1] | – | – | – |
| Mg2+ (ao) | -466.85[1] | -454.8[1] | -138.1[1] | – |
| CO32− (ao) | -677.14[1] | -527.81[1] | -56.9[1] | – |
* (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°, -1095.8 kJ · mol−1
- ^ ΔfG°, -1012.1 kJ · mol−1
- ^ S°, 65.7 J · K−1 · mol−1
- ^ Cp°, 75.52 J · K−1 · mol−1
- ^ ΔfG°, -1726.1 kJ · mol−1
- ^ ΔfG°, -2199.2 kJ · mol−1
- ^ ΔfH°, 2348.504 kJ · mol−1
- ^ ΔfH°, -466.85 kJ · mol−1
- ^ ΔfG°, -454.8 kJ · mol−1
- ^ S°, -138.1 J · K−1 · mol−1
- ^ ΔfH°, -677.14 kJ · mol−1
- ^ ΔfG°, -527.81 kJ · mol−1
- ^ S°, -56.9 J · K−1 · mol−1