Mg(HCO3)2 + (NH4)2SO3 💧→ MgCO3↓ + (NH4)2CO3 + H2SO3
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The reaction of magnesium hydrogencarbonate and ammonium sulfite yields magnesium carbonate, ammonium carbonate, and sulfurous acid (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of magnesium hydrogencarbonate and ammonium sulfite
General equation
- Precipitation reaction
- Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base💧⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)
Oxidation state of each atom
- Reaction of magnesium hydrogencarbonate and ammonium sulfite
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mg(HCO3)2 | Magnesium hydrogencarbonate | 1 | Lewis acid | Soluble in water |
| (NH4)2SO3 | Ammonium sulfite | 1 | Lewis base | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgCO3 | Magnesium carbonate | 1 | Lewis conjugate | Very slightly soluble in water |
| (NH4)2CO3 | Ammonium carbonate | 1 | Non-redox product | – |
| H2SO3 | Sulfurous acid | 1 | Non-redox product | – |
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 |
|---|---|---|---|---|
| Mg(HCO3)2 | – | – | – | – |
| (NH4)2SO3 (cr) | -885.3[1] | – | – | – |
| (NH4)2SO3 (ai) | -900.4[1] | -645.0[1] | 197.5[1] | – |
| (NH4)2SO3 (cr) 1 hydrate | -1187.4[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 |
|---|---|---|---|---|
| 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] | – | – |
| (NH4)2CO3 (ai) | -942.15[1] | -686.42[1] | 169.9[1] | – |
| H2SO3 (ao) | -608.81[1] | -537.81[1] | 232.2[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, -885.3 kJ · mol−1
- ^ ΔfH°, -900.4 kJ · mol−1
- ^ ΔfG°, -645.0 kJ · mol−1
- ^ S°, 197.5 J · K−1 · mol−1
- ^ ΔfH°, -1187.4 kJ · mol−1
- ^ 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°, -942.15 kJ · mol−1
- ^ ΔfG°, -686.42 kJ · mol−1
- ^ S°, 169.9 J · K−1 · mol−1
- ^ ΔfH°, -608.81 kJ · mol−1
- ^ ΔfG°, -537.81 kJ · mol−1
- ^ S°, 232.2 J · K−1 · mol−1