MgSO4 + (NH4)2CO3 💧→ MgCO3↓ + (NH4)2SO4
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The reaction of magnesium sulfate and ammonium carbonate yields magnesium carbonate and ammonium sulfate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of magnesium sulfate and ammonium carbonate
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 sulfate and ammonium carbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgSO4 | Magnesium sulfate | 1 | Lewis acid | Very soluble in water |
| (NH4)2CO3 | Ammonium carbonate | 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)2SO4 | Ammonium sulfate | 1 | Non-redox product | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of magnesium sulfate and ammonium carbonate◆
ΔrG −29.3 kJ/mol K 1.36 × 105 pK −5.13
| 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 | −29.3 | 260.7 | – |
per 1 mol of | 48.2 | −29.3 | 260.7 | – |
per 1 mol of | 48.2 | −29.3 | 260.7 | – |
per 1 mol of | 48.2 | −29.3 | 260.7 | – |
per 1 mol of | 48.2 | −29.3 | 260.7 | – |
Changes in aqueous solution (2)
- Reaction of magnesium sulfate and ammonium carbonate◆
ΔrG −16.6 kJ/mol K 8.09 × 102 pK −2.91
| 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 | 28.1 | −16.6 | 149.8 | – |
per 1 mol of | 28.1 | −16.6 | 149.8 | – |
per 1 mol of | 28.1 | −16.6 | 149.8 | – |
per 1 mol of | 28.1 | −16.6 | 149.8 | – |
per 1 mol of | 28.1 | −16.6 | 149.8 | – |
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 |
|---|---|---|---|---|
| MgSO4 (cr) | -1284.9[1] | -1170.6[1] | 91.6[1] | 96.48[1] |
| MgSO4 (ai) | -1376.12[1] | -1199.5[1] | -118.0[1] | – |
| MgSO4 (ao) | -1356.0[1] | -1212.21[1] | -7.1[1] | – |
| MgSO4 (cr) 1 hydrate | -1602.1[1] | -1428.7[1] | 126.4[1] | – |
| MgSO4 (am) 1 hydrate | -1574.9[1] | -1404.9[1] | 138.1[1] | – |
| MgSO4 (cr) 2 hydrate | -1896.2[1] | – | – | – |
| MgSO4 (cr) 4 hydrate | -2496.6[1] | – | – | – |
| MgSO4 (cr) 6 hydrate | -3087.0[1] | -2631.8[1] | 348.1[1] | 348.11[1] |
| MgSO4 (cr) 7 hydrate | -3388.71[1] | -2871.5[1] | 372[1] | – |
| (NH4)2CO3 (ai) | -942.15[1] | -686.42[1] | 169.9[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (am):Amorphous 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 |
|---|---|---|---|---|
| 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)2SO4 (cr) | -1180.85[1] | -901.67[1] | 220.1[1] | 187.49[1] |
| (NH4)2SO4 (ai) | -1174.28[1] | -903.14[1] | 246.9[1] | -133.1[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°, -1284.9 kJ · mol−1
- ^ ΔfG°, -1170.6 kJ · mol−1
- ^ S°, 91.6 J · K−1 · mol−1
- ^ Cp°, 96.48 J · K−1 · mol−1
- ^ ΔfH°, -1376.12 kJ · mol−1
- ^ ΔfG°, -1199.5 kJ · mol−1
- ^ S°, -118.0 J · K−1 · mol−1
- ^ ΔfH°, -1356.0 kJ · mol−1
- ^ ΔfG°, -1212.21 kJ · mol−1
- ^ S°, -7.1 J · K−1 · mol−1
- ^ ΔfH°, -1602.1 kJ · mol−1
- ^ ΔfG°, -1428.7 kJ · mol−1
- ^ S°, 126.4 J · K−1 · mol−1
- ^ ΔfH°, -1574.9 kJ · mol−1
- ^ ΔfG°, -1404.9 kJ · mol−1
- ^ S°, 138.1 J · K−1 · mol−1
- ^ ΔfH°, -1896.2 kJ · mol−1
- ^ ΔfH°, -2496.6 kJ · mol−1
- ^ ΔfH°, -3087.0 kJ · mol−1
- ^ ΔfG°, -2631.8 kJ · mol−1
- ^ S°, 348.1 J · K−1 · mol−1
- ^ Cp°, 348.11 J · K−1 · mol−1
- ^ ΔfH°, -3388.71 kJ · mol−1
- ^ ΔfG°, -2871.5 kJ · mol−1
- ^ S°, 372. J · K−1 · mol−1
- ^ ΔfH°, -942.15 kJ · mol−1
- ^ ΔfG°, -686.42 kJ · mol−1
- ^ S°, 169.9 J · K−1 · 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°, -1180.85 kJ · mol−1
- ^ ΔfG°, -901.67 kJ · mol−1
- ^ S°, 220.1 J · K−1 · mol−1
- ^ Cp°, 187.49 J · K−1 · mol−1
- ^ ΔfH°, -1174.28 kJ · mol−1
- ^ ΔfG°, -903.14 kJ · mol−1
- ^ S°, 246.9 J · K−1 · mol−1
- ^ Cp°, -133.1 J · K−1 · mol−1