BaI2 + MgSO4 💧→ BaSO4↓ + MgI2
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The reaction of barium iodide and magnesium sulfate yields barium sulfate and magnesium iodide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of barium iodide and magnesium sulfate
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 barium iodide and magnesium sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaI2 | Barium iodide | 1 | Lewis acid | Very soluble in water |
| MgSO4 | Magnesium sulfate | 1 | Lewis base | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaSO4 | Barium sulfate | 1 | Lewis conjugate | Insoluble in water |
| MgI2 | Magnesium iodide | 1 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of barium iodide and magnesium sulfate
| 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 | 49.8 | – | – | – |
per 1 mol of | 49.8 | – | – | – |
per 1 mol of | 49.8 | – | – | – |
per 1 mol of | 49.8 | – | – | – |
per 1 mol of | 49.8 | – | – | – |
Changes in standard condition (2)
- Reaction of barium iodide and magnesium sulfate
| 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 | 56.5 | – | – | – |
per 1 mol of | 56.5 | – | – | – |
per 1 mol of | 56.5 | – | – | – |
per 1 mol of | 56.5 | – | – | – |
per 1 mol of | 56.5 | – | – | – |
Changes in aqueous solution (1)
- Reaction of barium iodide and magnesium sulfate◆
ΔrG 0.0 kJ/mol K 1.00 × 100 pK 0.00
| 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 | 1302.23 | 0.0 | 0.0 | – |
per 1 mol of | 1302.23 | 0.0 | 0.0 | – |
per 1 mol of | 1302.23 | 0.0 | 0.0 | – |
per 1 mol of | 1302.23 | 0.0 | 0.0 | – |
per 1 mol of | 1302.23 | 0.0 | 0.0 | – |
Changes in aqueous solution (2)
- Reaction of barium iodide and magnesium sulfate◆
ΔrG 12.7 kJ/mol K 0.60 × 10−2 pK 2.22
| 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 | 1282.1 | 12.7 | −110.9 | – |
per 1 mol of | 1282.1 | 12.7 | −110.9 | – |
per 1 mol of | 1282.1 | 12.7 | −110.9 | – |
per 1 mol of | 1282.1 | 12.7 | −110.9 | – |
per 1 mol of | 1282.1 | 12.7 | −110.9 | – |
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 |
|---|---|---|---|---|
| BaI2 (cr) | -602.1[1] | – | – | – |
| BaI2 (g) | -326[1] | -377[1] | 343[1] | 61.5[1] |
| BaI2 (ai) | -648.02[1] | -663.92[1] | 232.2[1] | – |
| BaI2 (cr) 1 hydrate | -919.2[1] | – | – | – |
| BaI2 (cr) 2 hydrate | -1216.7[1] | – | – | – |
| BaI2 (cr) 2.5 hydrate | -1363.6[1] | – | – | – |
| BaI2 (cr) 7 hydrate | -2676.5[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] | – |
* (cr):Crystalline solid, (g):Gas, (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 |
|---|---|---|---|---|
| BaSO4 (cr) | -1473.2[1] | -1362.2[1] | 132.2[1] | 101.75[1] |
| BaSO4 (cr) precipitated | -1466.5[1] | – | – | – |
| BaSO4 (ai) | -144.691[1] | -1305.30[1] | 29.7[1] | – |
| MgI2 (cr) | -364.0[1] | -358.2[1] | 129.7[1] | – |
| MgI2 (g) | -172[1] | – | – | – |
| MgI2 (ai) | -577.22[1] | -558.1[1] | 84.5[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas
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°, -602.1 kJ · mol−1
- ^ ΔfH°, -326. kJ · mol−1
- ^ ΔfG°, -377. kJ · mol−1
- ^ S°, 343. J · K−1 · mol−1
- ^ Cp°, 61.5 J · K−1 · mol−1
- ^ ΔfH°, -648.02 kJ · mol−1
- ^ ΔfG°, -663.92 kJ · mol−1
- ^ S°, 232.2 J · K−1 · mol−1
- ^ ΔfH°, -919.2 kJ · mol−1
- ^ ΔfH°, -1216.7 kJ · mol−1
- ^ ΔfH°, -1363.6 kJ · mol−1
- ^ ΔfH°, -2676.5 kJ · mol−1
- ^ 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°, -1473.2 kJ · mol−1
- ^ ΔfG°, -1362.2 kJ · mol−1
- ^ S°, 132.2 J · K−1 · mol−1
- ^ Cp°, 101.75 J · K−1 · mol−1
- ^ ΔfH°, -1466.5 kJ · mol−1
- ^ ΔfH°, -144.691 kJ · mol−1
- ^ ΔfG°, -1305.30 kJ · mol−1
- ^ S°, 29.7 J · K−1 · mol−1
- ^ ΔfH°, -364.0 kJ · mol−1
- ^ ΔfG°, -358.2 kJ · mol−1
- ^ S°, 129.7 J · K−1 · mol−1
- ^ ΔfH°, -172. kJ · mol−1
- ^ ΔfH°, -577.22 kJ · mol−1
- ^ ΔfG°, -558.1 kJ · mol−1
- ^ S°, 84.5 J · K−1 · mol−1