BaI2 + K2CO3 💧→ BaCO3↓ + 2KI
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The reaction of barium iodide and potassium carbonate yields barium carbonate and potassium 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 potassium 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 barium iodide and potassium carbonate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
BaI2 | Barium iodide | 1 | Lewis acid | Very soluble in water |
K2CO3 | Potassium carbonate | 1 | Lewis base | Very soluble in water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
BaCO3 | Barium carbonate | 1 | Lewis conjugate | Insoluble in water |
KI | Potassium iodide | 2 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of barium iodide and potassium carbonate
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 | −119.0 | – | – | – |
per 1 mol of | −119.0 | – | – | – |
per 1 mol of | −119.0 | – | – | – |
per 1 mol of | −119.0 | – | – | – |
per 1 mol of | −59.50 | – | – | – |
Changes in aqueous solution
- Reaction of barium iodide and potassium carbonate◆
ΔrG −49.0 kJ/mol K 3.84 × 108 pK −8.58
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 | −1.5 | −49.0 | 159.4 | – |
per 1 mol of | −1.5 | −49.0 | 159.4 | – |
per 1 mol of | −1.5 | −49.0 | 159.4 | – |
per 1 mol of | −1.5 | −49.0 | 159.4 | – |
per 1 mol of | −0.75 | −24.5 | 79.70 | – |
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] | – | – | – |
K2CO3 (cr) | -1151.02[1] | -1063.5[1] | 155.52[1] | 114.43[1] |
K2CO3 (ai) | -1181.90[1] | -1094.36[1] | 148.1[1] | – |
K2CO3 (cr) 1.5 hydrate | -1609.2[1] | -1432.5[1] | 203.3[1] | – |
* (cr):Crystalline solid, (g):Gas, (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 |
---|---|---|---|---|
BaCO3 (cr) | -1216.3[1] | -1137.6[1] | 112.1[1] | 85.35[1] |
BaCO3 (ai) | -1214.78[1] | -1088.59[1] | -47.3[1] | – |
KI (cr) | -327.900[1] | -324.892[1] | 106.32[1] | 52.93[1] |
KI (g) | -125.5[1] | -166.1[1] | 258.3[1] | 37.11[1] |
KI (ai) | -307.57[1] | -334.85[1] | 213.8[1] | -120.5[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°, -1151.02 kJ · mol−1
- ^ ΔfG°, -1063.5 kJ · mol−1
- ^ S°, 155.52 J · K−1 · mol−1
- ^ Cp°, 114.43 J · K−1 · mol−1
- ^ ΔfH°, -1181.90 kJ · mol−1
- ^ ΔfG°, -1094.36 kJ · mol−1
- ^ S°, 148.1 J · K−1 · mol−1
- ^ ΔfH°, -1609.2 kJ · mol−1
- ^ ΔfG°, -1432.5 kJ · mol−1
- ^ S°, 203.3 J · K−1 · mol−1
- ^ ΔfH°, -1216.3 kJ · mol−1
- ^ ΔfG°, -1137.6 kJ · mol−1
- ^ S°, 112.1 J · K−1 · mol−1
- ^ Cp°, 85.35 J · K−1 · mol−1
- ^ ΔfH°, -1214.78 kJ · mol−1
- ^ ΔfG°, -1088.59 kJ · mol−1
- ^ S°, -47.3 J · K−1 · mol−1
- ^ ΔfH°, -327.900 kJ · mol−1
- ^ ΔfG°, -324.892 kJ · mol−1
- ^ S°, 106.32 J · K−1 · mol−1
- ^ Cp°, 52.93 J · K−1 · mol−1
- ^ ΔfH°, -125.5 kJ · mol−1
- ^ ΔfG°, -166.1 kJ · mol−1
- ^ S°, 258.3 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -307.57 kJ · mol−1
- ^ ΔfG°, -334.85 kJ · mol−1
- ^ S°, 213.8 J · K−1 · mol−1
- ^ Cp°, -120.5 J · K−1 · mol−1