2AlI3 + 3Ca(OH)2 → 3CaI2 + 2Al(OH)3
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The reaction of aluminium iodide and calcium hydroxide yields calcium iodide and aluminium hydroxide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of aluminium iodide and calcium hydroxide
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
Oxidation state of each atom
- Reaction of aluminium iodide and calcium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| AlI3 | Aluminium iodide | 2 | Brønsted acid | Salt of weak base |
| Ca(OH)2 | Calcium hydroxide | 3 | Brønsted base | Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CaI2 | Calcium iodide | 3 | Conjugate acid | Salt of strong base |
| Al(OH)3 | Aluminium hydroxide | 2 | Conjugate base | Weak base |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of aluminium iodide and calcium hydroxide◆
ΔrG −902 kJ/mol K 1.06 × 10158 pK −158.02
| 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 | −583 | −902 | 0 | – |
per 1 mol of | −292 | −451 | 0 | – |
per 1 mol of | −194 | −301 | 0 | – |
per 1 mol of | −194 | −301 | 0 | – |
per 1 mol of | −292 | −451 | 0 | – |
Changes in standard condition (2)
- Reaction of aluminium iodide and calcium hydroxide
| 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 | −567 | – | – | – |
per 1 mol of | −284 | – | – | – |
per 1 mol of | −189 | – | – | – |
per 1 mol of | −189 | – | – | – |
per 1 mol of | −284 | – | – | – |
Changes in aqueous solution (1)
- Reaction of aluminium iodide and calcium hydroxide◆
ΔrG −607 kJ/mol K 2.20 × 10106 pK −106.34
| 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 | −171 | −607 | 376 | – |
per 1 mol of | −85.5 | −304 | 188 | – |
per 1 mol of | −57.0 | −202 | 125 | – |
per 1 mol of | −57.0 | −202 | 125 | – |
per 1 mol of | −85.5 | −304 | 188 | – |
Changes in aqueous solution (2)
- Reaction of aluminium iodide and calcium hydroxide
| 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 | −182 | – | – | – |
per 1 mol of | −91.0 | – | – | – |
per 1 mol of | −60.7 | – | – | – |
per 1 mol of | −60.7 | – | – | – |
per 1 mol of | −91.0 | – | – | – |
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 |
|---|---|---|---|---|
| AlI3 (cr) | -313.8[1] | -300.8[1] | 159[1] | 98.7[1] |
| AlI3 (g) | -207.5[1] | – | – | – |
| AlI3 (ai) | -699[1] | -640[1] | 12.1[1] | – |
| AlI3 (aq) | -693.7[1] | – | – | – |
| Ca(OH)2 (cr) | -986.09[1] | -898.49[1] | 83.39[1] | 87.49[1] |
| Ca(OH)2 (g) | -544[1] | – | – | – |
| Ca(OH)2 (ai) | -1002.82[1] | -868.07[1] | -74.5[1] | – |
| Ca(OH)2 (cr) 2 hydrate | -1218.4[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (aq):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 |
|---|---|---|---|---|
| CaI2 (cr) | -533.5[1] | -528.9[1] | 142[1] | – |
| CaI2 (g) | -272[1] | – | – | – |
| CaI2 (ai) | -653.21[1] | -656.72[1] | 169.5[1] | – |
| CaI2 (cr) 8 hydrate | -2929.6[1] | – | – | – |
| Al(OH)3 (cr) | -1284[2] | -1306[2] | 71[2] | 93.1[2] |
| Al(OH)3 (am) | -1276[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (am):Amorphous solid
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°, -313.8 kJ · mol−1
- ^ ΔfG°, -300.8 kJ · mol−1
- ^ S°, 159. J · K−1 · mol−1
- ^ Cp°, 98.7 J · K−1 · mol−1
- ^ ΔfH°, -207.5 kJ · mol−1
- ^ ΔfH°, -699. kJ · mol−1
- ^ ΔfG°, -640. kJ · mol−1
- ^ S°, 12.1 J · K−1 · mol−1
- ^ ΔfH°, -693.7 kJ · mol−1
- ^ ΔfH°, -986.09 kJ · mol−1
- ^ ΔfG°, -898.49 kJ · mol−1
- ^ S°, 83.39 J · K−1 · mol−1
- ^ Cp°, 87.49 J · K−1 · mol−1
- ^ ΔfH°, -544. kJ · mol−1
- ^ ΔfH°, -1002.82 kJ · mol−1
- ^ ΔfG°, -868.07 kJ · mol−1
- ^ S°, -74.5 J · K−1 · mol−1
- ^ ΔfH°, -1218.4 kJ · mol−1
- ^ ΔfH°, -533.5 kJ · mol−1
- ^ ΔfG°, -528.9 kJ · mol−1
- ^ S°, 142. J · K−1 · mol−1
- ^ ΔfH°, -272. kJ · mol−1
- ^ ΔfH°, -653.21 kJ · mol−1
- ^ ΔfG°, -656.72 kJ · mol−1
- ^ S°, 169.5 J · K−1 · mol−1
- ^ ΔfH°, -2929.6 kJ · mol−1
- ^ ΔfH°, -1276. kJ · mol−1
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfH°, -1284 kJ · mol−1 - p.254
- ^ ΔfG°, -1306 kJ · mol−1 - p.254
- ^ S°, 71 J · K−1 · mol−1 - p.254
- ^ Cp°, 93.1 J · K−1 · mol−1 - p.254