3HgCl2 + 2FeI3 💧→ 3HgI2↓ + 2FeCl3
Last updated:
The reaction of mercury(II) chloride and iron(III) iodide yields mercury(II) iodide and iron(III) chloride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of mercury(II) chloride and iron(III) iodide
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 mercury(II) chloride and iron(III) iodide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgCl2 | Mercury(II) chloride | 3 | Lewis acid | Soluble in water |
| FeI3 | Iron(III) iodide | 2 | Lewis base | Soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgI2 | Mercury(II) iodide | 3 | Lewis conjugate | Very slightly soluble in water |
| FeCl3 | Iron(III) chloride | 2 | Non-redox product | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of mercury(II) chloride and iron(III) iodide◆
ΔrG −196.5 kJ/mol K 2.66 × 1034 pK −34.43
| 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 | – | −196.5 | – | – |
per 1 mol of | – | −65.50 | – | – |
per 1 mol of | – | −98.25 | – | – |
per 1 mol of | – | −65.50 | – | – |
per 1 mol of | – | −98.25 | – | – |
Changes in aqueous solution (2)
- Reaction of mercury(II) chloride and iron(III) iodide◆
ΔrG −184.1 kJ/mol K 1.79 × 1032 pK −32.25
| 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 | −261.6 | −184.1 | −266 | – |
per 1 mol of | −87.20 | −61.37 | −88.7 | – |
per 1 mol of | −130.8 | −92.05 | −133 | – |
per 1 mol of | −87.20 | −61.37 | −88.7 | – |
per 1 mol of | −130.8 | −92.05 | −133 | – |
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 |
|---|---|---|---|---|
| HgCl2 (cr) | -224.3[1] | -178.6[1] | 146.0[1] | – |
| HgCl2 (ao) | -216.3[1] | -173.2[1] | 155[1] | – |
| FeI3 (g) | 71[1] | – | – | – |
| FeI3 (ai) | -214.2[1] | -159.4[1] | 18.0[1] | – |
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (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 |
|---|---|---|---|---|
| HgI2 (cr) red | -105.4[1] | -101.7[1] | 180[1] | – |
| HgI2 (cr) yellow | -102.9[1] | – | – | – |
| HgI2 (g) | -17.2[1] | -59.9[1] | 336.13[1] | 61.09[1] |
| HgI2 (ao) | -79.5[1] | -75.3[1] | 176[1] | – |
| FeCl3 (cr) | -399.49[1] | -334.00[1] | 142.3[1] | 96.65[1] |
| FeCl3 (g) | -254.0[1] | – | – | – |
| FeCl3 (ai) | -550.2[1] | -398.3[1] | -146.4[1] | – |
| FeCl3 (ao) | – | -404.5[1] | – | – |
| FeCl3 (cr) 6 hydrate | -2223.8[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (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°, -224.3 kJ · mol−1
- ^ ΔfG°, -178.6 kJ · mol−1
- ^ S°, 146.0 J · K−1 · mol−1
- ^ ΔfH°, -216.3 kJ · mol−1
- ^ ΔfG°, -173.2 kJ · mol−1
- ^ S°, 155. J · K−1 · mol−1
- ^ ΔfH°, 71. kJ · mol−1
- ^ ΔfH°, -214.2 kJ · mol−1
- ^ ΔfG°, -159.4 kJ · mol−1
- ^ S°, 18.0 J · K−1 · mol−1
- ^ ΔfH°, -105.4 kJ · mol−1
- ^ ΔfG°, -101.7 kJ · mol−1
- ^ S°, 180. J · K−1 · mol−1
- ^ ΔfH°, -102.9 kJ · mol−1
- ^ ΔfH°, -17.2 kJ · mol−1
- ^ ΔfG°, -59.9 kJ · mol−1
- ^ S°, 336.13 J · K−1 · mol−1
- ^ Cp°, 61.09 J · K−1 · mol−1
- ^ ΔfH°, -79.5 kJ · mol−1
- ^ ΔfG°, -75.3 kJ · mol−1
- ^ S°, 176. J · K−1 · mol−1
- ^ ΔfH°, -399.49 kJ · mol−1
- ^ ΔfG°, -334.00 kJ · mol−1
- ^ S°, 142.3 J · K−1 · mol−1
- ^ Cp°, 96.65 J · K−1 · mol−1
- ^ ΔfH°, -254.0 kJ · mol−1
- ^ ΔfH°, -550.2 kJ · mol−1
- ^ ΔfG°, -398.3 kJ · mol−1
- ^ S°, -146.4 J · K−1 · mol−1
- ^ ΔfG°, -404.5 kJ · mol−1
- ^ ΔfH°, -2223.8 kJ · mol−1