Hg2Cl2 + Cl2 → 2HgCl2
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- Reaction of mercury(I) chloride and
The reaction of mercury(I) chloride and yields mercury(II) chloride. This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of mercury(I) chloride and
General equation
- Reaction of oxidizable species and oxidizing species
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of mercury(I) chloride and
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Hg2Cl2 | Mercury(I) chloride | 1 | Reducing | Oxidizable |
| 1 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgCl2 | Mercury(II) chloride | 2 | Redoxed product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of mercury(I) chloride and ◆
ΔrG −146.5 kJ/mol K 4.63 × 1025 pK −25.67
| 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 | −183.4 | −146.5 | −123.6 | – |
per 1 mol of | −183.4 | −146.5 | −123.6 | – |
| −183.4 | −146.5 | −123.6 | – | |
per 1 mol of | −91.70 | −73.25 | −61.80 | – |
Changes in aqueous solution
- Reaction of mercury(I) chloride and ◆
ΔrG −142.6 kJ/mol K 9.60 × 1024 pK −24.98
| 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 | −144.0 | −142.6 | −4 | – |
per 1 mol of | −144.0 | −142.6 | −4 | – |
| −144.0 | −142.6 | −4 | – | |
per 1 mol of | −72.00 | −71.30 | −2 | – |
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 |
|---|---|---|---|---|
| Hg2Cl2 (cr) | -265.22[1] | -210.745[1] | 192.5[1] | – |
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[1] | – |
* (cr):Crystalline solid, (g):Gas, (ao):Un-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 |
|---|---|---|---|---|
| HgCl2 (cr) | -224.3[1] | -178.6[1] | 146.0[1] | – |
| HgCl2 (ao) | -216.3[1] | -173.2[1] | 155[1] | – |
* (cr):Crystalline solid, (ao):Un-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°, -265.22 kJ · mol−1
- ^ ΔfG°, -210.745 kJ · mol−1
- ^ S°, 192.5 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ 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