HgBr2 + 6Cl2 + 6H2O 🔥→ HgCl2 + 2HBrO3 + 10HCl
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- Reaction of mercury(II) bromide and under neutral condition
The reaction of mercury(II) bromide, , and water yields mercury(II) chloride, bromic acid, and hydrogen chloride (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of mercury(II) bromide and under neutral condition
General equation
- Reaction of hardly oxidizable species and oxidizing species under neutral condition
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of mercury(II) bromide and under neutral condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgBr2 | Mercury(II) bromide | 1 | Reducing | Hardly oxidizable |
| 6 | Oxidizing | Oxidizing | ||
| H2O | Water | 6 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgCl2 | Mercury(II) chloride | 1 | Reduced | – |
| HBrO3 | Bromic acid | 2 | Oxidized | – |
| HCl | Hydrogen chloride | 10 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of mercury(II) bromide and under neutral condition◆
ΔrG 435.2 kJ/mol K 0.57 × 10−76 pK 76.24
| 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 | 742.6 | 435.2 | 1030 | – |
per 1 mol of | 742.6 | 435.2 | 1030 | – |
| 123.8 | 72.53 | 171.7 | – | |
per 1 mol of | 123.8 | 72.53 | 171.7 | – |
per 1 mol of | 742.6 | 435.2 | 1030 | – |
per 1 mol of | 371.3 | 217.6 | 515.0 | – |
per 1 mol of | 74.26 | 43.52 | 103.0 | – |
Changes in standard condition (2)
- Reaction of mercury(II) bromide and under neutral condition◆
ΔrG 76.0 kJ/mol K 0.48 × 10−13 pK 13.31
| 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 | −6.0 | 76.0 | −274 | – |
per 1 mol of | −6.0 | 76.0 | −274 | – |
| −1.0 | 12.7 | −45.7 | – | |
per 1 mol of | −1.0 | 12.7 | −45.7 | – |
per 1 mol of | −6.0 | 76.0 | −274 | – |
per 1 mol of | −3.0 | 38.0 | −137 | – |
per 1 mol of | −0.60 | 7.60 | −27.4 | – |
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 |
|---|---|---|---|---|
| HgBr2 (cr) | -170.7[1] | -153.1[1] | 172[1] | – |
| HgBr2 (ao) | -160.7[1] | -143.1[1] | 172[1] | – |
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[1] | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (g):Gas, (l):Liquid
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] | – |
| HBrO3 (ai) | -67.07[1] | 18.60[1] | 161.71[1] | – |
| HCl (g) | -92.307[1] | -95.299[1] | 186.908[1] | 29.12[1] |
| HCl (ai) | -167.159[1] | -131.228[1] | 56.5[1] | -136.4[1] |
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (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°, -170.7 kJ · mol−1
- ^ ΔfG°, -153.1 kJ · mol−1
- ^ S°, 172. J · K−1 · mol−1
- ^ ΔfH°, -160.7 kJ · mol−1
- ^ ΔfG°, -143.1 kJ · mol−1
- ^ S°, 172. 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°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 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
- ^ ΔfH°, -67.07 kJ · mol−1
- ^ ΔfG°, 18.60 kJ · mol−1
- ^ S°, 161.71 J · K−1 · mol−1
- ^ ΔfH°, -92.307 kJ · mol−1
- ^ ΔfG°, -95.299 kJ · mol−1
- ^ S°, 186.908 J · K−1 · mol−1
- ^ Cp°, 29.12 J · K−1 · mol−1
- ^ ΔfH°, -167.159 kJ · mol−1
- ^ ΔfG°, -131.228 kJ · mol−1
- ^ S°, 56.5 J · K−1 · mol−1
- ^ Cp°, -136.4 J · K−1 · mol−1