HgCl2 + K2S 💧→ HgS↓ + 2KCl
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The reaction of mercury(II) chloride and potassium sulfide yields mercury(II) sulfide and potassium 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 potassium sulfide
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 potassium sulfide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgCl2 | Mercury(II) chloride | 1 | Lewis acid | Soluble in water |
| K2S | Potassium sulfide | 1 | Lewis base | Soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgS | Mercury(II) sulfide | 1 | Lewis conjugate | Insoluble in water |
| KCl | Potassium chloride | 2 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of mercury(II) chloride and potassium sulfide◆
ΔrG −326.3 kJ/mol K 1.46 × 1057 pK −57.17
| 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 | −326.7 | −326.3 | −3 | – |
per 1 mol of | −326.7 | −326.3 | −3 | – |
per 1 mol of | −326.7 | −326.3 | −3 | – |
per 1 mol of | −326.7 | −326.3 | −3 | – |
per 1 mol of | −163.3 | −163.2 | −2 | – |
Changes in standard condition (2)
- Reaction of mercury(II) chloride and potassium sulfide◆
ΔrG −323.4 kJ/mol K 4.54 × 1056 pK −56.66
| 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 | −322.1 | −323.4 | 2 | – |
per 1 mol of | −322.1 | −323.4 | 2 | – |
per 1 mol of | −322.1 | −323.4 | 2 | – |
per 1 mol of | −322.1 | −323.4 | 2 | – |
per 1 mol of | −161.1 | −161.7 | 1 | – |
Changes in aqueous solution
- Reaction of mercury(II) chloride and potassium sulfide◆
ΔrG −225.7 kJ/mol K 3.47 × 1039 pK −39.54
| 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 | −209.5 | −225.7 | 55 | – |
per 1 mol of | −209.5 | −225.7 | 55 | – |
per 1 mol of | −209.5 | −225.7 | 55 | – |
per 1 mol of | −209.5 | −225.7 | 55 | – |
per 1 mol of | −104.8 | −112.8 | 28 | – |
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] | – |
| K2S (cr) | -380.7[1] | -364.0[1] | 105[1] | – |
| K2S (ai) | -471.5[1] | -480.7[1] | 190.4[1] | – |
| K2S (cr) 2 hydrate | -975.3[1] | – | – | – |
| K2S (cr) 5 hydrate | -1871.5[1] | – | – | – |
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (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 |
|---|---|---|---|---|
| HgS (cr) red | -58.2[1] | -50.6[1] | 82.4[1] | 48.41[1] |
| HgS (cr) black | -53.6[1] | -47.7[1] | 88.3[1] | – |
| HgS (g) | – | – | 254.75[1] | – |
| KCl (cr) | -436.747[1] | -409.14[1] | 82.59[1] | 51.30[1] |
| KCl (g) | -214.14[1] | -233.0[1] | 239.10[1] | 36.48[1] |
| KCl (ai) | -419.53[1] | -414.49[1] | 159.0[1] | -114.6[1] |
* (cr):Crystalline solid, (g):Gas, (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°, -380.7 kJ · mol−1
- ^ ΔfG°, -364.0 kJ · mol−1
- ^ S°, 105. J · K−1 · mol−1
- ^ ΔfH°, -471.5 kJ · mol−1
- ^ ΔfG°, -480.7 kJ · mol−1
- ^ S°, 190.4 J · K−1 · mol−1
- ^ ΔfH°, -975.3 kJ · mol−1
- ^ ΔfH°, -1871.5 kJ · mol−1
- ^ ΔfH°, -58.2 kJ · mol−1
- ^ ΔfG°, -50.6 kJ · mol−1
- ^ S°, 82.4 J · K−1 · mol−1
- ^ Cp°, 48.41 J · K−1 · mol−1
- ^ ΔfH°, -53.6 kJ · mol−1
- ^ ΔfG°, -47.7 kJ · mol−1
- ^ S°, 88.3 J · K−1 · mol−1
- ^ S°, 254.75 J · K−1 · mol−1
- ^ ΔfH°, -436.747 kJ · mol−1
- ^ ΔfG°, -409.14 kJ · mol−1
- ^ S°, 82.59 J · K−1 · mol−1
- ^ Cp°, 51.30 J · K−1 · mol−1
- ^ ΔfH°, -214.14 kJ · mol−1
- ^ ΔfG°, -233.0 kJ · mol−1
- ^ S°, 239.10 J · K−1 · mol−1
- ^ Cp°, 36.48 J · K−1 · mol−1
- ^ ΔfH°, -419.53 kJ · mol−1
- ^ ΔfG°, -414.49 kJ · mol−1
- ^ S°, 159.0 J · K−1 · mol−1
- ^ Cp°, -114.6 J · K−1 · mol−1