HgS + H2[PtCl6] → HgCl2 + PtCl4 + H2S↑
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The reaction of mercury(II) sulfide and hexachloridoplatinic(IV) acid yields mercury(II) chloride, platinum(IV) chloride, and hydrogen sulfide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of mercury(II) sulfide and hexachloridoplatinic(IV) acid
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Weak acidConjugate acid
Oxidation state of each atom
- Reaction of mercury(II) sulfide and hexachloridoplatinic(IV) acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgS | Mercury(II) sulfide | 1 | Brønsted base | Salt of weak acid |
| H2[PtCl6] | Hexachloridoplatinic(IV) acid | 1 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgCl2 | Mercury(II) chloride | 1 | Conjugate base | Salt of strong acid |
| PtCl4 | Platinum(IV) chloride | 1 | Conjugate base | Salt of strong acid |
| H2S | Hydrogen sulfide | 1 | Conjugate acid | Weak acid |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of mercury(II) sulfide and hexachloridoplatinic(IV) acid
| 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 | 175.3 | – | – | – |
per 1 mol of | 175.3 | – | – | – |
per 1 mol of | 175.3 | – | – | – |
per 1 mol of | 175.3 | – | – | – |
per 1 mol of | 175.3 | – | – | – |
per 1 mol of | 175.3 | – | – | – |
Changes in aqueous solution (2)
- Reaction of mercury(II) sulfide and hexachloridoplatinic(IV) acid
| 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 | 156.2 | – | – | – |
per 1 mol of | 156.2 | – | – | – |
per 1 mol of | 156.2 | – | – | – |
per 1 mol of | 156.2 | – | – | – |
per 1 mol of | 156.2 | – | – | – |
per 1 mol of | 156.2 | – | – | – |
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 |
|---|---|---|---|---|
| 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] | – |
| H2[PtCl6] (ai) | -668.2[1] | -482.7[1] | 219.7[1] | – |
| H2[PtCl6] (cr) 6 hydrate | -2371.1[1] | – | – | – |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| HgCl2 (cr) | -224.3[1] | -178.6[1] | 146.0[1] | – |
| HgCl2 (ao) | -216.3[1] | -173.2[1] | 155[1] | – |
| PtCl4 (cr) | -231.8[1] | – | – | – |
| PtCl4 (aq) | -314.2[1] | – | – | – |
| PtCl4 (cr) 5 hydrate | -1752.7[1] | – | – | – |
| H2S (g) | -20.63[1] | -33.56[1] | 205.79[1] | 34.23[1] |
| H2S (ao) | -39.7[1] | -27.83[1] | 121[1] | – |
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (aq):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°, -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°, -668.2 kJ · mol−1
- ^ ΔfG°, -482.7 kJ · mol−1
- ^ S°, 219.7 J · K−1 · mol−1
- ^ ΔfH°, -2371.1 kJ · 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°, -231.8 kJ · mol−1
- ^ ΔfH°, -314.2 kJ · mol−1
- ^ ΔfH°, -1752.7 kJ · mol−1
- ^ ΔfH°, -20.63 kJ · mol−1
- ^ ΔfG°, -33.56 kJ · mol−1
- ^ S°, 205.79 J · K−1 · mol−1
- ^ Cp°, 34.23 J · K−1 · mol−1
- ^ ΔfH°, -39.7 kJ · mol−1
- ^ ΔfG°, -27.83 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1