Ag2S + H2[PtCl6] → 2AgCl + PtCl4 + H2S↑
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The reaction of silver(I) sulfide and hexachloridoplatinic(IV) acid yields silver(I) 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 silver(I) 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 silver(I) sulfide and hexachloridoplatinic(IV) acid
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Ag2S | Silver(I) 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 |
---|---|---|---|---|
AgCl | Silver(I) chloride | 2 | 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 silver(I) 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 | 242.8 | – | – | – |
per 1 mol of | 242.8 | – | – | – |
per 1 mol of | 242.8 | – | – | – |
per 1 mol of | 121.4 | – | – | – |
per 1 mol of | 242.8 | – | – | – |
per 1 mol of | 242.8 | – | – | – |
Changes in aqueous solution (2)
- Reaction of silver(I) 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 | 223.7 | – | – | – |
per 1 mol of | 223.7 | – | – | – |
per 1 mol of | 223.7 | – | – | – |
per 1 mol of | 111.8 | – | – | – |
per 1 mol of | 223.7 | – | – | – |
per 1 mol of | 223.7 | – | – | – |
Changes in aqueous solution (3)
- Reaction of silver(I) 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 | 220.4 | – | – | – |
per 1 mol of | 220.4 | – | – | – |
per 1 mol of | 220.4 | – | – | – |
per 1 mol of | 110.2 | – | – | – |
per 1 mol of | 220.4 | – | – | – |
per 1 mol of | 220.4 | – | – | – |
Changes in aqueous solution (4)
- Reaction of silver(I) 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 | 201.3 | – | – | – |
per 1 mol of | 201.3 | – | – | – |
per 1 mol of | 201.3 | – | – | – |
per 1 mol of | 100.7 | – | – | – |
per 1 mol of | 201.3 | – | – | – |
per 1 mol of | 201.3 | – | – | – |
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 |
---|---|---|---|---|
Ag2S (cr) α, orthorhombic | -32.59[1] | -40.67[1] | 144.01[1] | 76.53[1] |
Ag2S (cr) β | -29.41[1] | -39.46[1] | 150.6[1] | – |
H2[PtCl6] (ai) | -668.2[1] | -482.7[1] | 219.7[1] | – |
H2[PtCl6] (cr) 6 hydrate | -2371.1[1] | – | – | – |
* (cr):Crystalline solid, (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 |
---|---|---|---|---|
AgCl (cr) | -127.068[1] | -109.789[1] | 96.2[1] | 50.79[1] |
AgCl (g) | – | – | 245.92[1] | 35.86[1] |
AgCl (ai) | -61.580[1] | -54.120[1] | 129.3[1] | -114.6[1] |
AgCl (ao) | -72.8[1] | -72.8[1] | 154.0[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, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (aq):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°, -32.59 kJ · mol−1
- ^ ΔfG°, -40.67 kJ · mol−1
- ^ S°, 144.01 J · K−1 · mol−1
- ^ Cp°, 76.53 J · K−1 · mol−1
- ^ ΔfH°, -29.41 kJ · mol−1
- ^ ΔfG°, -39.46 kJ · mol−1
- ^ S°, 150.6 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°, -127.068 kJ · mol−1
- ^ ΔfG°, -109.789 kJ · mol−1
- ^ S°, 96.2 J · K−1 · mol−1
- ^ Cp°, 50.79 J · K−1 · mol−1
- ^ S°, 245.92 J · K−1 · mol−1
- ^ Cp°, 35.86 J · K−1 · mol−1
- ^ ΔfH°, -61.580 kJ · mol−1
- ^ ΔfG°, -54.120 kJ · mol−1
- ^ S°, 129.3 J · K−1 · mol−1
- ^ Cp°, -114.6 J · K−1 · mol−1
- ^ ΔfH°, -72.8 kJ · mol−1
- ^ ΔfG°, -72.8 kJ · mol−1
- ^ S°, 154.0 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