2H2S + Na2[PtCl6] → 2S + Pt + 2NaCl + 4HCl
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The reaction of hydrogen sulfide and sodium hexachloridoplatinate(IV) yields , , sodium chloride, 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 hydrogen sulfide and sodium hexachloridoplatinate(IV)
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of hydrogen sulfide and sodium hexachloridoplatinate(IV)
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
H2S | Hydrogen sulfide | 2 | Reducing | Reducing |
Na2[PtCl6] | Sodium hexachloridoplatinate(IV) | 1 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
2 | Oxidized | – | ||
1 | Reduced | – | ||
NaCl | Sodium chloride | 2 | – | – |
HCl | Hydrogen chloride | 4 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen sulfide and sodium hexachloridoplatinate(IV)
- 2H2SGas + Na2[PtCl6]Crystalline solid2Crystalline solidrhombic + Crystalline solid + 2NaClCrystalline solid + 4HClGas⟶
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 | −34.4 | – | – | – |
per 1 mol of | −17.2 | – | – | – |
per 1 mol of | −34.4 | – | – | – |
−17.2 | – | – | – | |
−34.4 | – | – | – | |
per 1 mol of | −17.2 | – | – | – |
per 1 mol of | −8.60 | – | – | – |
Changes in standard condition (2)
- Reaction of hydrogen sulfide and sodium hexachloridoplatinate(IV)
- 2H2SGas + Na2[PtCl6]Crystalline solid2Crystalline solidmonoclinic + Crystalline solid + 2NaClCrystalline solid + 4HClGas⟶
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 | −33.7 | – | – | – |
per 1 mol of | −16.9 | – | – | – |
per 1 mol of | −33.7 | – | – | – |
−16.9 | – | – | – | |
−33.7 | – | – | – | |
per 1 mol of | −16.9 | – | – | – |
per 1 mol of | −8.43 | – | – | – |
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and sodium hexachloridoplatinate(IV)
- 2H2SUn-ionized aqueous solution + Na2[PtCl6]Crystalline solid2Crystalline solidrhombic + Crystalline solid + 2NaClIonized aqueous solution + 4HClGas⟶
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 | 11.5 | – | – | – |
per 1 mol of | 5.75 | – | – | – |
per 1 mol of | 11.5 | – | – | – |
5.75 | – | – | – | |
11.5 | – | – | – | |
per 1 mol of | 5.75 | – | – | – |
per 1 mol of | 2.88 | – | – | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and sodium hexachloridoplatinate(IV)
- 2H2SUn-ionized aqueous solution + Na2[PtCl6]Crystalline solid2Crystalline solidrhombic + Crystalline solid + 2NaClIonized aqueous solution + 4HClIonized aqueous solution⟶
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 | −287.9 | – | – | – |
per 1 mol of | −143.9 | – | – | – |
per 1 mol of | −287.9 | – | – | – |
−143.9 | – | – | – | |
−287.9 | – | – | – | |
per 1 mol of | −143.9 | – | – | – |
per 1 mol of | −71.97 | – | – | – |
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 |
---|---|---|---|---|
H2S (g) | -20.63[1] | -33.56[1] | 205.79[1] | 34.23[1] |
H2S (ao) | -39.7[1] | -27.83[1] | 121[1] | – |
Na2[PtCl6] (cr) | -1115.9[1] | – | – | – |
Na2[PtCl6] (cr) 2 hydrate | -1723.8[1] | – | – | – |
Na2[PtCl6] (cr) 6 hydrate | -2912.1[1] | – | – | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid
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 |
---|---|---|---|---|
(cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
(cr) monoclinic | 0.33[1] | – | – | – |
(g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
(cr) | 0[1] | 0[1] | 41.63[1] | 25.86[1] |
(g) | 565.3[1] | 520.5[1] | 192.406[1] | 25.531[1] |
NaCl (cr) | -411.153[1] | -384.138[1] | 72.13[1] | 50.50[1] |
NaCl (g) | -176.65[1] | -196.66[1] | 229.81[1] | 35.77[1] |
NaCl (ai) | -407.27[1] | -393.133[1] | 115.5[1] | -90.0[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, (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°, -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
- ^ ΔfH°, -1115.9 kJ · mol−1
- ^ ΔfH°, -1723.8 kJ · mol−1
- ^ ΔfH°, -2912.1 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 41.63 J · K−1 · mol−1
- ^ Cp°, 25.86 J · K−1 · mol−1
- ^ ΔfH°, 565.3 kJ · mol−1
- ^ ΔfG°, 520.5 kJ · mol−1
- ^ S°, 192.406 J · K−1 · mol−1
- ^ Cp°, 25.531 J · K−1 · mol−1
- ^ ΔfH°, -411.153 kJ · mol−1
- ^ ΔfG°, -384.138 kJ · mol−1
- ^ S°, 72.13 J · K−1 · mol−1
- ^ Cp°, 50.50 J · K−1 · mol−1
- ^ ΔfH°, -176.65 kJ · mol−1
- ^ ΔfG°, -196.66 kJ · mol−1
- ^ S°, 229.81 J · K−1 · mol−1
- ^ Cp°, 35.77 J · K−1 · mol−1
- ^ ΔfH°, -407.27 kJ · mol−1
- ^ ΔfG°, -393.133 kJ · mol−1
- ^ S°, 115.5 J · K−1 · mol−1
- ^ Cp°, -90.0 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