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2H2S + Na2[PtCl6] → 2S + Pt + 2NaCl + 4HCl

The reaction of hydrogen sulfide and sodium hexachloridoplatinate(IV) yields sulfur, platinum, sodium chloride, and hydrogen chloride (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide2
Reducing
Reducing
Na2[PtCl6]Sodium hexachloridoplatinate(IV)1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SSulfur2
Oxidized
PtPlatinum1
Reduced
NaClSodium chloride2
HClHydrogen chloride4

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and sodium hexachloridoplatinate(IV)
2H2SGas + Na2[PtCl6]Crystalline solid
2SCrystalline solidrhombic + PtCrystalline 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
−34.4
per 1 mol of
−17.2
per 1 mol of
−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 solid
2SCrystalline solidmonoclinic + PtCrystalline 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
−33.7
per 1 mol of
−16.9
per 1 mol of
−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 solid
2SCrystalline solidrhombic + PtCrystalline 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
11.5
per 1 mol of
5.75
per 1 mol of
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 solid
2SCrystalline solidrhombic + PtCrystalline 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
−287.9
per 1 mol of
−143.9
per 1 mol of
−287.9
per 1 mol of
−143.9
per 1 mol of
−71.97

Thermodynamic data of reactants

Chemical formulaStandard 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 formulaStandard 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
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
Pt (cr)0[1]0[1]41.63[1]25.86[1]
Pt (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

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)