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2H2S + 3HgSO4 🔥→ 5SO2 + 3Hg + 2H2O

The reaction of hydrogen sulfide and mercury(II) sulfate yields sulfur dioxide, mercury, and water (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 reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide2
Reducing
Reducing
HgSO4Mercury(II) sulfate3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide5
Redoxed product
HgMercury3
Reduced
H2OWater2

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and mercury(II) sulfate
2H2SGas + 3HgSO4Crystalline solid
🔥
5SO2Gas + 3HgLiquid + 2H2OLiquid
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
108.0
per 1 mol of
54.00
36.00
per 1 mol of
21.60
per 1 mol of
36.00
per 1 mol of
54.00

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and mercury(II) sulfate
ΔrG−37.1 kJ/mol
K3.16 × 106
pK−6.50
2H2SUn-ionized aqueous solution + 3HgSO4Un-ionized aqueous solution
🔥
5SO2Gas + 3HgUn-ionized aqueous solution + 2H2OLiquid
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
−37.1
per 1 mol of
−18.6
−12.4
per 1 mol of
−7.42
per 1 mol of
−12.4
per 1 mol of
−18.6

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and mercury(II) sulfate
ΔrG−39.5 kJ/mol
K8.32 × 106
pK−6.92
2H2SUn-ionized aqueous solution + 3HgSO4Un-ionized aqueous solution
🔥
5SO2Un-ionized aqueous solution + 3HgUn-ionized aqueous solution + 2H2OLiquid
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
−39.5
per 1 mol of
−19.8
−13.2
per 1 mol of
−7.90
per 1 mol of
−13.2
per 1 mol of
−19.8

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]
HgSO4 (cr)-707.5[1]
HgSO4 (ao)-588.2[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
SO2 (l)-320.5[1]
SO2 (g)-296.830[1]-300.194[1]248.22[1]39.87[1]
SO2 (ao)-322.980[1]-300.676[1]161.9[1]
Hg (cr)
Hg (l)0[1]0[1]76.02[1]27.983[1]
Hg (g)61.317[1]31.820[1]174.96[1]20.786[1]
Hg (ao)37.7[1]39.3[1]71[1]
H2O (cr)
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid

References

List of references

  1. 1