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HgSO4 + 6e → Hg2+ + S + 4O2−

Reduction of mercury(II) sulfate
HgSO4Mercury(II) sulfate + 6eElectron
Hg2+Mercury(II) ion + SSulfur + 4O2−Oxide ion

Reduction of mercury(II) sulfate yields mercury(II) ion, sulfur, and oxide ion (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

Reduction of mercury(II) sulfate
HgSO4Mercury(II) sulfate + 6eElectron
Hg2+Mercury(II) ion + SSulfur + 4O2−Oxide ion

General equation

Reduction of reducible species
ReactantOxidizing agent + e
ProductReduction product

Oxidation state of each atom

Reduction of mercury(II) sulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HgSO4Mercury(II) sulfate1
Oxidizing
eElectron6
Electron

Products

Chemical formulaNameCoefficientTypeType in general
equation
Hg2+Mercury(II) ion1
SSulfur1
Reduced
O2−Oxide ion4

Thermodynamic changes

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
HgSO4 (cr)-707.5[1]
HgSO4 (ao)-588.2[1]
e
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution

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
Hg2+ (g)2890.47[1]
Hg2+ (ao)171.1[1]164.40[1]-32.2[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]
O2−
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid

References

List of references

  1. 1