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15Cu + 4HgSO4 + 32H+ 🔥→ 15Cu2+ + 2Hg22+ + 4S + 16H2O

Reaction of copper and mercury(II) sulfate under acidic condition
15CuCopper + 4HgSO4Mercury(II) sulfate + 32H+Hydrogen ion
🔥
15Cu2+Copper(II) ion + 2Hg22+Dimercury(I) ion + 4SSulfur + 16H2OWater

The reaction of copper, mercury(II) sulfate, and hydrogen ion yields copper(II) ion, dimercury(I) ion, sulfur, 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

Reaction of copper and mercury(II) sulfate under acidic condition
15CuCopper + 4HgSO4Mercury(II) sulfate + 32H+Hydrogen ion
🔥
15Cu2+Copper(II) ion + 2Hg22+Dimercury(I) ion + 4SSulfur + 16H2OWater

General equation

Reaction of oxidizable species and oxidizing species under acidic condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent
ProductOxidation product + ProductReduction product + H2ONon-redox product

Oxidation state of each atom

Reaction of copper and mercury(II) sulfate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper15
Reducing
Oxidizable
HgSO4Mercury(II) sulfate4
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion32
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu2+Copper(II) ion15
Oxidized
Hg22+Dimercury(I) ion2
Reduced
SSulfur4
Reduced
H2OWater16
Water

Thermodynamic changes

Changes in standard condition

Reaction of copper and mercury(II) sulfate under acidic condition
ΔrG−151.9 kJ/mol
K4.09 × 1026
pK−26.61
15CuCrystalline solid + 4HgSO4Un-ionized aqueous solution + 32H+Un-ionized aqueous solution
🔥
15Cu2+Un-ionized aqueous solution + 2Hg22+Un-ionized aqueous solution + 4SCrystalline solidrhombic + 16H2OLiquid
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
−151.9
per 1 mol of
−10.13
−37.98
per 1 mol of
Hydrogen ion
−4.747
per 1 mol of
Copper(II) ion
−10.13
per 1 mol of
Dimercury(I) ion
−75.95
per 1 mol of
−37.98
per 1 mol of
−9.494

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
Cu (cr)0[1]0[1]33.150[1]24.435[1]
Cu (g)338.32[1]298.58[1]166.38[1]20.786[1]
HgSO4 (cr)-707.5[1]
HgSO4 (ao)-588.2[1]
H+ (g)1536.202[1]
H+ (ao)0[1]0[1]0[1]0[1]
* (cr):Crystalline solid, (g):Gas, (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
Cu2+ (g)3054.07[1]
Cu2+ (ao)64.77[1]65.49[1]-99.6[1]
Hg22+ (ao)172.4[1]153.52[1]84.5[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]
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]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid

References

List of references

  1. 1