You-iggy

6Cu + 2HgSO4 + 4H+ 🔥→ 2Cu2SO3 + 2Cu+ + Hg22+ + 2H2O

Reaction of copper and mercury(II) sulfate under acidic condition
6CuCopper + 2HgSO4Mercury(II) sulfate + 4H+Hydrogen ion
🔥
2Cu2SO3Copper(I) sulfite + 2Cu+Copper(I) ion + Hg22+Dimercury(I) ion + 2H2OWater

The reaction of copper, mercury(II) sulfate, and hydrogen ion yields copper(I) sulfite, copper(I) ion, dimercury(I) ion, 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
6CuCopper + 2HgSO4Mercury(II) sulfate + 4H+Hydrogen ion
🔥
2Cu2SO3Copper(I) sulfite + 2Cu+Copper(I) ion + Hg22+Dimercury(I) ion + 2H2OWater

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
CuCopper6
Reducing
Oxidizable
HgSO4Mercury(II) sulfate2
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion4
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu2SO3Copper(I) sulfite2
Redoxed product
Cu+Copper(I) ion2
Oxidized
Hg22+Dimercury(I) ion1
Reduced
H2OWater2
Water

Thermodynamic changes

Changes in aqueous solution

Reaction of copper and mercury(II) sulfate under acidic condition
ΔrG182.4 kJ/mol
K0.11 × 10−31
pK31.96
6CuCrystalline solid + 2HgSO4Un-ionized aqueous solution + 4H+Un-ionized aqueous solution
🔥
2Cu2SO3Ionized aqueous solution + 2Cu+Un-ionized aqueous solution + Hg22+Un-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
182.4
per 1 mol of
30.40
91.20
per 1 mol of
Hydrogen ion
45.60
per 1 mol of
91.20
per 1 mol of
Copper(I) ion
91.20
per 1 mol of
Dimercury(I) ion
182.4
per 1 mol of
91.20

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
Cu2SO3 (ai)-492.0[1]-386.6[1]50[1]
Cu+ (g)1089.986[1]
Cu+ (ao)71.67[1]49.98[1]40.6[1]
Hg22+ (ao)172.4[1]153.52[1]84.5[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]
* (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid

References

List of references

  1. 1