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HgI2 + Cl2 → HgCl2 + I2

The reaction of mercury(II) iodide and chlorine yields mercury(II) chloride and iodine. 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 categories

Reaction data

Chemical equation

General equation

Reaction of oxidizable species and oxidizing species
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HgI2Mercury(II) iodide1
Reducing
Oxidizable
Cl2Chlorine1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
HgCl2Mercury(II) chloride1
Reduced
I2Iodine1
Oxidized

Thermodynamic changes

Changes in standard condition (1)

Reaction of mercury(II) iodide and chlorine
ΔrG−76.9 kJ/mol
K2.97 × 1013
pK−13.47
HgI2Crystalline solidred + Cl2Gas
HgCl2Crystalline solid + I2Crystalline solid
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
−118.9−76.9−141
per 1 mol of
−118.9−76.9−141
per 1 mol of
−118.9−76.9−141
−118.9−76.9−141
per 1 mol of
−118.9−76.9−141

Changes in standard condition (2)

Reaction of mercury(II) iodide and chlorine
HgI2Crystalline solidyellow + Cl2Gas
HgCl2Crystalline solid + I2Crystalline solid
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
−121.4
per 1 mol of
−121.4
per 1 mol of
−121.4
−121.4
per 1 mol of
−121.4

Changes in aqueous solution

Reaction of mercury(II) iodide and chlorine
ΔrG−88.4 kJ/mol
K3.07 × 1015
pK−15.49
HgI2Un-ionized aqueous solution + Cl2Un-ionized aqueous solution
HgCl2Un-ionized aqueous solution + I2Un-ionized 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
−90.8−88.4−5
per 1 mol of
−90.8−88.4−5
per 1 mol of
−90.8−88.4−5
−90.8−88.4−5
per 1 mol of
−90.8−88.4−5

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
HgI2 (cr)
red
-105.4[1]-101.7[1]180[1]
HgI2 (cr)
yellow
-102.9[1]
HgI2 (g)-17.2[1]-59.9[1]336.13[1]61.09[1]
HgI2 (ao)-79.5[1]-75.3[1]176[1]
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[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
HgCl2 (cr)-224.3[1]-178.6[1]146.0[1]
HgCl2 (ao)-216.3[1]-173.2[1]155[1]
I2 (cr)0[1]0[1]116.135[1]54.438[1]
I2 (g)62.438[1]19.327[1]260.69[1]36.90[1]
I2 (ao)22.6[1]16.40[1]137.2[1]
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (g):Gas

References

List of references

  1. 1