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4Hg + 2KMnO4 → 4HgO + Mn2O3 + K2O

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Reaction of mercury and potassium permanganate
4HgMercury + 2KMnO4Potassium permanganate
⟶
4HgOMercury(II) oxide + Mn2O3Manganese(III) oxide + K2OPotassium oxide

The reaction of mercury and potassium permanganate yields mercury(II) oxide, manganese(III) oxide, and potassium oxide (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 mercury and potassium permanganate
4HgMercury + 2KMnO4Potassium permanganate
⟶
4HgOMercury(II) oxide + Mn2O3Manganese(III) oxide + K2OPotassium oxide

General equation

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

Oxidation state of each atom

Reaction of mercury and potassium permanganate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HgMercury4
Reducing
Oxidizable
KMnO4Potassium permanganate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
HgOMercury(II) oxide4
Oxidized
–
Mn2O3Manganese(III) oxide1
Reduced
–
K2OPotassium oxide1
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of mercury and potassium permanganate
◆
ΔrG37.8 kJ/mol
K0.24 × 10−6
pK6.62
4HgLiquid + 2KMnO4Crystalline solid
⟶
4HgOCrystalline solidred, orthorhombic + Mn2O3Crystalline solid + K2OCrystalline 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
−9.437.8−161.720.5
per 1 mol of
−2.49.45−40.425.13
−4.718.9−80.8510.3
per 1 mol of
−2.49.45−40.425.13
−9.437.8−161.720.5
per 1 mol of
−9.437.8−161.720.5

Changes in standard condition (2)

Reaction of mercury and potassium permanganate
◆
ΔrG38.4 kJ/mol
K0.19 × 10−6
pK6.73
4HgLiquid + 2KMnO4Crystalline solid
⟶
4HgOCrystalline solidyellow + Mn2O3Crystalline solid + K2OCrystalline 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
−7.938.4−158.5–
per 1 mol of
−2.09.60−39.63–
−4.019.2−79.25–
per 1 mol of
−2.09.60−39.63–
−7.938.4−158.5–
per 1 mol of
−7.938.4−158.5–

Changes in standard condition (3)

Reaction of mercury and potassium permanganate
◆
ΔrG39.1 kJ/mol
K0.14 × 10−6
pK6.85
4HgLiquid + 2KMnO4Crystalline solid
⟶
4HgOCrystalline solidhexagonal + Mn2O3Crystalline solid + K2OCrystalline 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
−4.139.1−148.5–
per 1 mol of
−1.09.78−37.13–
−2.019.6−74.25–
per 1 mol of
−1.09.78−37.13–
−4.139.1−148.5–
per 1 mol of
−4.139.1−148.5–

Changes in aqueous solution

Reaction of mercury and potassium permanganate
◆
ΔrG−133.6 kJ/mol
K2.55 × 1023
pK−23.41
4HgUn-ionized aqueous solution + 2KMnO4Ionized aqueous solution
⟶
4HgOCrystalline solidred, orthorhombic + Mn2O3Crystalline solid + K2OCrystalline 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
−247.0−133.6−386–
per 1 mol of
−61.75−33.40−96.5–
−123.5−66.80−193–
per 1 mol of
−61.75−33.40−96.5–
−247.0−133.6−386–
per 1 mol of
−247.0−133.6−386–

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
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]–
KMnO4 (cr)-837.2[1]-737.6[1]171.71[1]117.57[1]
KMnO4 (ai)-793.8[1]-730.5[1]293.7[1]-60.2[1]
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (ai):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
HgO (cr)
red, orthorhombic
-90.83[1]-58.539[1]70.29[1]44.06[1]
HgO (cr)
yellow
-90.46[1]-58.409[1]71.1[1]–
HgO (cr)
hexagonal
-89.5[1]-58.22[1]73.6[1]–
HgO (g)––241.9[1]34.10[1]
Mn2O3 (cr)-959.0[1]-881.1[1]110.5[1]107.65[1]
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]–––
* (cr):Crystalline solid, (g):Gas

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)
    • 2
      James G. Speight (2017)
      Lange's Handbook of Chemistry, 17th edition
      McGraw Hill Education