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15Co(OH)2 + 2KMnO4 → 5Co3O4 + 2MnO + 2KOH + 14H2O

The reaction of cobalt(II) hydroxide and potassium permanganate yields cobalt(II,III) oxide, manganese(II) oxide, potassium hydroxide, 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

General equation

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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Co(OH)2Cobalt(II) hydroxide15
Reducing
Hardly oxidizable
KMnO4Potassium permanganate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Co3O4Cobalt(II,III) oxide5
Oxidized
MnOManganese(II) oxide2
Reduced
KOHPotassium hydroxide2
H2OWater14

Thermodynamic changes

Changes in standard condition (1)

Reaction of cobalt(II) hydroxide and potassium permanganate
ΔrG−447 kJ/mol
K2.05 × 1078
pK−78.31
15Co(OH)2Crystalline solidblue, precipitated + 2KMnO4Crystalline solid
5Co3O4Crystalline solid + 2MnOCrystalline solid + 2KOHCrystalline solid + 14H2OLiquid
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
−447
−29.8
−224
−89.4
−224
−224
per 1 mol of
−31.9

Changes in standard condition (2)

Reaction of cobalt(II) hydroxide and potassium permanganate
ΔrG−384 kJ/mol
K1.88 × 1067
pK−67.27
15Co(OH)2Crystalline solidpink, precipitated + 2KMnO4Crystalline solid
5Co3O4Crystalline solid + 2MnOCrystalline solid + 2KOHCrystalline solid + 14H2OLiquid
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
−307−384240
−20.5−25.616.0
−154−192120
−61.4−76.848.0
−154−192120
−154−192120
per 1 mol of
−21.9−27.417.1

Changes in standard condition (3)

Reaction of cobalt(II) hydroxide and potassium permanganate
ΔrG−327 kJ/mol
K1.94 × 1057
pK−57.29
15Co(OH)2Crystalline solidpink, precipitated, aged + 2KMnO4Crystalline solid
5Co3O4Crystalline solid + 2MnOCrystalline solid + 2KOHCrystalline solid + 14H2OLiquid
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
−327
−21.8
−164
−65.4
−164
−164
per 1 mol of
−23.4

Changes in aqueous solution (1)

Reaction of cobalt(II) hydroxide and potassium permanganate
ΔrG−1010 kJ/mol
K8.80 × 10176
pK−176.94
15Co(OH)2Un-ionized aqueous solution + 2KMnO4Ionized aqueous solution
5Co3O4Crystalline solid + 2MnOCrystalline solid + 2KOHIonized aqueous solution + 14H2OLiquid
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
−1010
−67.33
−505.0
−202.0
−505.0
−505.0
per 1 mol of
−72.14

Changes in aqueous solution (2)

Reaction of cobalt(II) hydroxide and potassium permanganate
ΔrG−584 kJ/mol
K2.05 × 10102
pK−102.31
15Co(OH)2Crystalline solidblue, precipitated + 2KMnO4Ionized aqueous solution
5Co3O4Crystalline solid + 2MnOCrystalline solid + 2KOHIonized aqueous solution + 14H2OLiquid
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
−584
−38.9
−292
−117
−292
−292
per 1 mol of
−41.7

Changes in aqueous solution (3)

Reaction of cobalt(II) hydroxide and potassium permanganate
ΔrG−521 kJ/mol
K1.88 × 1091
pK−91.28
15Co(OH)2Crystalline solidpink, precipitated + 2KMnO4Ionized aqueous solution
5Co3O4Crystalline solid + 2MnOCrystalline solid + 2KOHIonized aqueous solution + 14H2OLiquid
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
−509−52121
−33.9−34.71.4
−255−26111
−102−1044.2
−255−26111
−255−26111
per 1 mol of
−36.4−37.21.5

Changes in aqueous solution (4)

Reaction of cobalt(II) hydroxide and potassium permanganate
ΔrG−464 kJ/mol
K1.95 × 1081
pK−81.29
15Co(OH)2Crystalline solidpink, precipitated, aged + 2KMnO4Ionized aqueous solution
5Co3O4Crystalline solid + 2MnOCrystalline solid + 2KOHIonized aqueous solution + 14H2OLiquid
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
−464
−30.9
−232
−92.8
−232
−232
per 1 mol of
−33.1

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
Co(OH)2 (cr)
blue, precipitated
-450.1[1]
Co(OH)2 (cr)
pink, precipitated
-539.7[1]-454.3[1]79[1]
Co(OH)2 (cr)
pink, precipitated, aged
-458.1[1]
Co(OH)2 (ai)-518.0[1]-369.0[1]-134[1]
Co(OH)2 (ao)-421.7[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, (ai):Ionized aqueous solution, (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
Co3O4 (cr)-891[1]-774[1]102.5[1]123.4[1]
MnO (cr)-385.22[1]-362.90[1]59.71[1]45.44[1]
MnO (g)124.22[1]
KOH (cr)-424.764[1]-379.08[1]78.9[1]64.9[1]
KOH (g)-231.0[1]-232.6[1]238.3[1]49.20[1]
KOH (ai)-482.37[1]-440.50[1]91.6[1]-126.8[1]
KOH (cr)
1 hydrate
-748.9[1]-645.1[1]117.2[1]
KOH (cr)
2 hydrate
-1051.0[1]-887.3[1]150.6[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]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid

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)