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Li[AlH4] + 2KMnO4 → LiOH + Mn2O3 + Al(OH)3 + K2O

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Reaction of lithium tetrahydridoaluminate and potassium permanganate
Li[AlH4]Lithium tetrahydridoaluminate + 2KMnO4Potassium permanganate
⟶
LiOHLithium hydroxide + Mn2O3Manganese(III) oxide + Al(OH)3Aluminium hydroxide + K2OPotassium oxide

The reaction of lithium tetrahydridoaluminate and potassium permanganate yields lithium hydroxide, manganese(III) oxide, aluminium hydroxide, 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 lithium tetrahydridoaluminate and potassium permanganate
Li[AlH4]Lithium tetrahydridoaluminate + 2KMnO4Potassium permanganate
⟶
LiOHLithium hydroxide + Mn2O3Manganese(III) oxide + Al(OH)3Aluminium hydroxide + K2OPotassium oxide

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of lithium tetrahydridoaluminate and potassium permanganate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Li[AlH4]Lithium tetrahydridoaluminate1
Reducing
Reducing
KMnO4Potassium permanganate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
LiOHLithium hydroxide1
Oxidized
–
Mn2O3Manganese(III) oxide1
Reduced
–
Al(OH)3Aluminium hydroxide1
Oxidized
–
K2OPotassium oxide1
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of lithium tetrahydridoaluminate and potassium permanganate
◆
ΔrG−1428 kJ/mol
K1.50 × 10250
pK−250.17
Li[AlH4]Crystalline solid + 2KMnO4Crystalline solid
⟶
LiOHCrystalline solid + Mn2O3Crystalline solid + Al(OH)3Crystalline 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
−1299−1428−10415.8
−1299−1428−10415.8
−649.5−714.0−52.07.90
per 1 mol of
−1299−1428−10415.8
−1299−1428−10415.8
−1299−1428−10415.8
per 1 mol of
−1299−1428−10415.8

Changes in standard condition (2)

Reaction of lithium tetrahydridoaluminate and potassium permanganate
Li[AlH4]Crystalline solid + 2KMnO4Crystalline solid
⟶
LiOHCrystalline solid + Mn2O3Crystalline solid + Al(OH)3Amorphous 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
−1291–––
−1291–––
−645.5–––
per 1 mol of
−1291–––
−1291–––
−1291–––
per 1 mol of
−1291–––

Changes in aqueous solution (1)

Reaction of lithium tetrahydridoaluminate and potassium permanganate
◆
ΔrG−1454 kJ/mol
K5.37 × 10254
pK−254.73
Li[AlH4]Crystalline solid + 2KMnO4Ionized aqueous solution
⟶
LiOHIonized aqueous solution + Mn2O3Crystalline solid + Al(OH)3Crystalline 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
−1409−1454−388241.8
−1409−1454−388241.8
−704.5−727.0−194120.9
per 1 mol of
−1409−1454−388241.8
−1409−1454−388241.8
−1409−1454−388241.8
per 1 mol of
−1409−1454−388241.8

Changes in aqueous solution (2)

Reaction of lithium tetrahydridoaluminate and potassium permanganate
◆
ΔrG−1455 kJ/mol
K8.03 × 10254
pK−254.90
Li[AlH4]Crystalline solid + 2KMnO4Ionized aqueous solution
⟶
LiOHUn-ionized aqueous solution + Mn2O3Crystalline solid + Al(OH)3Crystalline 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
−1409−1455−383–
−1409−1455−383–
−704.5−727.5−192–
per 1 mol of
−1409−1455−383–
−1409−1455−383–
−1409−1455−383–
per 1 mol of
−1409−1455−383–

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
Li[AlH4] (cr)-116.3[1]-44.7[1]78.74[1]83.18[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

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
LiOH (cr)-484.93[1]-438.95[1]42.80[1]49.66[1]
LiOH (g)-238.1[1]-242.3[1]210.90[1]46.02[1]
LiOH (ai)-508.48[1]-450.58[1]2.80[1]-79.9[1]
LiOH (ao)-508.4[1]-451.8[1]7.1[1]–
LiOH (cr)
1 hydrate
-788.01[1]-680.95[1]71.21[1]79.50[1]
Mn2O3 (cr)-959.0[1]-881.1[1]110.5[1]107.65[1]
Al(OH)3 (cr)-1284[2]-1306[2]71[2]93.1[2]
Al(OH)3 (am)-1276[1]–––
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]–––
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (am):Amorphous solid

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