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  3. 3K4[Fe(CN)6] + 14KMnO4 → 13K2O + Fe3O4 + 9N2↑ + 7Mn2O3 + 18CO↑

3K4[Fe(CN)6] + 14KMnO4 → 13K2O + Fe3O4 + 9N2↑ + 7Mn2O3 + 18CO↑

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Reaction of potassium hexacyanidoferrate(II) and potassium permanganate
3K4[Fe(CN)6]Potassium hexacyanidoferrate(II) + 14KMnO4Potassium permanganate
⟶
13K2OPotassium oxide + Fe3O4Iron(II,III) oxide + 9N2↑Nitrogen + 7Mn2O3Manganese(III) oxide + 18CO↑Carbon monoxide

The reaction of potassium hexacyanidoferrate(II) and potassium permanganate yields potassium oxide, iron(II,III) oxide, nitrogen, manganese(III) oxide, and carbon monoxide (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 potassium hexacyanidoferrate(II) and potassium permanganate
3K4[Fe(CN)6]Potassium hexacyanidoferrate(II) + 14KMnO4Potassium permanganate
⟶
13K2OPotassium oxide + Fe3O4Iron(II,III) oxide + 9N2↑Nitrogen + 7Mn2O3Manganese(III) oxide + 18CO↑Carbon monoxide

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 potassium hexacyanidoferrate(II) and potassium permanganate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
K4[Fe(CN)6]Potassium hexacyanidoferrate(II)3
Reducing
Reducing
KMnO4Potassium permanganate14
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2OPotassium oxide13
–
–
Fe3O4Iron(II,III) oxide1
Oxidized
–
N2Nitrogen9
Oxidized
–
Mn2O3Manganese(III) oxide7
Reduced
–
COCarbon monoxide18
–
–

Thermodynamic changes

Changes in standard condition

Reaction of potassium hexacyanidoferrate(II) and potassium permanganate
◆
ΔrG−2154.0 kJ/mol
K2.31 × 10377
pK−377.36
3K4[Fe(CN)6]Crystalline solid + 14KMnO4Crystalline solid
⟶
13K2OCrystalline solid + Fe3O4Crystalline solid + 9N2↑Gas + 7Mn2O3Crystalline solid + 18CO↑Gas
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
−1017.3−2154.03765.5129.2
−339.10−718.001255.243.07
−72.664−153.86268.969.229
per 1 mol of
−78.254−165.69289.659.938
per 1 mol of
−1017.3−2154.03765.5129.2
per 1 mol of
−113.03−239.33418.3914.36
−145.33−307.71537.9318.46
per 1 mol of
−56.517−119.67209.197.178

Changes in aqueous solution (1)

Reaction of potassium hexacyanidoferrate(II) and potassium permanganate
◆
ΔrG−2298.4 kJ/mol
K4.59 × 10402
pK−402.66
3K4[Fe(CN)6]Ionized aqueous solution + 14KMnO4Ionized aqueous solution
⟶
13K2OCrystalline solid + Fe3O4Crystalline solid + 9N2↑Gas + 7Mn2O3Crystalline solid + 18CO↑Gas
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
−1745.2−2298.41799.0–
−581.73−766.13599.67–
−124.66−164.17128.50–
per 1 mol of
−134.25−176.80138.38–
per 1 mol of
−1745.2−2298.41799.0–
per 1 mol of
−193.91−255.38199.89–
−249.31−328.34257.00–
per 1 mol of
−96.956−127.6999.944–

Changes in aqueous solution (2)

Reaction of potassium hexacyanidoferrate(II) and potassium permanganate
◆
ΔrG−1987.6 kJ/mol
K1.63 × 10348
pK−348.21
3K4[Fe(CN)6]Ionized aqueous solution + 14KMnO4Ionized aqueous solution
⟶
13K2OCrystalline solid + Fe3O4Crystalline solid + 9N2↑Gas + 7Mn2O3Crystalline solid + 18CO↑Un-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
−1933.0−1987.6123.7–
−644.33−662.5341.23–
−138.07−141.978.836–
per 1 mol of
−148.69−152.899.515–
per 1 mol of
−1933.0−1987.6123.7–
per 1 mol of
−214.78−220.8413.74–
−276.14−283.9417.67–
per 1 mol of
−107.39−110.426.872–

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
K4[Fe(CN)6] (cr)-594.1[1]-453.0[1]418.8[1]332.21[1]
K4[Fe(CN)6] (ai)-554.0[1]-438.01[1]505.0[1]–
K4[Fe(CN)6] (cr)
3 hydrate
-1466.5[1]-1168.8[1]593.7[1]482.42[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
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]–––
Fe3O4 (cr)-1118.4[1]-1015.4[1]146.4[1]143.43[1]
N2 (g)0[1]0[1]191.61[1]29.125[1]
Mn2O3 (cr)-959.0[1]-881.1[1]110.5[1]107.65[1]
CO (g)-110.525[1]-137.168[1]197.674[1]29.142[1]
CO (ao)-120.96[1]-119.90[1]104.6[1]–
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution

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