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  3. 2K3[Fe(CN)6] + 28KMnO4 → 12K2CO3 + 5K2O + 12NO↑ + 28MnO2 + Fe2O3

2K3[Fe(CN)6] + 28KMnO4 → 12K2CO3 + 5K2O + 12NO↑ + 28MnO2 + Fe2O3

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Reaction of potassium hexacyanidoferrate(III) and potassium permanganate
2K3[Fe(CN)6]Potassium hexacyanidoferrate(III) + 28KMnO4Potassium permanganate
⟶
12K2CO3Potassium carbonate + 5K2OPotassium oxide + 12NO↑Nitrogen monoxide + 28MnO2Manganese(IV) oxide + Fe2O3Iron(III) oxide

The reaction of potassium hexacyanidoferrate(III) and potassium permanganate yields potassium carbonate, potassium oxide, nitrogen monoxide, manganese(IV) oxide, and iron(III) 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 potassium hexacyanidoferrate(III) and potassium permanganate
2K3[Fe(CN)6]Potassium hexacyanidoferrate(III) + 28KMnO4Potassium permanganate
⟶
12K2CO3Potassium carbonate + 5K2OPotassium oxide + 12NO↑Nitrogen monoxide + 28MnO2Manganese(IV) oxide + Fe2O3Iron(III) 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 potassium hexacyanidoferrate(III) and potassium permanganate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
K3[Fe(CN)6]Potassium hexacyanidoferrate(III)2
Reducing
Reducing
KMnO4Potassium permanganate28
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2CO3Potassium carbonate12
Oxidized
–
K2OPotassium oxide5
–
–
NONitrogen monoxide12
Oxidized
–
MnO2Manganese(IV) oxide28
Reduced
–
Fe2O3Iron(III) oxide1
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium hexacyanidoferrate(III) and potassium permanganate
◆
ΔrG−6188.0 kJ/mol
K1.23 × 101084
pK−1084.09
2K3[Fe(CN)6]Crystalline solid + 28KMnO4Crystalline solid
⟶
12K2CO3Crystalline solid + 5K2OCrystalline solid + 12NO↑Gas + 28MnO2Crystalline solid + Fe2O3Crystalline 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
−5980.6−6188.0778.7–
−2990.3−3094.0389.4–
−213.59−221.0027.81–
−498.38−515.6764.89–
per 1 mol of
−1196.1−1237.6155.7–
per 1 mol of
−498.38−515.6764.89–
−213.59−221.0027.81–
per 1 mol of
−5980.6−6188.0778.7–

Changes in standard condition (2)

Reaction of potassium hexacyanidoferrate(III) and potassium permanganate
2K3[Fe(CN)6]Crystalline solid + 28KMnO4Crystalline solid
⟶
12K2CO3Crystalline solid + 5K2OCrystalline solid + 12NO↑Gas + 28MnO2Amorphous solidprecipitated + Fe2O3Crystalline 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
−5489.7–––
−2744.8–––
−196.06–––
−457.47–––
per 1 mol of
−1097.9–––
per 1 mol of
−457.47–––
−196.06–––
per 1 mol of
−5489.7–––

Changes in aqueous solution

Reaction of potassium hexacyanidoferrate(III) and potassium permanganate
◆
ΔrG−6775.5 kJ/mol
K1.04 × 101187
pK−1187.02
2K3[Fe(CN)6]Ionized aqueous solution + 28KMnO4Ionized aqueous solution
⟶
12K2CO3Ionized aqueous solution + 5K2OCrystalline solid + 12NO↑Gas + 28MnO2Crystalline solid + Fe2O3Crystalline 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
−7675.1−6775.5−3029.6–
−3837.6−3387.8−1514.8–
−274.11−241.98−108.20–
−639.59−564.63−252.47–
per 1 mol of
−1535.0−1355.1−605.92–
per 1 mol of
−639.59−564.63−252.47–
−274.11−241.98−108.20–
per 1 mol of
−7675.1−6775.5−3029.6–

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
K3[Fe(CN)6] (cr)-249.8[1]-129.6[1]426.06[1]–
K3[Fe(CN)6] (ai)-195.4[1]-120.4[1]577.8[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
K2CO3 (cr)-1151.02[1]-1063.5[1]155.52[1]114.43[1]
K2CO3 (ai)-1181.90[1]-1094.36[1]148.1[1]–
K2CO3 (cr)
1.5 hydrate
-1609.2[1]-1432.5[1]203.3[1]–
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]–––
NO (g)90.25[1]86.55[1]210.761[1]29.844[1]
MnO2 (cr)-520.03[1]-465.14[1]53.05[1]54.14[1]
MnO2 (am)
precipitated
-502.5[1]–––
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (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