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  3. 2K3[Fe(CN)6] + 6KMnO4 → 4KNO2 + 8KCN + 3Mn2O3 + Fe2O3 + 4CO↑

2K3[Fe(CN)6] + 6KMnO4 → 4KNO2 + 8KCN + 3Mn2O3 + Fe2O3 + 4CO↑

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Reaction of potassium hexacyanidoferrate(III) and potassium permanganate
2K3[Fe(CN)6]Potassium hexacyanidoferrate(III) + 6KMnO4Potassium permanganate
⟶
4KNO2Potassium nitrite + 8KCNPotassium cyanide + 3Mn2O3Manganese(III) oxide + Fe2O3Iron(III) oxide + 4CO↑Carbon monoxide

The reaction of potassium hexacyanidoferrate(III) and potassium permanganate yields potassium nitrite, potassium cyanide, manganese(III) oxide, iron(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(III) and potassium permanganate
2K3[Fe(CN)6]Potassium hexacyanidoferrate(III) + 6KMnO4Potassium permanganate
⟶
4KNO2Potassium nitrite + 8KCNPotassium cyanide + 3Mn2O3Manganese(III) oxide + Fe2O3Iron(III) oxide + 4CO↑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(III) and potassium permanganate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
K3[Fe(CN)6]Potassium hexacyanidoferrate(III)2
Reducing
Reducing
KMnO4Potassium permanganate6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
KNO2Potassium nitrite4
Oxidized
–
KCNPotassium cyanide8
–
–
Mn2O3Manganese(III) oxide3
Reduced
–
Fe2O3Iron(III) oxide1
–
–
COCarbon monoxide4
–
–

Thermodynamic changes

Changes in standard condition

Reaction of potassium hexacyanidoferrate(III) and potassium permanganate
◆
ΔrG−1290.5 kJ/mol
K1.22 × 10226
pK−226.09
2K3[Fe(CN)6]Crystalline solid + 6KMnO4Crystalline solid
⟶
4KNO2Crystalline solidrhombic + 8KCNCrystalline solid + 3Mn2O3Crystalline solid + Fe2O3Crystalline solid + 4CO↑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
−1003.8−1290.5963.5–
−501.90−645.25481.8–
−167.30−215.08160.6–
per 1 mol of
−250.95−322.63240.9–
per 1 mol of
−125.47−161.31120.4–
−334.60−430.17321.2–
per 1 mol of
−1003.8−1290.5963.5–
per 1 mol of
−250.95−322.63240.9–

Changes in aqueous solution (1)

Reaction of potassium hexacyanidoferrate(III) and potassium permanganate
◆
ΔrG−1459.2 kJ/mol
K4.37 × 10255
pK−255.64
2K3[Fe(CN)6]Ionized aqueous solution + 6KMnO4Ionized aqueous solution
⟶
4KNO2Ionized aqueous solution + 8KCNIonized aqueous solution + 3Mn2O3Crystalline solid + Fe2O3Crystalline solid + 4CO↑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
−1230.9−1459.2766.6–
−615.45−729.60383.3–
−205.15−243.20127.8–
per 1 mol of
−307.73−364.80191.7–
per 1 mol of
−153.86−182.4095.83–
−410.30−486.40255.5–
per 1 mol of
−1230.9−1459.2766.6–
per 1 mol of
−307.73−364.80191.7–

Changes in aqueous solution (2)

Reaction of potassium hexacyanidoferrate(III) and potassium permanganate
◆
ΔrG−1390.1 kJ/mol
K3.43 × 10243
pK−243.53
2K3[Fe(CN)6]Ionized aqueous solution + 6KMnO4Ionized aqueous solution
⟶
4KNO2Ionized aqueous solution + 8KCNIonized aqueous solution + 3Mn2O3Crystalline solid + Fe2O3Crystalline solid + 4CO↑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
−1272.6−1390.1394.3–
−636.30−695.05197.2–
−212.10−231.6865.72–
per 1 mol of
−318.15−347.5298.58–
per 1 mol of
−159.07−173.7649.29–
−424.20−463.37131.4–
per 1 mol of
−1272.6−1390.1394.3–
per 1 mol of
−318.15−347.5298.58–

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
KNO2 (cr)
rhombic
-369.82[1]-306.55[1]152.09[1]107.40[1]
KNO2 (ai)-356.9[1]-315.4[1]225.5[1]–
KCN (cr)-113.0[1]-101.86[1]128.49[1]66.27[1]
KCN (g)90.8[1]64.17[1]261.90[1]52.34[1]
KCN (ai)-101.7[1]-110.9[1]196.6[1]–
Mn2O3 (cr)-959.0[1]-881.1[1]110.5[1]107.65[1]
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[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, (ai):Ionized aqueous solution, (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)