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9Na4[Fe(CN)6] + 39KMnO4 🔥→ 36NaMnO4 + 5K3[Fe(CN)6] + 2Fe2O3 + 3MnO2 + 24KCN

The reaction of sodium hexacyanidoferrate(II) and potassium permanganate yields sodium permanganate, potassium hexacyanidoferrate(III), iron(III) oxide, manganese(IV) oxide, and potassium cyanide (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 reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na4[Fe(CN)6]Sodium hexacyanidoferrate(II)9
Reducing
Reducing
KMnO4Potassium permanganate39
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaMnO4Sodium permanganate36
K3[Fe(CN)6]Potassium hexacyanidoferrate(III)5
Oxidized
Fe2O3Iron(III) oxide2
Oxidized
MnO2Manganese(IV) oxide3
Reduced
KCNPotassium cyanide24

Thermodynamic changes

Changes in aqueous solution

Reaction of sodium hexacyanidoferrate(II) and potassium permanganate
ΔrG−8.7 kJ/mol
K3.34 × 101
pK−1.52
9Na4[Fe(CN)6]Ionized aqueous solution + 39KMnO4Ionized aqueous solution
🔥
36NaMnO4Ionized aqueous solution + 5K3[Fe(CN)6]Ionized aqueous solution + 2Fe2O3Crystalline solid + 3MnO2Crystalline solid + 24KCNIonized 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
739.3−8.72515.3
82.14−0.97279.48
18.96−0.2264.495
20.54−0.2469.869
147.9−1.7503.06
per 1 mol of
369.6−4.31257.7
246.4−2.9838.43
per 1 mol of
30.80−0.36104.80

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
Na4[Fe(CN)6] (ai)-505.0[1]-352.53[1]331.0[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]
* (ai):Ionized aqueous solution, (cr):Crystalline solid

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
NaMnO4 (ai)-781.6[1]-709.1[1]250.2[1]
NaMnO4 (cr)
1 hydrate
-1079.14[1]
NaMnO4 (cr)
3 hydrate
-1672.85[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]
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[1]
MnO2 (cr)-520.03[1]-465.14[1]53.05[1]54.14[1]
MnO2 (am)
precipitated
-502.5[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]
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (am):Amorphous solid, (g):Gas

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)