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  3. 2K3[Fe(CN)6] + 6H2O 💧⚡→ 6KCN + 2Fe + 3NH4NO2 + 6C

2K3[Fe(CN)6] + 6H2O 💧⚡→ 6KCN + 2Fe + 3NH4NO2 + 6C

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Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
2K3[Fe(CN)6]Potassium hexacyanidoferrate(III) + 6H2OWater
💧⚡
⟶
6KCNPotassium cyanide + 2FeIron + 3NH4NO2Ammonium nitrite + 6CCarbon

Electrolysis of aqueous potassium hexacyanidoferrate(III) yields potassium cyanide, iron, ammonium nitrite, and carbon (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

Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
2K3[Fe(CN)6]Potassium hexacyanidoferrate(III) + 6H2OWater
💧⚡
⟶
6KCNPotassium cyanide + 2FeIron + 3NH4NO2Ammonium nitrite + 6CCarbon

General equation

Electrolysis of aqueous solution with water as non redox agent
Miscible with water/Very soluble in water/Soluble in waterSelf redox agent + H2ONon-redox agent
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⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
K3[Fe(CN)6]Potassium hexacyanidoferrate(III)2
Self redox agent
Very soluble in water
H2OWater6
–
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
KCNPotassium cyanide6
–
–
FeIron2
Reduced
–
NH4NO2Ammonium nitrite3
Oxidized
–
CCarbon6
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
2K3[Fe(CN)6]Crystalline solid + 6H2OLiquid
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⟶
6KCNCrystalline solid + 2FeCrystalline solid + 3NH4NO2Crystalline solid + 6CCrystalline solidgraphite
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
767.1–––
383.6–––
per 1 mol of
127.9–––
per 1 mol of
127.9–––
per 1 mol of
383.6–––
per 1 mol of
255.7–––
per 1 mol of
127.9–––

Changes in standard condition (2)

Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
2K3[Fe(CN)6]Crystalline solid + 6H2OLiquid
💧⚡
⟶
6KCNCrystalline solid + 2FeCrystalline solid + 3NH4NO2Crystalline solid + 6CCrystalline soliddiamond
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
778.5–––
389.3–––
per 1 mol of
129.8–––
per 1 mol of
129.8–––
per 1 mol of
389.3–––
per 1 mol of
259.5–––
per 1 mol of
129.8–––

Changes in aqueous solution

Electrolysis of aqueous potassium hexacyanidoferrate(III) with water as non-redox agent
◆
ΔrG663.4 kJ/mol
K0.60 × 10−116
pK116.22
2K3[Fe(CN)6]Ionized aqueous solution + 6H2OLiquid
💧⚡
⟶
6KCNIonized aqueous solution + 2FeCrystalline solid + 3NH4NO2Ionized aqueous solution + 6CCrystalline solidgraphite
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
784.0663.4402.7–
392.0331.7201.3–
per 1 mol of
130.7110.667.12–
per 1 mol of
130.7110.667.12–
per 1 mol of
392.0331.7201.3–
per 1 mol of
261.3221.1134.2–
per 1 mol of
130.7110.667.12–

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]–
H2O (cr)––––
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas

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
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]–
Fe (cr)0[1]0[1]27.28[1]25.10[1]
Fe (g)416.3[1]370.7[1]180.490[1]25.677[1]
NH4NO2 (cr)-256.5[1]–––
NH4NO2 (ai)-237.2[1]-111.6[1]236.4[1]-17.6[1]
C (cr)
graphite
0[1]0[1]5.740[1]8.527[1]
C (cr)
diamond
1.895[1]2.900[1]2.377[1]6.113[1]
C (g)716.682[1]671.257[1]158.096[1]20.838[1]
* (cr):Crystalline solid, (g):Gas, (ai):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)