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2Na3[Fe(CN)6] + 12H2O 💧⚡→ 6NaCN + Fe2O3 + 3(NH4)2CO3 + 3C

Electrolysis of aqueous sodium hexacyanidoferrate(III) yields sodium cyanide, iron(III) oxide, ammonium carbonate, 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

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
💧⚡
ProductOxidation product + ProductReduction product

Oxidation state of each atom

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

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na3[Fe(CN)6]Sodium hexacyanidoferrate(III)2
Soluble in water
H2OWater12
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaCNSodium cyanide6
Fe2O3Iron(III) oxide1
(NH4)2CO3Ammonium carbonate3
Oxidized
CCarbon3
Reduced

Thermodynamic changes

Changes in aqueous solution

Electrolysis of aqueous sodium hexacyanidoferrate(III) with water as non-redox agent
ΔrG−380.1 kJ/mol
K3.90 × 1066
pK−66.59
2Na3[Fe(CN)6]Ionized aqueous solution + 12H2OLiquid
💧⚡
6NaCNIonized aqueous solution + Fe2O3Crystalline solid + 3(NH4)2CO3Ionized aqueous solution + 3CCrystalline 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
−440.5−380.1−200.6
−220.3−190.1−100.3
per 1 mol of
−36.71−31.68−16.72
per 1 mol of
−73.42−63.35−33.43
per 1 mol of
−440.5−380.1−200.6
per 1 mol of
−146.8−126.7−66.87
per 1 mol of
−146.8−126.7−66.87

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
Na3[Fe(CN)6] (ai)-158.6[1]-56.4[1]447.3[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]
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (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
NaCN (cr)
cubic
-87.49[1]-76.43[1]115.60[1]70.37[1]
NaCN (cr)
orthorhombic
-90.75[1]
NaCN (g)109[1]79.94[1]249.43[1]51.17[1]
NaCN (ai)-89.5[1]-89.5[1]153.1[1]
NaCN (cr)
1/2 hydrate
-235.77[1]
NaCN (cr)
2 hydrate
-679.77[1]
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[1]
(NH4)2CO3 (ai)-942.15[1]-686.42[1]169.9[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)