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  3. 6Na4[Fe(CN)6] + 18H2O ๐Ÿ’งโšกโ†’ 5Na3[Fe(CN)6] + 9NaOH + Fe(OH)3 + 6NOโ†‘ + 6CH4โ†‘

6Na4[Fe(CN)6] + 18H2O ๐Ÿ’งโšกโ†’ 5Na3[Fe(CN)6] + 9NaOH + Fe(OH)3 + 6NOโ†‘ + 6CH4โ†‘

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Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as non-redox agent
6Na4[Fe(CN)6]Sodium hexacyanidoferrate(II) + 18H2OWater
๐Ÿ’งโšก
โŸถ
5Na3[Fe(CN)6]Sodium hexacyanidoferrate(III) + 9NaOHSodium hydroxide + Fe(OH)3Iron(III) hydroxide + 6NOโ†‘Nitrogen monoxide + 6CH4โ†‘Methane

Electrolysis of aqueous sodium hexacyanidoferrate(II) yields sodium hexacyanidoferrate(III), sodium hydroxide, iron(III) hydroxide, nitrogen monoxide, and methane (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 sodium hexacyanidoferrate(II) with water as non-redox agent
6Na4[Fe(CN)6]Sodium hexacyanidoferrate(II) + 18H2OWater
๐Ÿ’งโšก
โŸถ
5Na3[Fe(CN)6]Sodium hexacyanidoferrate(III) + 9NaOHSodium hydroxide + Fe(OH)3Iron(III) hydroxide + 6NOโ†‘Nitrogen monoxide + 6CH4โ†‘Methane

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
๐Ÿ’งโšก
โŸถ
ProductOxidation product + ProductReduction product

Oxidation state of each atom

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

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na4[Fe(CN)6]Sodium hexacyanidoferrate(II)6
Self redox agent
Soluble in water
H2OWater18
โ€“
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na3[Fe(CN)6]Sodium hexacyanidoferrate(III)5
Oxidized
โ€“
NaOHSodium hydroxide9
โ€“
โ€“
Fe(OH)3Iron(III) hydroxide1
Oxidized
โ€“
NONitrogen monoxide6
Oxidized
โ€“
CH4Methane6
Reduced
โ€“

Thermodynamic changes

Changes in aqueous solution (1)

Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as non-redox agent
โ—†
ฮ”rG1884.8 kJ/mol
K0.63 ร— 10โˆ’330
pK330.20
6Na4[Fe(CN)6]Ionized aqueous solution + 18H2OLiquid
๐Ÿ’งโšก
โŸถ
5Na3[Fe(CN)6]Ionized aqueous solution + 9NaOHIonized aqueous solution + Fe(OH)3Un-ionized aqueous solution + 6NOโ†‘Gas + 6CH4โ†‘Gas
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
โ€“1884.8โ€“โ€“
โ€“314.13โ€“โ€“
per 1 mol of
โ€“104.71โ€“โ€“
โ€“376.96โ€“โ€“
per 1 mol of
โ€“209.42โ€“โ€“
โ€“1884.8โ€“โ€“
per 1 mol of
โ€“314.13โ€“โ€“
per 1 mol of
โ€“314.13โ€“โ€“

Changes in aqueous solution (2)

Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as non-redox agent
โ—†
ฮ”rG1983.2 kJ/mol
K0.36 ร— 10โˆ’347
pK347.44
6Na4[Fe(CN)6]Ionized aqueous solution + 18H2OLiquid
๐Ÿ’งโšก
โŸถ
5Na3[Fe(CN)6]Ionized aqueous solution + 9NaOHIonized aqueous solution + Fe(OH)3Un-ionized aqueous solution + 6NOโ†‘Gas + 6CH4โ†‘Un-ionized aqueous solution
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
โ€“1983.2โ€“โ€“
โ€“330.53โ€“โ€“
per 1 mol of
โ€“110.18โ€“โ€“
โ€“396.64โ€“โ€“
per 1 mol of
โ€“220.36โ€“โ€“
โ€“1983.2โ€“โ€“
per 1 mol of
โ€“330.53โ€“โ€“
per 1 mol of
โ€“330.53โ€“โ€“

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ฮ”fHยฐ
kJ ยท molโˆ’1		Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1		Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
Na4[Fe(CN)6] (ai)-505.0[1]-352.53[1]331.0[1]โ€“
H2O (cr)โ€“โ€“โ€“โ€“
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
ฮ”fHยฐ
kJ ยท molโˆ’1		Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1		Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
Na3[Fe(CN)6] (ai)-158.6[1]-56.4[1]447.3[1]โ€“
NaOH (cr)-425.609[1]-379.494[1]64.455[1]59.54[1]
NaOH (g)-207.1[1]-210.0[1]228.43[1]48.37[1]
NaOH (ai)-470.114[1]-419.150[1]48.1[1]-102.1[1]
NaOH (cr)
1 hydrate
-734.543[1]-629.338[1]99.50[1]90.17[1]
NaOH (l)
2 hydrate
-1019.076[1]-873.091[1]195.979[1]239.41[1]
NaOH (l)
3.5 hydrate
-1459.798[1]-1236.356[1]286.089[1]354.43[1]
NaOH (l)
4 hydrate
-1605.15[1]-1356.64[1]318.70[1]โ€“
NaOH (l)
5 hydrate
-1894.31[1]-1596.34[1]386.06[1]โ€“
NaOH (l)
7 hydrate
-2469.02[1]-2073.80[1]526.31[1]โ€“
Fe(OH)3 (cr)
precipitated
-823.0[1]-696.5[1]106.7[1]โ€“
Fe(OH)3 (ao)โ€“-659.3[1]โ€“โ€“
NO (g)90.25[1]86.55[1]210.761[1]29.844[1]
CH4 (g)-74.81[1]-50.72[1]186.264[1]35.309[1]
CH4 (ao)-89.04[1]-34.33[1]83.7[1]โ€“
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (g):Gas, (l):Liquid, (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)