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Na4[Fe(CN)6] + 18H2O 💧⚡→ 4NaHCO3 + 3N2H4 + FeCO3 + H2CO3 + 9H2

Electrolysis of aqueous sodium hexacyanidoferrate(II) yields sodium hydrogencarbonate, hydrazine, iron(II) carbonate, carbonic acid, and hydrogen (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 oxidizing agent
Miscible with water/Very soluble in water/Soluble in waterReducing agent + H2OOxidizing agent
💧⚡
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na4[Fe(CN)6]Sodium hexacyanidoferrate(II)1
Reducing
Soluble in water
H2OWater18
Oxidizing
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaHCO3Sodium hydrogencarbonate4
Oxidized
N2H4Hydrazine3
Oxidized
FeCO3Iron(II) carbonate1
Oxidized
H2CO3Carbonic acid1
Oxidized
H2Hydrogen9
Reduced

Thermodynamic changes

Changes in aqueous solution (1)

Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent
ΔrG320.8 kJ/mol
K0.63 × 10−56
pK56.20
Na4[Fe(CN)6]Ionized aqueous solution + 18H2OLiquid
💧⚡
4NaHCO3Ionized aqueous solution + 3N2H4Un-ionized aqueous solution + FeCO3Crystalline solidsiderite + H2CO3Un-ionized aqueous solution + 9H2Gas
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
584.2320.8882
584.2320.8882
per 1 mol of
32.4617.8249.0
146.180.20221
per 1 mol of
194.7106.9294
per 1 mol of
584.2320.8882
per 1 mol of
584.2320.8882
per 1 mol of
64.9135.6498.0

Changes in aqueous solution (2)

Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent
ΔrG479.2 kJ/mol
K0.11 × 10−83
pK83.95
Na4[Fe(CN)6]Ionized aqueous solution + 18H2OLiquid
💧⚡
4NaHCO3Ionized aqueous solution + 3N2H4Un-ionized aqueous solution + FeCO3Crystalline solidsiderite + H2CO3Un-ionized aqueous solution + 9H2Un-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
546.4479.24899
546.4479.24899
per 1 mol of
30.3626.62272.2
136.6119.81225
per 1 mol of
182.1159.71633
per 1 mol of
546.4479.24899
per 1 mol of
546.4479.24899
per 1 mol of
60.7153.24544.3

Changes in aqueous solution (3)

Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent
ΔrG316.6 kJ/mol
K0.34 × 10−55
pK55.47
Na4[Fe(CN)6]Ionized aqueous solution + 18H2OLiquid
💧⚡
4NaHCO3Un-ionized aqueous solution + 3N2H4Un-ionized aqueous solution + FeCO3Crystalline solidsiderite + H2CO3Un-ionized aqueous solution + 9H2Gas
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
537.1316.6736
537.1316.6736
per 1 mol of
29.8417.5940.9
134.379.15184
per 1 mol of
179.0105.5245
per 1 mol of
537.1316.6736
per 1 mol of
537.1316.6736
per 1 mol of
59.6835.1881.8

Changes in aqueous solution (4)

Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent
ΔrG475.0 kJ/mol
K0.61 × 10−83
pK83.22
Na4[Fe(CN)6]Ionized aqueous solution + 18H2OLiquid
💧⚡
4NaHCO3Un-ionized aqueous solution + 3N2H4Un-ionized aqueous solution + FeCO3Crystalline solidsiderite + H2CO3Un-ionized aqueous solution + 9H2Un-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
499.3475.04753
499.3475.04753
per 1 mol of
27.7426.39264.1
124.8118.81188
per 1 mol of
166.4158.31584
per 1 mol of
499.3475.04753
per 1 mol of
499.3475.04753
per 1 mol of
55.4852.78528.1

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]
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
NaHCO3 (cr)-950.81[1]-851.0[1]101.7[1]87.61[1]
NaHCO3 (ai)-932.11[1]-848.66[1]150.2[1]
NaHCO3 (ao)-943.9[1]-849.7[1]113.8[1]
N2H4 (l)50.63[1]149.34[1]121.21[1]98.87[1]
N2H4 (g)95.40[1]159.35[1]238.47[1]49.58[1]
N2H4 (ao)34.31[1]128.1[1]138[1]
FeCO3 (cr)
siderite
-740.57[1]-666.67[1]92.9[1]82.13[1]
H2CO3 (ao)-699.65[1]-623.08[1]187.4[1]
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid, (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)