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Na4[Fe(CN)6] + 18H2O 💧⚡→ 2Na2CO3 + 6NO↑ + FeCO3 + 3CO↑ + 18H2

Electrolysis of aqueous sodium hexacyanidoferrate(II) yields sodium carbonate, nitrogen monoxide, iron(II) carbonate, carbon monoxide, 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
Na2CO3Sodium carbonate2
Oxidized
NONitrogen monoxide6
Oxidized
FeCO3Iron(II) carbonate1
Oxidized
COCarbon monoxide3
H2Hydrogen18
Reduced

Thermodynamic changes

Changes in aqueous solution (1)

Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent
ΔrG1958.70 kJ/mol
K0.71 × 10−343
pK343.15
Na4[Fe(CN)6]Ionized aqueous solution + 18H2OLiquid
💧⚡
2Na2CO3Ionized aqueous solution + 6NOGas + FeCO3Crystalline solidsiderite + 3COGas + 18H2Gas
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
2804.51958.702835.6
2804.51958.702835.6
per 1 mol of
155.81108.817157.53
per 1 mol of
1402.3979.3501417.8
per 1 mol of
467.42326.450472.60
per 1 mol of
2804.51958.702835.6
per 1 mol of
934.83652.900945.20
per 1 mol of
155.81108.817157.53

Changes in aqueous solution (2)

Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent
ΔrG2275.5 kJ/mol
K0.22 × 10−398
pK398.65
Na4[Fe(CN)6]Ionized aqueous solution + 18H2OLiquid
💧⚡
2Na2CO3Ionized aqueous solution + 6NOGas + FeCO3Crystalline solidsiderite + 3COGas + 18H2Un-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
2728.92275.510869
2728.92275.510869
per 1 mol of
151.61126.42603.83
per 1 mol of
1364.51137.85434.5
per 1 mol of
454.82379.251811.5
per 1 mol of
2728.92275.510869
per 1 mol of
909.63758.503623.0
per 1 mol of
151.61126.42603.83

Changes in aqueous solution (3)

Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent
ΔrG2010.50 kJ/mol
K0.60 × 10−352
pK352.22
Na4[Fe(CN)6]Ionized aqueous solution + 18H2OLiquid
💧⚡
2Na2CO3Ionized aqueous solution + 6NOGas + FeCO3Crystalline solidsiderite + 3COUn-ionized aqueous solution + 18H2Gas
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
2773.22010.502556.4
2773.22010.502556.4
per 1 mol of
154.07111.694142.02
per 1 mol of
1386.61005.251278.2
per 1 mol of
462.20335.083426.07
per 1 mol of
2773.22010.502556.4
per 1 mol of
924.40670.167852.13
per 1 mol of
154.07111.694142.02

Changes in aqueous solution (4)

Electrolysis of aqueous sodium hexacyanidoferrate(II) with water as oxidizing agent
ΔrG2327.3 kJ/mol
K0.19 × 10−407
pK407.73
Na4[Fe(CN)6]Ionized aqueous solution + 18H2OLiquid
💧⚡
2Na2CO3Ionized aqueous solution + 6NOGas + FeCO3Crystalline solidsiderite + 3COUn-ionized aqueous solution + 18H2Un-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
2697.62327.310590
2697.62327.310590
per 1 mol of
149.87129.29588.33
per 1 mol of
1348.81163.75295.0
per 1 mol of
449.60387.881765.0
per 1 mol of
2697.62327.310590
per 1 mol of
899.20775.773530.0
per 1 mol of
149.87129.29588.33

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
Na2CO3 (cr)-1130.68[1]-1044.44[1]134.98[1]112.30[1]
Na2CO3 (ai)-1157.38[1]-1051.64[1]61.1[1]
Na2CO3 (cr)
1 hydrate
-1431.26[1]-1285.31[1]168.11[1]145.60[1]
Na2CO3 (cr)
7 hydrate
-3199.96[1]-2714.2[1]422.2[1]
Na2CO3 (cr)
10 hydrate
-4081.32[1]-3427.66[1]562.7[1]550.32[1]
NO (g)90.25[1]86.55[1]210.761[1]29.844[1]
FeCO3 (cr)
siderite
-740.57[1]-666.67[1]92.9[1]82.13[1]
CO (g)-110.525[1]-137.168[1]197.674[1]29.142[1]
CO (ao)-120.96[1]-119.90[1]104.6[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, (g):Gas, (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)