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3H2 + Na4[Fe(CN)6] → Fe + 4NaCN + 2NH3 + 2C

The reaction of hydrogen and sodium hexacyanidoferrate(II) yields iron, sodium cyanide, ammonia, 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

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2Hydrogen3
Reducing
Reducing
Na4[Fe(CN)6]Sodium hexacyanidoferrate(II)1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
FeIron1
Reduced
NaCNSodium cyanide4
NH3Ammonia2
Oxidized
CCarbon2
Reduced

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of hydrogen and sodium hexacyanidoferrate(II)
ΔrG−91.2 kJ/mol
K9.50 × 1015
pK−15.98
3H2Un-ionized aqueous solution + Na4[Fe(CN)6]Ionized aqueous solution
FeCrystalline solid + 4NaCNIonized aqueous solution + 2NH3Gas + 2CCrystalline 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
67.4−91.2−1026
per 1 mol of
22.5−30.4−342.0
67.4−91.2−1026
per 1 mol of
67.4−91.2−1026
per 1 mol of
16.9−22.8−256.5
per 1 mol of
33.7−45.6−513.0
per 1 mol of
33.7−45.6−513.0

Changes in aqueous solution (2)

Reaction of hydrogen and sodium hexacyanidoferrate(II)
ΔrG−111.3 kJ/mol
K3.15 × 1019
pK−19.50
3H2Un-ionized aqueous solution + Na4[Fe(CN)6]Ionized aqueous solution
FeCrystalline solid + 4NaCNIonized aqueous solution + 2NH3Un-ionized aqueous solution + 2CCrystalline 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
−1.0−111.3−1188
per 1 mol of
−0.33−37.10−396.0
−1.0−111.3−1188
per 1 mol of
−1.0−111.3−1188
per 1 mol of
−0.25−27.82−297.0
per 1 mol of
−0.50−55.65−594.0
per 1 mol of
−0.50−55.65−594.0

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
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]
Na4[Fe(CN)6] (ai)-505.0[1]-352.53[1]331.0[1]
* (g):Gas, (ao):Un-ionized aqueous solution, (ai):Ionized aqueous solution

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
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]
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]
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[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, (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)