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2AgF + Na4[Fe(CN)6] 💧→ 2AgCN↓ + FeF2↓ + 4NaCN

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Reaction of silver(I) fluoride and sodium hexacyanidoferrate(II)
2AgFSilver(I) fluoride + Na4[Fe(CN)6]Sodium hexacyanidoferrate(II)
💧
⟶
2AgCN↓Silver(I) cyanide + FeF2↓Iron(II) fluoride + 4NaCNSodium cyanide

The reaction of silver(I) fluoride and sodium hexacyanidoferrate(II) yields silver(I) cyanide, iron(II) fluoride, and sodium cyanide (Other reactions are here). This reaction is an acid-base 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

Reaction of silver(I) fluoride and sodium hexacyanidoferrate(II)
2AgFSilver(I) fluoride + Na4[Fe(CN)6]Sodium hexacyanidoferrate(II)
💧
⟶
2AgCN↓Silver(I) cyanide + FeF2↓Iron(II) fluoride + 4NaCNSodium cyanide

General equation

Precipitation reaction
Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base
💧
⟶
Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)

Oxidation state of each atom

Reaction of silver(I) fluoride and sodium hexacyanidoferrate(II)

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
AgFSilver(I) fluoride2
Lewis acid
Very soluble in water
Na4[Fe(CN)6]Sodium hexacyanidoferrate(II)1
Lewis base
Soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
AgCNSilver(I) cyanide2
Lewis conjugate
Insoluble in water
FeF2Iron(II) fluoride1
Lewis conjugate
Slightly soluble in water
NaCNSodium cyanide4
Non-redox product
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of silver(I) fluoride and sodium hexacyanidoferrate(II)
2AgFIonized aqueous solution + Na4[Fe(CN)6]Ionized aqueous solution
💧
⟶
2AgCN↓Crystalline solid + FeF2↓Aqueous solution + 4NaCNIonized 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
48.3–––
per 1 mol of
24.1–––
48.3–––
per 1 mol of
24.1–––
per 1 mol of
48.3–––
per 1 mol of
12.1–––

Changes in aqueous solution (2)

Reaction of silver(I) fluoride and sodium hexacyanidoferrate(II)
◆
ΔrG−48.1 kJ/mol
K2.67 × 108
pK−8.43
2AgFIonized aqueous solution + Na4[Fe(CN)6]Ionized aqueous solution
💧
⟶
2AgCN↓Crystalline solid + FeF2↓Crystalline solid + 4NaCNIonized 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
82.2−48.1419.4–
per 1 mol of
41.1−24.1209.7–
82.2−48.1419.4–
per 1 mol of
41.1−24.1209.7–
per 1 mol of
82.2−48.1419.4–
per 1 mol of
20.6−12.0104.8–

Changes in aqueous solution (3)

Reaction of silver(I) fluoride and sodium hexacyanidoferrate(II)
2AgFUn-ionized aqueous solution + Na4[Fe(CN)6]Ionized aqueous solution
💧
⟶
2AgCN↓Crystalline solid + FeF2↓Aqueous solution + 4NaCNIonized 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
72.0–––
per 1 mol of
36.0–––
72.0–––
per 1 mol of
36.0–––
per 1 mol of
72.0–––
per 1 mol of
18.0–––

Changes in aqueous solution (4)

Reaction of silver(I) fluoride and sodium hexacyanidoferrate(II)
◆
ΔrG−44.1 kJ/mol
K5.32 × 107
pK−7.73
2AgFUn-ionized aqueous solution + Na4[Fe(CN)6]Ionized aqueous solution
💧
⟶
2AgCN↓Crystalline solid + FeF2↓Crystalline solid + 4NaCNIonized 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
105.9−44.1485.6–
per 1 mol of
52.95−22.1242.8–
105.9−44.1485.6–
per 1 mol of
52.95−22.1242.8–
per 1 mol of
105.9−44.1485.6–
per 1 mol of
26.48−11.0121.4–

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
AgF (cr)-204.6[1]–––
AgF (ai)-227.07[1]-201.69[1]59.0[1]-84.9[1]
AgF (ao)-238.9[1]-203.7[1]25.9[1]–
AgF (cr)
2 hydrate
-800.8[1]-671.0[1]174.9[1]130[1]
AgF (cr)
4 hydrate
-1388.3[1]-1147.0[1]268[1]209[1]
Na4[Fe(CN)6] (ai)-505.0[1]-352.53[1]331.0[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-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
AgCN (cr)96.2[1]111.3[1]84.5[1]–
FeF2 (cr)-711.3[1]-668.6[1]86.99[1]68.12[1]
FeF2 (ai)-754.4[1]-636.48[1]-165.3[1]–
FeF2 (aq)-745.2[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]–––
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (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)