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2AgF + (NH4)2SO4 💧→ Ag2SO4↓ + 2NH4F

The reaction of silver(I) fluoride and ammonium sulfate yields silver(I) sulfate and ammonium fluoride. 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 categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
AgFSilver(I) fluoride2
Lewis acid
Very soluble in water
(NH4)2SO4Ammonium sulfate1
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Ag2SO4Silver(I) sulfate1
Lewis conjugate
Slightly soluble in water
NH4FAmmonium fluoride2
Non-redox product

Thermodynamic changes

Changes in standard condition

Reaction of silver(I) fluoride and ammonium sulfate
2AgFCrystalline solid + (NH4)2SO4Crystalline solid
💧
Ag2SO4Crystalline solid + 2NH4FCrystalline solid
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
−53.8
per 1 mol of
−26.9
per 1 mol of
−53.8
per 1 mol of
−53.8
per 1 mol of
−26.9

Changes in aqueous solution (1)

Reaction of silver(I) fluoride and ammonium sulfate
ΔrG0.04 kJ/mol
K0.98 × 100
pK0.01
2AgFIonized aqueous solution + (NH4)2SO4Ionized aqueous solution
💧
Ag2SO4Ionized aqueous solution + 2NH4FIonized 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
0.040.040.0−2
per 1 mol of
0.02000.02000.0−1
per 1 mol of
0.04000.04000.0−2
per 1 mol of
0.04000.04000.0−2
per 1 mol of
0.02000.02000.0−1

Changes in aqueous solution (2)

Reaction of silver(I) fluoride and ammonium sulfate
ΔrG4.1 kJ/mol
K0.19 × 100
pK0.72
2AgFUn-ionized aqueous solution + (NH4)2SO4Ionized aqueous solution
💧
Ag2SO4Ionized aqueous solution + 2NH4FIonized 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
23.74.166.2
per 1 mol of
11.82.033.1
per 1 mol of
23.74.166.2
per 1 mol of
23.74.166.2
per 1 mol of
11.82.033.1

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
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]
(NH4)2SO4 (cr)-1180.85[1]-901.67[1]220.1[1]187.49[1]
(NH4)2SO4 (ai)-1174.28[1]-903.14[1]246.9[1]-133.1[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
Ag2SO4 (cr)-715.88[1]-618.41[1]200.4[1]131.38[1]
Ag2SO4 (ai)-698.10[1]-590.30[1]165.7[1]-251[1]
NH4F (cr)-463.96[1]-348.68[1]71.96[1]65.27[1]
NH4F (ai)-465.14[1]-358.09[1]99.6[1]-26.8[1]
* (cr):Crystalline solid, (ai):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)