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AgF + RbBr 💧→ AgBr↓ + RbF

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Reaction of silver(I) fluoride and rubidium bromide
AgFSilver(I) fluoride + RbBrRubidium bromide
💧
⟶
AgBr↓Silver(I) bromide + RbFRubidium fluoride

The reaction of silver(I) fluoride and rubidium bromide yields silver(I) bromide and rubidium 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

Reaction of silver(I) fluoride and rubidium bromide
AgFSilver(I) fluoride + RbBrRubidium bromide
💧
⟶
AgBr↓Silver(I) bromide + RbFRubidium fluoride

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 rubidium bromide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
AgFSilver(I) fluoride1
Lewis acid
Very soluble in water
RbBrRubidium bromide1
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
AgBrSilver(I) bromide1
Lewis conjugate
Insoluble in water
RbFRubidium fluoride1
Non-redox product
–

Thermodynamic changes

Changes in standard condition

Reaction of silver(I) fluoride and rubidium bromide
AgFCrystalline solid + RbBrCrystalline solid
💧
⟶
AgBr↓Crystalline solid + RbFCrystalline 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
−58.9–––
per 1 mol of
−58.9–––
per 1 mol of
−58.9–––
per 1 mol of
−58.9–––
per 1 mol of
−58.9–––

Changes in aqueous solution (1)

Reaction of silver(I) fluoride and rubidium bromide
◆
ΔrG0.00 kJ/mol
K1.00 × 100
pK0.00
AgFIonized aqueous solution + RbBrIonized aqueous solution
💧
⟶
AgBr↓Ionized aqueous solution + RbFIonized 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
0.010.00−0.2–
per 1 mol of
0.01000.00−0.20–
per 1 mol of
0.01000.00−0.20–
per 1 mol of
0.01000.00−0.20–
per 1 mol of
0.01000.00−0.20–

Changes in aqueous solution (2)

Reaction of silver(I) fluoride and rubidium bromide
◆
ΔrG−24.1 kJ/mol
K1.67 × 104
pK−4.22
AgFIonized aqueous solution + RbBrIonized aqueous solution
💧
⟶
AgBr↓Un-ionized aqueous solution + RbFIonized 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
–−24.1––
per 1 mol of
–−24.1––
per 1 mol of
–−24.1––
per 1 mol of
–−24.1––
per 1 mol of
–−24.1––

Changes in aqueous solution (3)

Reaction of silver(I) fluoride and rubidium bromide
◆
ΔrG2.0 kJ/mol
K0.45 × 100
pK0.35
AgFUn-ionized aqueous solution + RbBrIonized aqueous solution
💧
⟶
AgBr↓Ionized aqueous solution + RbFIonized 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
11.82.032.9–
per 1 mol of
11.82.032.9–
per 1 mol of
11.82.032.9–
per 1 mol of
11.82.032.9–
per 1 mol of
11.82.032.9–

Changes in aqueous solution (4)

Reaction of silver(I) fluoride and rubidium bromide
◆
ΔrG−22.1 kJ/mol
K7.44 × 103
pK−3.87
AgFUn-ionized aqueous solution + RbBrIonized aqueous solution
💧
⟶
AgBr↓Un-ionized aqueous solution + RbFIonized 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
–−22.1––
per 1 mol of
–−22.1––
per 1 mol of
–−22.1––
per 1 mol of
–−22.1––
per 1 mol of
–−22.1––

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]
RbBr (cr)-394.59[1]-381.79[1]109.96[1]52.84[1]
RbBr (g)-182.8[1]-215.1[1]261.02[1]37.20[1]
RbBr (ai)-372.71[1]-387.94[1]203.93[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (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
AgBr (cr)-100.37[1]-96.90[1]107.1[1]52.38[1]
AgBr (ai)-15.98[1]-26.86[1]155.2[1]-120.1[1]
AgBr (ao)–-51.0[1]––
RbF (cr)-557.7[1]–––
RbF (g)-331.4[1]-349.0[1]237.09[1]35.69[1]
RbF (ai)-583.79[1]-562.77[1]107.5[1]–
RbF (cr)
1.5 hydrate
-1013.8[1]–––
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized 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)