You-iggy

ZnBr2 + 2KF 💧→ ZnF2↓ + 2KBr

The reaction of zinc bromide and potassium fluoride yields zinc fluoride and potassium bromide. 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
ZnBr2Zinc bromide1
Lewis acid
Very soluble in water
KFPotassium fluoride2
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
ZnF2Zinc fluoride1
Lewis conjugate
Slightly soluble in water
KBrPotassium bromide2
Non-redox product

Thermodynamic changes

Changes in standard condition

Reaction of zinc bromide and potassium fluoride
ΔrG−87.0 kJ/mol
K1.74 × 1015
pK−15.24
ZnBr2Crystalline solid + 2KFCrystalline solid
💧
ZnF2Crystalline solid + 2KBrCrystalline 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
−88.8−87.0−6.2
per 1 mol of
−88.8−87.0−6.2
per 1 mol of
−44.4−43.5−3.1
per 1 mol of
−88.8−87.0−6.2
per 1 mol of
−44.4−43.5−3.1

Changes in aqueous solution (1)

Reaction of zinc bromide and potassium fluoride
ΔrG−8.7 kJ/mol
K3.34 × 101
pK−1.52
ZnBr2Ionized aqueous solution + 2KFIonized aqueous solution
💧
ZnF2Crystalline solid + 2KBrIonized 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
54.8−8.7213.4233
per 1 mol of
54.8−8.7213.4233
per 1 mol of
27.4−4.3106.7117
per 1 mol of
54.8−8.7213.4233
per 1 mol of
27.4−4.3106.7117

Changes in aqueous solution (2)

Reaction of zinc bromide and potassium fluoride
ΔrG−14.2 kJ/mol
K3.07 × 102
pK−2.49
ZnBr2Un-ionized aqueous solution + 2KFIonized aqueous solution
💧
ZnF2Crystalline solid + 2KBrIonized 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
−14.2
per 1 mol of
−14.2
per 1 mol of
−7.10
per 1 mol of
−14.2
per 1 mol of
−7.10

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
ZnBr2 (cr)-328.65[1]-312.13[1]138.5[1]
ZnBr2 (ai)-396.98[1]-354.97[1]52.7[1]-238[1]
ZnBr2 (ao)-349.4[1]
ZnBr2 (cr)
2 hydrate
-937.2[1]-799.5[1]198.7[1]
KF (cr)-567.27[1]-537.75[1]66.57[1]49.04[1]
KF (g)-325.43[1]-343.62[1]226.41[1]35.23[1]
KF (ai)-585.01[1]-562.06[1]88.7[1]-84.9[1]
KF (cr)
2 hydrate
-1163.621[1]-1021.49[1]155.2[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
ZnF2 (cr)-764.4[1]-713.3[1]73.68[1]65.65[1]
ZnF2 (ai)-819.14[1]-704.64[1]-139.7[1]-167[1]
KBr (cr)-393.798[1]-380.66[1]95.90[1]52.30[1]
KBr (g)-180.08[1]-212.96[1]250.52[1]36.920[1]
KBr (ai)-373.92[1]-387.23[1]184.9[1]-120.1[1]
* (cr):Crystalline solid, (ai):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)