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CaF2 + 2HBr 🔥→ CaBr2 + 2HF

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Reaction of calcium fluoride and hydrogen bromide
CaF2Calcium fluoride + 2HBrHydrogen bromide
🔥
⟶
CaBr2Calcium bromide + 2HFHydrogen fluoride

The reaction of calcium fluoride and hydrogen bromide yields calcium bromide and hydrogen 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 calcium fluoride and hydrogen bromide
CaF2Calcium fluoride + 2HBrHydrogen bromide
🔥
⟶
CaBr2Calcium bromide + 2HFHydrogen fluoride

General equation

Reaction of salt of weak acid and strong acid with generating weak acid
Salt of weak acidBrønsted base + Strong acidBrønsted acid
⟶
Salt of strong acidConjugate base + Weak acidConjugate acid

Oxidation state of each atom

Reaction of calcium fluoride and hydrogen bromide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CaF2Calcium fluoride1
Brønsted base
Salt of weak acid
HBrHydrogen bromide2
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
CaBr2Calcium bromide1
Conjugate base
Salt of strong acid
HFHydrogen fluoride2
Conjugate acid
Weak acid

Thermodynamic changes

Changes in standard condition

Reaction of calcium fluoride and hydrogen bromide
◆
ΔrG64.2 kJ/mol
K0.57 × 10−11
pK11.25
CaF2Crystalline solid + 2HBrGas
🔥
⟶
CaBr2Crystalline solid + 2HFGas
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
67.464.211–
per 1 mol of
67.464.211–
per 1 mol of
33.732.15.5–
per 1 mol of
67.464.211–
per 1 mol of
33.732.15.5–

Changes in aqueous solution (1)

Reaction of calcium fluoride and hydrogen bromide
◆
ΔrG67.3 kJ/mol
K0.16 × 10−11
pK11.79
CaF2Crystalline solid + 2HBrIonized aqueous solution
🔥
⟶
CaBr2Ionized aqueous solution + 2HFGas
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
134.667.3225.6–
per 1 mol of
134.667.3225.6–
per 1 mol of
67.3033.6112.8–
per 1 mol of
134.667.3225.6–
per 1 mol of
67.3033.6112.8–

Changes in aqueous solution (2)

Reaction of calcium fluoride and hydrogen bromide
◆
ΔrG20.1 kJ/mol
K0.30 × 10−3
pK3.52
CaF2Crystalline solid + 2HBrIonized aqueous solution
🔥
⟶
CaBr2Ionized aqueous solution + 2HFUn-ionized 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
36.620.155.4–
per 1 mol of
36.620.155.4–
per 1 mol of
18.310.127.7–
per 1 mol of
36.620.155.4–
per 1 mol of
18.310.127.7–

Changes in aqueous solution (3)

Reaction of calcium fluoride and hydrogen bromide
◆
ΔrG20.1 kJ/mol
K0.30 × 10−3
pK3.52
CaF2Crystalline solid + 2HBrIonized aqueous solution
🔥
⟶
CaBr2Ionized aqueous solution + 2HFUn-ionized 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
36.620.155.4–
per 1 mol of
36.620.155.4–
per 1 mol of
18.310.127.7–
per 1 mol of
36.620.155.4–
per 1 mol of
18.310.127.7–

Changes in aqueous solution (4)

Reaction of calcium fluoride and hydrogen bromide
◆
ΔrG56.2 kJ/mol
K0.14 × 10−9
pK9.85
CaF2Crystalline solid + 2HBrIonized aqueous solution
🔥
⟶
CaBr2Ionized aqueous solution + 2HFIonized 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
11.556.2−149.6–
per 1 mol of
11.556.2−149.6–
per 1 mol of
5.7528.1−74.80–
per 1 mol of
11.556.2−149.6–
per 1 mol of
5.7528.1−74.80–

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
CaF2 (cr)-1219.6[1]-1167.3[1]68.87[1]67.03[1]
CaF2 (g)-781.6[1]-790.4[1]274.37[1]51.25[1]
CaF2 (ai)-1208.09[1]-1111.15[1]-80.8[1]–
HBr (g)-36.40[1]-53.45[1]198.695[1]29.142[1]
HBr (ai)-121.55[1]-103.96[1]82.4[1]-141.8[1]
* (cr):Crystalline solid, (g):Gas, (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
CaBr2 (cr)-682.8[1]-663.6[1]130[1]–
CaBr2 (g)-398.3[1]–––
CaBr2 (ai)-785.92[1]-761.49[1]111.7[1]–
CaBr2 (cr)
6 hydrate
-2506.2[1]-2152.8[1]410[1]–
HF (l)
x denotes undetermined zero point entropy
-299.78[1]–75.40+x[1]–
HF (g)-271.1[1]-273.2[1]173.779[1]29.133[1]
HF (ai)-332.63[1]-278.79[1]-13.8[1]-106.7[1]
HF (ao)-320.08[1]-296.82[1]88.7[1]–
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (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)