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Na + CsF → NaF + Cs

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Reaction of sodium and caesium fluoride
NaSodium + CsFCaesium fluoride
⟶
NaFSodium fluoride + CsCaesium

The reaction of sodium and caesium fluoride yields sodium fluoride and caesium. This reaction is an oxidation-reduction 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 sodium and caesium fluoride
NaSodium + CsFCaesium fluoride
⟶
NaFSodium fluoride + CsCaesium

General equation

Reaction of reducing species and hardly reducible species
Reducing speciesReducing agent + Hardly reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of sodium and caesium fluoride

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium1
Reducing
Reducing
CsFCaesium fluoride1
Oxidizing
Hardly reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaFSodium fluoride1
Oxidized
–
CsCaesium1
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of sodium and caesium fluoride
◆
ΔrG−18.0 kJ/mol
K1.42 × 103
pK−3.15
NaCrystalline solid + CsFCrystalline solid
⟶
NaFCrystalline solid + CsCrystalline 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
−20.1−18.0−7.32−0.30
per 1 mol of
−20.1−18.0−7.32−0.300
per 1 mol of
−20.1−18.0−7.32−0.300
per 1 mol of
−20.1−18.0−7.32−0.300
per 1 mol of
−20.1−18.0−7.32−0.300

Changes in aqueous solution

Reaction of sodium and caesium fluoride
◆
ΔrG30.13 kJ/mol
K0.53 × 10−5
pK5.28
NaCrystalline solid + CsFIonized aqueous solution
⟶
NaFIonized aqueous solution + CsCrystalline 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
18.1630.13−40.0–
per 1 mol of
18.1630.13−40.0–
per 1 mol of
18.1630.13−40.0–
per 1 mol of
18.1630.13−40.0–
per 1 mol of
18.1630.13−40.0–

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
Na (cr)0[1]0[1]51.21[1]28.24[1]
Na (g)107.32[1]76.761[1]153.712[1]20.786[1]
CsF (cr)-553.5[1]-525.5[1]92.80[1]51.09[1]
CsF (g)-359.0[1]-375.7[1]243.24[1]35.86[1]
CsF (ai)-590.91[1]-570.81[1]119.2[1]–
CsF (cr)
1.5 hydrate
-1013.8[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
NaF (cr)-573.647[1]-543.494[1]51.46[1]46.86[1]
NaF (g)-291.2[1]-310.5[1]217.59[1]34.221[1]
NaF (ai)-572.75[1]-540.68[1]45.2[1]-60.2[1]
Cs (cr)0[1]0[1]85.23[1]32.17[1]
Cs (g)76.065[1]49.121[1]175.595[1]20.786[1]
* (cr):Crystalline solid, (g):Gas, (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)