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2Na + HgF2 → 2NaF + Hg

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Reaction of sodium and mercury(II) fluoride
2NaSodium + HgF2Mercury(II) fluoride
⟶
2NaFSodium fluoride + HgMercury

The reaction of sodium and mercury(II) fluoride yields sodium fluoride and mercury. 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 mercury(II) fluoride
2NaSodium + HgF2Mercury(II) fluoride
⟶
2NaFSodium fluoride + HgMercury

General equation

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

Oxidation state of each atom

Reaction of sodium and mercury(II) fluoride

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium2
Reducing
Reducing
HgF2Mercury(II) fluoride1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaFSodium fluoride2
Oxidized
–
HgMercury1
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of sodium and mercury(II) fluoride
◆
ΔrG−908.4 kJ/mol
K1.40 × 10159
pK−159.14
2NaCrystalline solid + HgF2Solid
⟶
2NaFCrystalline solid + HgLiquid
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
−923.0−908.4−69.5–
per 1 mol of
−461.5−454.2−34.8–
per 1 mol of
Mercury(II) fluoride
−923.0−908.4−69.5–
per 1 mol of
−461.5−454.2−34.8–
per 1 mol of
−923.0−908.4−69.5–

Changes in aqueous solution

Reaction of sodium and mercury(II) fluoride
◆
ΔrG−863.5 kJ/mol
K1.90 × 10151
pK−151.28
2NaCrystalline solid + HgF2Solid
⟶
2NaFIonized aqueous solution + HgUn-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
−883.5−863.5−87–
per 1 mol of
−441.8−431.8−44–
per 1 mol of
Mercury(II) fluoride
−883.5−863.5−87–
per 1 mol of
−441.8−431.8−44–
per 1 mol of
−883.5−863.5−87–

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]
HgF2 (s)-224.3-178.6146.0–
* (cr):Crystalline solid, (g):Gas, (s):Solid

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]
Hg (cr)––––
Hg (l)0[1]0[1]76.02[1]27.983[1]
Hg (g)61.317[1]31.820[1]174.96[1]20.786[1]
Hg (ao)37.7[1]39.3[1]71[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)