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  3. 4CuF + 2HNO3 + 8H^+ → 4Cu^2+ + N2O3↑ + 4HF↑ + 3H2O

4CuF + 2HNO3 + 8H+ → 4Cu2+ + N2O3↑ + 4HF↑ + 3H2O

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Reaction of copper(I) fluoride and nitric acid under acidic condition
4CuFCopper(I) fluoride + 2HNO3Nitric acid + 8H+Hydrogen ion
⟶
4Cu2+Copper(II) ion + N2O3↑Dinitrogen trioxide + 4HF↑Hydrogen fluoride + 3H2OWater

The reaction of copper(I) fluoride, nitric acid, and hydrogen ion yields copper(II) ion, dinitrogen trioxide, hydrogen fluoride, and water (Other reactions are here). 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 reactions
  5. 5Related categories

Reaction data

Chemical equation

Reaction of copper(I) fluoride and nitric acid under acidic condition
4CuFCopper(I) fluoride + 2HNO3Nitric acid + 8H+Hydrogen ion
⟶
4Cu2+Copper(II) ion + N2O3↑Dinitrogen trioxide + 4HF↑Hydrogen fluoride + 3H2OWater

General equation

Reaction of oxidizable species and oxidizing species under acidic condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent
⟶
ProductOxidation product + ProductReduction product + H2ONon-redox product

Oxidation state of each atom

Reaction of copper(I) fluoride and nitric acid under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuFCopper(I) fluoride4
Reducing
Oxidizable
HNO3Nitric acid2
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion8
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu2+Copper(II) ion4
Oxidized
–
N2O3Dinitrogen trioxide1
Reduced
–
HFHydrogen fluoride4
–
–
H2OWater3
–
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of copper(I) fluoride and nitric acid under acidic condition
◆
ΔrG−140 kJ/mol
K3.36 × 1024
pK−24.53
4CuFSolid + 2HNO3Ionized aqueous solution + 8H+Un-ionized aqueous solution
⟶
4Cu2+Un-ionized aqueous solution + N2O3↑Gas + 4HF↑Gas + 3H2OLiquid
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
−64−140266.3–
per 1 mol of
−16−35.066.58–
per 1 mol of
−32−70.0133.2–
per 1 mol of
Hydrogen ion
−8.0−17.533.29–
per 1 mol of
Copper(II) ion
−16−35.066.58–
−64−140266.3–
per 1 mol of
−16−35.066.58–
per 1 mol of
−21−46.788.77–

Changes in standard condition (2)

Reaction of copper(I) fluoride and nitric acid under acidic condition
◆
ΔrG−235 kJ/mol
K1.48 × 1041
pK−41.17
4CuFSolid + 2HNO3Ionized aqueous solution + 8H+Un-ionized aqueous solution
⟶
4Cu2+Un-ionized aqueous solution + N2O3↑Gas + 4HF↑Un-ionized aqueous solution + 3H2OLiquid
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
−260−235−74.0–
per 1 mol of
−65.0−58.8−18.5–
per 1 mol of
−130−118−37.0–
per 1 mol of
Hydrogen ion
−32.5−29.4−9.25–
per 1 mol of
Copper(II) ion
−65.0−58.8−18.5–
−260−235−74.0–
per 1 mol of
−65.0−58.8−18.5–
per 1 mol of
−86.7−78.3−24.7–

Changes in standard condition (3)

Reaction of copper(I) fluoride and nitric acid under acidic condition
◆
ΔrG−163 kJ/mol
K3.60 × 1028
pK−28.56
4CuFSolid + 2HNO3Ionized aqueous solution + 8H+Un-ionized aqueous solution
⟶
4Cu2+Un-ionized aqueous solution + N2O3↑Gas + 4HF↑Ionized aqueous solution + 3H2OLiquid
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
−310−163−484.0–
per 1 mol of
−77.5−40.8−121.0–
per 1 mol of
−155−81.5−242.0–
per 1 mol of
Hydrogen ion
−38.8−20.4−60.50–
per 1 mol of
Copper(II) ion
−77.5−40.8−121.0–
−310−163−484.0–
per 1 mol of
−77.5−40.8−121.0–
per 1 mol of
−103−54.3−161.3–

Changes in standard condition (4)

Reaction of copper(I) fluoride and nitric acid under acidic condition
◆
ΔrG−235 kJ/mol
K1.48 × 1041
pK−41.17
4CuFSolid + 2HNO3Ionized aqueous solution + 8H+Un-ionized aqueous solution
⟶
4Cu2+Un-ionized aqueous solution + N2O3↑Gas + 4HF↑Un-ionized aqueous solution + 3H2OLiquid
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
−260−235−74.0–
per 1 mol of
−65.0−58.8−18.5–
per 1 mol of
−130−118−37.0–
per 1 mol of
Hydrogen ion
−32.5−29.4−9.25–
per 1 mol of
Copper(II) ion
−65.0−58.8−18.5–
−260−235−74.0–
per 1 mol of
−65.0−58.8−18.5–
per 1 mol of
−86.7−78.3−24.7–

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
CuF (s)-280-26064.9–
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[1]
H+ (g)1536.202[1]–––
H+ (ao)0[1]0[1]0[1]0[1]
* (s):Solid, (l):Liquid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-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
Cu2+ (g)3054.07[1]–––
Cu2+ (ao)64.77[1]65.49[1]-99.6[1]–
N2O3 (l)50.29[1]–––
N2O3 (g)83.72[1]139.46[1]312.28[1]65.61[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]–
H2O (cr)––––
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid, (ai):Ionized aqueous solution, (cr):Crystalline solid

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)