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14Cu + 2KClO4 → 7Cu2O + Cl2↑ + K2O

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Reaction of copper and potassium perchlorate
14CuCopper + 2KClO4Potassium perchlorate
⟶
7Cu2OCopper(I) oxide + Cl2↑Chlorine + K2OPotassium oxide

The reaction of copper and potassium perchlorate yields copper(I) oxide, chlorine, and potassium oxide (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 and potassium perchlorate
14CuCopper + 2KClO4Potassium perchlorate
⟶
7Cu2OCopper(I) oxide + Cl2↑Chlorine + K2OPotassium oxide

General equation

Reaction of oxidizable species and oxidizing species
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of copper and potassium perchlorate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper14
Reducing
Oxidizable
KClO4Potassium perchlorate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu2OCopper(I) oxide7
Oxidized
–
Cl2Chlorine1
Reduced
–
K2OPotassium oxide1
–
–

Thermodynamic changes

Changes in standard condition

Reaction of copper and potassium perchlorate
◆
ΔrG−737.9 kJ/mol
K1.88 × 10129
pK−129.27
14CuCrystalline solid + 2KClO4Crystalline solid
⟶
7Cu2OCrystalline solid + Cl2↑Gas + K2OCrystalline 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
−676.2−737.9203.0−3.8
per 1 mol of
−48.30−52.7114.50−0.27
−338.1−368.9101.5−1.9
per 1 mol of
−96.60−105.429.00−0.54
per 1 mol of
−676.2−737.9203.0−3.8
per 1 mol of
−676.2−737.9203.0−3.8

Changes in aqueous solution (1)

Reaction of copper and potassium perchlorate
◆
ΔrG−760.5 kJ/mol
K1.71 × 10133
pK−133.23
14CuCrystalline solid + 2KClO4Ionized aqueous solution
⟶
7Cu2OCrystalline solid + Cl2↑Gas + K2OCrystalline 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
−778.3−760.5−64.0–
per 1 mol of
−55.59−54.32−4.57–
−389.1−380.3−32.0–
per 1 mol of
−111.2−108.6−9.14–
per 1 mol of
−778.3−760.5−64.0–
per 1 mol of
−778.3−760.5−64.0–

Changes in aqueous solution (2)

Reaction of copper and potassium perchlorate
◆
ΔrG−753.6 kJ/mol
K1.06 × 10132
pK−132.03
14CuCrystalline solid + 2KClO4Ionized aqueous solution
⟶
7Cu2OCrystalline solid + Cl2↑Un-ionized aqueous solution + K2OCrystalline 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
−801.7−753.6−166–
per 1 mol of
−57.26−53.83−11.9–
−400.9−376.8−83.0–
per 1 mol of
−114.5−107.7−23.7–
per 1 mol of
−801.7−753.6−166–
per 1 mol of
−801.7−753.6−166–

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
Cu (cr)0[1]0[1]33.150[1]24.435[1]
Cu (g)338.32[1]298.58[1]166.38[1]20.786[1]
KClO4 (cr)-432.75[1]-303.09[1]151.0[1]112.38[1]
KClO4 (ai)-381.71[1]-291.79[1]284.5[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
Cu2O (cr)-168.6[1]-146.0[1]93.14[1]63.64[1]
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]–
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]–––
* (cr):Crystalline solid, (g):Gas, (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)
    • 2
      James G. Speight (2017)
      Lange's Handbook of Chemistry, 17th edition
      McGraw Hill Education