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4Na + 2KClO4 → 2NaClO3 + Na2O + K2O

The reaction of sodium and potassium perchlorate yields sodium chlorate, sodium oxide, 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

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium4
Reducing
Reducing
KClO4Potassium perchlorate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaClO3Sodium chlorate2
Redoxed product
Na2OSodium oxide1
Oxidized
K2OPotassium oxide1

Thermodynamic changes

Changes in standard condition

Reaction of sodium and potassium perchlorate
ΔrG−615.9 kJ/mol
K7.96 × 10107
pK−107.90
4NaCrystalline solid + 2KClO4Crystalline solid
2NaClO3Crystalline solid + Na2OCrystalline solid + 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
−641.8−615.9−90.9
per 1 mol of
−160.4−154.0−22.7
−320.9−307.9−45.5
per 1 mol of
−320.9−307.9−45.5
per 1 mol of
−641.8−615.9−90.9
per 1 mol of
−641.8−615.9−90.9

Changes in aqueous solution

Reaction of sodium and potassium perchlorate
ΔrG−653.7 kJ/mol
K3.34 × 10114
pK−114.52
4NaCrystalline solid + 2KClO4Ionized aqueous solution
2NaClO3Ionized aqueous solution + Na2OCrystalline solid + 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
−700.5−653.7−162.1
per 1 mol of
−175.1−163.4−40.52
−350.3−326.9−81.05
per 1 mol of
−350.3−326.9−81.05
per 1 mol of
−700.5−653.7−162.1
per 1 mol of
−700.5−653.7−162.1

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]
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
NaClO3 (cr)-365.774[1]-262.259[1]123.4[1]
NaClO3 (ai)-344.09[1]-269.84[1]221.3[1]
Na2O (cr)-414.22[1]-375.46[1]75.06[1]69.12[1]
Na2O (g)-35.6[1]-52.3[1]261.2[1]55.2[1]
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas

References

List of references

  1. 1
  2. 2
    James G. Speight (2017)
    Lange's Handbook of Chemistry, 17th edition
    McGraw Hill Education