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5Na + KClO2 → NaCl + 2Na2O + K

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Reaction of sodium and potassium chlorite
5NaSodium + KClO2Potassium chlorite
⟶
NaClSodium chloride + 2Na2OSodium oxide + KPotassium

The reaction of sodium and potassium chlorite yields sodium chloride, sodium oxide, and potassium (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 sodium and potassium chlorite
5NaSodium + KClO2Potassium chlorite
⟶
NaClSodium chloride + 2Na2OSodium oxide + KPotassium

General equation

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

Oxidation state of each atom

Reaction of sodium and potassium chlorite

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium5
Reducing
Reducing
KClO2Potassium chlorite1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaClSodium chloride1
Redoxed product
–
Na2OSodium oxide2
Oxidized
–
KPotassium1
Reduced
–

Thermodynamic changes

Changes in aqueous solution

Reaction of sodium and potassium chlorite
◆
ΔrG−878.0 kJ/mol
K6.59 × 10153
pK−153.82
5NaCrystalline solid + KClO2Ionized aqueous solution
⟶
NaClIonized aqueous solution + 2Na2OCrystalline solid + KCrystalline 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
−916.9−878.0−130.1–
per 1 mol of
−183.4−175.6−26.02–
per 1 mol of
−916.9−878.0−130.1–
per 1 mol of
−916.9−878.0−130.1–
per 1 mol of
−458.4−439.0−65.05–
per 1 mol of
−916.9−878.0−130.1–

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]
KClO2 (ai)-318.8[1]-266.1[1]203.8[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
NaCl (cr)-411.153[1]-384.138[1]72.13[1]50.50[1]
NaCl (g)-176.65[1]-196.66[1]229.81[1]35.77[1]
NaCl (ai)-407.27[1]-393.133[1]115.5[1]-90.0[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]
K (cr)0[1]0[1]64.18[1]29.58[1]
K (g)89.24[1]60.59[1]160.336[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)