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KI + 3NaClO4 → KIO3 + 3NaClO3

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Reaction of potassium iodide and sodium perchlorate
KIPotassium iodide + 3NaClO4Sodium perchlorate
⟶
KIO3Potassium iodate + 3NaClO3Sodium chlorate

The reaction of potassium iodide and sodium perchlorate yields potassium iodate and sodium chlorate (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 potassium iodide and sodium perchlorate
KIPotassium iodide + 3NaClO4Sodium perchlorate
⟶
KIO3Potassium iodate + 3NaClO3Sodium chlorate

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 potassium iodide and sodium perchlorate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide1
Reducing
Oxidizable
NaClO4Sodium perchlorate3
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
KIO3Potassium iodate1
Oxidized
–
NaClO3Sodium chlorate3
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of potassium iodide and sodium perchlorate
◆
ΔrG−115.69 kJ/mol
K1.85 × 1020
pK−20.27
KICrystalline solid + 3NaClO4Crystalline solid
⟶
KIO3Crystalline solid + 3NaClO3Crystalline 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
−120.89−115.69−11.6–
per 1 mol of
−120.89−115.69−11.6–
per 1 mol of
−40.297−38.563−3.87–
per 1 mol of
−120.89−115.69−11.6–
per 1 mol of
−40.297−38.563−3.87–

Changes in aqueous solution

Reaction of potassium iodide and sodium perchlorate
◆
ΔrG−74.6 kJ/mol
K1.17 × 1013
pK−13.07
KIIonized aqueous solution + 3NaClO4Ionized aqueous solution
⟶
KIO3Ionized aqueous solution + 3NaClO3Ionized 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
−90.0−74.6−52.0–
per 1 mol of
−90.0−74.6−52.0–
per 1 mol of
−30.0−24.9−17.3–
per 1 mol of
−90.0−74.6−52.0–
per 1 mol of
−30.0−24.9−17.3–

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
KI (cr)-327.900[1]-324.892[1]106.32[1]52.93[1]
KI (g)-125.5[1]-166.1[1]258.3[1]37.11[1]
KI (ai)-307.57[1]-334.85[1]213.8[1]-120.5[1]
NaClO4 (cr)-383.30[1]-254.85[1]142.3[1]–
NaClO4 (ai)-369.45[1]-270.41[1]241.0[1]–
NaClO4 (cr)
1 hydrate
-677.77[1]-494.29[1]190.8[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
KIO3 (cr)-501.37[1]-418.35[1]151.46[1]106.48[1]
KIO3 (ai)-473.6[1]-411.2[1]220.9[1]–
NaClO3 (cr)-365.774[1]-262.259[1]123.4[1]–
NaClO3 (ai)-344.09[1]-269.84[1]221.3[1]–
* (cr):Crystalline solid, (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)