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  3. 12NaCl + 2KIO3 🔥→ 2NaI + 5Na2O + 6Cl2↑ + K2O

12NaCl + 2KIO3 🔥→ 2NaI + 5Na2O + 6Cl2↑ + K2O

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Reaction of sodium chloride and potassium iodate
12NaClSodium chloride + 2KIO3Potassium iodate
🔥
⟶
2NaISodium iodide + 5Na2OSodium oxide + 6Cl2↑Chlorine + K2OPotassium oxide

The reaction of sodium chloride and potassium iodate yields sodium iodide, sodium 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 sodium chloride and potassium iodate
12NaClSodium chloride + 2KIO3Potassium iodate
🔥
⟶
2NaISodium iodide + 5Na2OSodium oxide + 6Cl2↑Chlorine + K2OPotassium oxide

General equation

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

Oxidation state of each atom

Reaction of sodium chloride and potassium iodate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaClSodium chloride12
Reducing
Hardly oxidizable
KIO3Potassium iodate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaISodium iodide2
Reduced
–
Na2OSodium oxide5
–
–
Cl2Chlorine6
Oxidized
–
K2OPotassium oxide1
–
–

Thermodynamic changes

Changes in standard condition

Reaction of sodium chloride and potassium iodate
◆
ΔrG2674.8 kJ/mol
K0.25 × 10−468
pK468.60
12NaClCrystalline solid + 2KIO3Crystalline solid
🔥
⟶
2NaICrystalline solid + 5Na2OCrystalline solid + 6Cl2↑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
2928.42674.8836.4−82.0
per 1 mol of
244.03222.9069.70−6.83
per 1 mol of
1464.21337.4418.2−41.0
per 1 mol of
1464.21337.4418.2−41.0
per 1 mol of
585.68534.96167.3−16.4
per 1 mol of
488.07445.80139.4−13.7
per 1 mol of
2928.42674.8836.4−82.0

Changes in aqueous solution (1)

Reaction of sodium chloride and potassium iodate
◆
ΔrG2713.7 kJ/mol
K0.38 × 10−475
pK475.42
12NaClIonized aqueous solution + 2KIO3Ionized aqueous solution
🔥
⟶
2NaIIonized aqueous solution + 5Na2OCrystalline solid + 6Cl2↑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
2811.22713.7320.6–
per 1 mol of
234.27226.1426.72–
per 1 mol of
1405.61356.8160.3–
per 1 mol of
1405.61356.8160.3–
per 1 mol of
562.24542.7464.12–
per 1 mol of
468.53452.2853.43–
per 1 mol of
2811.22713.7320.6–

Changes in aqueous solution (2)

Reaction of sodium chloride and potassium iodate
◆
ΔrG2755.3 kJ/mol
K0.20 × 10−482
pK482.71
12NaClIonized aqueous solution + 2KIO3Ionized aqueous solution
🔥
⟶
2NaIIonized aqueous solution + 5Na2OCrystalline solid + 6Cl2↑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
2670.82755.3−292–
per 1 mol of
222.57229.61−24.3–
per 1 mol of
1335.41377.7−146–
per 1 mol of
1335.41377.7−146–
per 1 mol of
534.16551.06−58.4–
per 1 mol of
445.13459.22−48.7–
per 1 mol of
2670.82755.3−292–

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
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]
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]–
* (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
NaI (cr)-287.78[1]-286.06[1]98.53[1]52.09[1]
NaI (g)-79.5[1]-121.0[1]248.978[1]36.65[1]
NaI (ai)-295.31[1]-313.47[1]170.3[1]-95.8[1]
NaI (cr)
1 hydrate
-883.096[1]-771.10[1]196.2[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]
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, (ai):Ionized aqueous solution, (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