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6KI + NaIO3 🔥→ 3K2O + 3I2 + NaI

The reaction of potassium iodide and sodium iodate yields potassium oxide, iodine, and sodium iodide (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 oxidizable species and oxidizing species
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide6
Reducing
Oxidizable
NaIO3Sodium iodate1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2OPotassium oxide3
I2Iodine3
Redoxed product
NaISodium iodide1

Thermodynamic changes

Changes in standard condition

Reaction of potassium iodide and sodium iodate
6KICrystalline solid + NaIO3Crystalline solid
🔥
3K2OCrystalline solid + 3I2Crystalline solid + NaICrystalline 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
1076.956.9
per 1 mol of
179.489.48
per 1 mol of
1076.956.9
per 1 mol of
358.9719.0
per 1 mol of
358.9719.0
per 1 mol of
1076.956.9

Changes in aqueous solution

Reaction of potassium iodide and sodium iodate
ΔrG1168.4 kJ/mol
K0.20 × 10−204
pK204.69
6KIIonized aqueous solution + NaIO3Ionized aqueous solution
🔥
3K2OCrystalline solid + 3I2Un-ionized aqueous solution + NaIIonized 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
994.91168.4−596.0
per 1 mol of
165.8194.73−99.33
per 1 mol of
994.91168.4−596.0
per 1 mol of
331.6389.47−198.7
per 1 mol of
331.6389.47−198.7
per 1 mol of
994.91168.4−596.0

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]
NaIO3 (cr)-481.788[1]92.0[1]
NaIO3 (ai)-461.5[1]-389.9[1]177.4[1]
NaIO3 (cr)
1 hydrate
-779.48[1]-634.03[1]162.3[1]
NaIO3 (cr)
5 hydrate
-1952.25[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
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]
I2 (cr)0[1]0[1]116.135[1]54.438[1]
I2 (g)62.438[1]19.327[1]260.69[1]36.90[1]
I2 (ao)22.6[1]16.40[1]137.2[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]
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (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)

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