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2KI + Fe(NO3)3 + 2H+ ๐Ÿ”ฅโ†’ 2KNO3 + I2 + Fe2+ + NO2โ†‘ + H2O

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Reaction of potassium iodide and iron(III) nitrate under acidic condition
2KIPotassium iodide + Fe(NO3)3Iron(III) nitrate + 2H+Hydrogen ion
๐Ÿ”ฅ
โŸถ
2KNO3Potassium nitrate + I2Iodine + Fe2+Iron(II) ion + NO2โ†‘Nitrogen dioxide + H2OWater

The reaction of potassium iodide, iron(III) nitrate, and hydrogen ion yields potassium nitrate, iodine, iron(II) ion, nitrogen dioxide, and water (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 iron(III) nitrate under acidic condition
2KIPotassium iodide + Fe(NO3)3Iron(III) nitrate + 2H+Hydrogen ion
๐Ÿ”ฅ
โŸถ
2KNO3Potassium nitrate + I2Iodine + Fe2+Iron(II) ion + NO2โ†‘Nitrogen dioxide + H2OWater

General equation

Reaction of oxidizable species and oxidizing species under acidic condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent
โŸถ
ProductOxidation product + ProductReduction product + H2ONon-redox product

Oxidation state of each atom

Reaction of potassium iodide and iron(III) nitrate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide2
Reducing
Oxidizable
Fe(NO3)3Iron(III) nitrate1
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion2
โ€“
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
KNO3Potassium nitrate2
โ€“
โ€“
I2Iodine1
Oxidized
โ€“
Fe2+Iron(II) ion1
Reduced
โ€“
NO2Nitrogen dioxide1
Reduced
โ€“
H2OWater1
โ€“
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium iodide and iron(III) nitrate under acidic condition
โ—†
ฮ”rGโˆ’29.4 kJ/mol
K1.41 ร— 105
pKโˆ’5.15
2KIIonized aqueous solution + Fe(NO3)3Ionized aqueous solution + 2H+Un-ionized aqueous solution
๐Ÿ”ฅ
โŸถ
2KNO3Ionized aqueous solution + I2Un-ionized aqueous solution + Fe2+Un-ionized aqueous solution + NO2โ†‘Gas + H2OLiquid
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
47.2โˆ’29.4256.3โ€“
per 1 mol of
23.6โˆ’14.7128.2โ€“
per 1 mol of
47.2โˆ’29.4256.3โ€“
per 1 mol of
Hydrogen ion
23.6โˆ’14.7128.2โ€“
per 1 mol of
23.6โˆ’14.7128.2โ€“
per 1 mol of
47.2โˆ’29.4256.3โ€“
per 1 mol of
Iron(II) ion
47.2โˆ’29.4256.3โ€“
per 1 mol of
47.2โˆ’29.4256.3โ€“
per 1 mol of
47.2โˆ’29.4256.3โ€“

Changes in standard condition (2)

Reaction of potassium iodide and iron(III) nitrate under acidic condition
2KIIonized aqueous solution + Fe(NO3)3Aqueous solution + 2H+Un-ionized aqueous solution
๐Ÿ”ฅ
โŸถ
2KNO3Ionized aqueous solution + I2Un-ionized aqueous solution + Fe2+Un-ionized aqueous solution + NO2โ†‘Gas + H2OLiquid
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
51.4โ€“โ€“โ€“
per 1 mol of
25.7โ€“โ€“โ€“
per 1 mol of
51.4โ€“โ€“โ€“
per 1 mol of
Hydrogen ion
25.7โ€“โ€“โ€“
per 1 mol of
25.7โ€“โ€“โ€“
per 1 mol of
51.4โ€“โ€“โ€“
per 1 mol of
Iron(II) ion
51.4โ€“โ€“โ€“
per 1 mol of
51.4โ€“โ€“โ€“
per 1 mol of
51.4โ€“โ€“โ€“

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ฮ”fHยฐ
kJ ยท molโˆ’1		Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1		Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’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]
Fe(NO3)3 (ai)-670.7[1]-338.3[1]123.4[1]โ€“
Fe(NO3)3 (aq)-674.9[1]โ€“โ€“โ€“
Fe(NO3)3 (cr)
9 hydrate
-3285.3[1]โ€“โ€“โ€“
H+ (g)1536.202[1]โ€“โ€“โ€“
H+ (ao)0[1]0[1]0[1]0[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (aq):Aqueous solution, (ao):Un-ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ฮ”fHยฐ
kJ ยท molโˆ’1		Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1		Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
KNO3 (cr)-494.63[1]-394.86[1]133.05[1]96.40[1]
KNO3 (ai)-459.74[1]-394.53[1]248.9[1]-64.9[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]โ€“
Fe2+ (g)2749.93[1]โ€“โ€“โ€“
Fe2+ (ao)-89.1[1]-78.90[1]-137.7[1]โ€“
NO2 (g)33.18[1]51.31[1]240.06[1]37.20[1]
H2O (cr)โ€“โ€“โ€“โ€“
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid

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)