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2KI + 2FeF3 🔥→ 2KF + I2 + 2FeF2

The reaction of potassium iodide and iron(III) fluoride yields potassium fluoride, iodine, and iron(II) fluoride (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 reducible species
Oxidizable speciesReducing agent + Reducible speciesOxidizing agent
🔥
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide2
Reducing
Oxidizable
FeF3Iron(III) fluoride2
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
KFPotassium fluoride2
I2Iodine1
Oxidized
FeF2Iron(II) fluoride2
Reduced

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of potassium iodide and iron(III) fluoride
2KIIonized aqueous solution + 2FeF3Aqueous solution
🔥
2KFIonized aqueous solution + I2Un-ionized aqueous solution + 2FeF2Aqueous 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
9.9
per 1 mol of
5.0
per 1 mol of
5.0
per 1 mol of
5.0
per 1 mol of
9.9
per 1 mol of
5.0

Changes in aqueous solution (2)

Reaction of potassium iodide and iron(III) fluoride
2KIIonized aqueous solution + 2FeF3Aqueous solution
🔥
2KFIonized aqueous solution + I2Un-ionized aqueous solution + 2FeF2Crystalline 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
77.7
per 1 mol of
38.9
per 1 mol of
38.9
per 1 mol of
38.9
per 1 mol of
77.7
per 1 mol of
38.9

Changes in aqueous solution (3)

Reaction of potassium iodide and iron(III) fluoride
2KIIonized aqueous solution + 2FeF3Ionized aqueous solution
🔥
2KFIonized aqueous solution + I2Un-ionized aqueous solution + 2FeF2Aqueous 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
70.1
per 1 mol of
35.0
per 1 mol of
35.0
per 1 mol of
35.0
per 1 mol of
70.1
per 1 mol of
35.0

Changes in aqueous solution (4)

Reaction of potassium iodide and iron(III) fluoride
ΔrG−93.4 kJ/mol
K2.31 × 1016
pK−16.36
2KIIonized aqueous solution + 2FeF3Ionized aqueous solution
🔥
2KFIonized aqueous solution + I2Un-ionized aqueous solution + 2FeF2Crystalline 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
137.9−93.4775.6
per 1 mol of
68.95−46.7387.8
per 1 mol of
68.95−46.7387.8
per 1 mol of
68.95−46.7387.8
per 1 mol of
137.9−93.4775.6
per 1 mol of
68.95−46.7387.8

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]
FeF3 (ai)-1046.4[1]-840.9[1]-357.3[1]
FeF3 (aq)-1016.3[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (aq):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
KF (cr)-567.27[1]-537.75[1]66.57[1]49.04[1]
KF (g)-325.43[1]-343.62[1]226.41[1]35.23[1]
KF (ai)-585.01[1]-562.06[1]88.7[1]-84.9[1]
KF (cr)
2 hydrate
-1163.621[1]-1021.49[1]155.2[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]
FeF2 (cr)-711.3[1]-668.6[1]86.99[1]68.12[1]
FeF2 (ai)-754.4[1]-636.48[1]-165.3[1]
FeF2 (aq)-745.2[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (aq):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)