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2KI + 2AgNO3 → 2KNO3 + I2 + 2Ag

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Reaction of potassium iodide and silver(I) nitrate
2KIPotassium iodide + 2AgNO3Silver(I) nitrate
⟶
2KNO3Potassium nitrate + I2Iodine + 2AgSilver

The reaction of potassium iodide and silver(I) nitrate yields potassium nitrate, iodine, and silver (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 silver(I) nitrate
2KIPotassium iodide + 2AgNO3Silver(I) nitrate
⟶
2KNO3Potassium nitrate + I2Iodine + 2AgSilver

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 silver(I) nitrate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide2
Reducing
Oxidizable
AgNO3Silver(I) nitrate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
KNO3Potassium nitrate2
–
–
I2Iodine1
Oxidized
–
AgSilver2
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of potassium iodide and silver(I) nitrate
◆
ΔrG−73.12 kJ/mol
K6.46 × 1012
pK−12.81
2KICrystalline solid + 2AgNO3Crystalline solid
⟶
2KNO3Crystalline solid + I2Crystalline solid + 2AgCrystalline 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
−84.68−73.12−27.145.98
per 1 mol of
−42.34−36.56−13.572.99
per 1 mol of
−42.34−36.56−13.572.99
per 1 mol of
−42.34−36.56−13.572.99
per 1 mol of
−84.68−73.12−27.145.98
per 1 mol of
−42.34−36.56−13.572.99

Changes in aqueous solution (1)

Reaction of potassium iodide and silver(I) nitrate
◆
ΔrG−34.64 kJ/mol
K1.17 × 106
pK−6.07
2KIIonized aqueous solution + 2AgNO3Ionized aqueous solution
⟶
2KNO3Ionized aqueous solution + I2Un-ionized aqueous solution + 2AgCrystalline 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
−78.1−34.64−145.9–
per 1 mol of
−39.0−17.32−72.95–
per 1 mol of
−39.0−17.32−72.95–
per 1 mol of
−39.0−17.32−72.95–
per 1 mol of
−78.1−34.64−145.9–
per 1 mol of
−39.0−17.32−72.95–

Changes in aqueous solution (2)

Reaction of potassium iodide and silver(I) nitrate
◆
ΔrG−37.98 kJ/mol
K4.51 × 106
pK−6.65
2KIIonized aqueous solution + 2AgNO3Un-ionized aqueous solution
⟶
2KNO3Ionized aqueous solution + I2Un-ionized aqueous solution + 2AgCrystalline 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
–−37.98––
per 1 mol of
–−18.99––
per 1 mol of
–−18.99––
per 1 mol of
–−18.99––
per 1 mol of
–−37.98––
per 1 mol of
–−18.99––

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]
AgNO3 (cr)-124.39[1]-33.41[1]140.92[1]93.05[1]
AgNO3 (ai)-101.80[1]-34.16[1]219.2[1]-64.9[1]
AgNO3 (ao)–-32.49[1]––
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-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
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]–
Ag (cr)0[1]0[1]42.55[1]25.351[1]
Ag (g)284.55[1]245.65[1]172.997[1]20.786[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (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)