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20KI + 2AgNO3 + 20H+ → 20K+ + 9I2 + 2Ag + 2NH4I + 6H2O

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Reaction of potassium iodide and silver(I) nitrate under acidic condition
20KIPotassium iodide + 2AgNO3Silver(I) nitrate + 20H+Hydrogen ion
⟶
20K+Potassium ion + 9I2Iodine + 2AgSilver + 2NH4IAmmonium iodide + 6H2OWater

The reaction of potassium iodide, silver(I) nitrate, and hydrogen ion yields potassium ion, iodine, silver, ammonium iodide, 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 silver(I) nitrate under acidic condition
20KIPotassium iodide + 2AgNO3Silver(I) nitrate + 20H+Hydrogen ion
⟶
20K+Potassium ion + 9I2Iodine + 2AgSilver + 2NH4IAmmonium iodide + 6H2OWater

General equation

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

Oxidation state of each atom

Reaction of potassium iodide and silver(I) nitrate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide20
Reducing
Oxidizable
AgNO3Silver(I) nitrate2
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion20
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
K+Potassium ion20
–
–
I2Iodine9
Oxidized
–
AgSilver2
Reduced
–
NH4IAmmonium iodide2
Reduced
–
H2OWater6
–
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium iodide and silver(I) nitrate under acidic condition
◆
ΔrG−437.01 kJ/mol
K3.64 × 1076
pK−76.56
20KIIonized aqueous solution + 2AgNO3Ionized aqueous solution + 20H+Un-ionized aqueous solution
⟶
20K+Un-ionized aqueous solution + 9I2Un-ionized aqueous solution + 2AgCrystalline solid + 2NH4IIonized aqueous solution + 6H2OLiquid
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
−579.6−437.01−475.6–
per 1 mol of
−28.98−21.851−23.78–
per 1 mol of
−289.8−218.50−237.8–
per 1 mol of
Hydrogen ion
−28.98−21.851−23.78–
per 1 mol of
Potassium ion
−28.98−21.851−23.78–
per 1 mol of
−64.40−48.557−52.84–
per 1 mol of
−289.8−218.50−237.8–
per 1 mol of
−289.8−218.50−237.8–
per 1 mol of
−96.60−72.835−79.27–

Changes in standard condition (2)

Reaction of potassium iodide and silver(I) nitrate under acidic condition
◆
ΔrG−440.35 kJ/mol
K1.40 × 1077
pK−77.15
20KIIonized aqueous solution + 2AgNO3Un-ionized aqueous solution + 20H+Un-ionized aqueous solution
⟶
20K+Un-ionized aqueous solution + 9I2Un-ionized aqueous solution + 2AgCrystalline solid + 2NH4IIonized aqueous solution + 6H2OLiquid
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
–−440.35––
per 1 mol of
–−22.018––
per 1 mol of
–−220.18––
per 1 mol of
Hydrogen ion
–−22.018––
per 1 mol of
Potassium ion
–−22.018––
per 1 mol of
–−48.928––
per 1 mol of
–−220.18––
per 1 mol of
–−220.18––
per 1 mol of
–−73.392––

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]––
H+ (g)1536.202[1]–––
H+ (ao)0[1]0[1]0[1]0[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
K+ (g)514.26[1]–––
K+ (ao)-252.38[1]-283.27[1]102.5[1]21.8[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]
NH4I (cr)-201.42[1]-112.5[1]117[1]–
NH4I (ai)-187.69[1]-130.88[1]224.7[1]-62.3[1]
H2O (cr)––––
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]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):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)