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11KI + 3Zn(NO3)2 + 11H+ → 11K+ + 5HIO3 + 3N2↑ + 3ZnI2 + 3H2O

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Reaction of potassium iodide and zinc nitrate under acidic condition
11KIPotassium iodide + 3Zn(NO3)2Zinc nitrate + 11H+Hydrogen ion
⟶
11K+Potassium ion + 5HIO3Iodic acid + 3N2↑Nitrogen + 3ZnI2Zinc iodide + 3H2OWater

The reaction of potassium iodide, zinc nitrate, and hydrogen ion yields potassium ion, iodic acid, nitrogen, zinc 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 zinc nitrate under acidic condition
11KIPotassium iodide + 3Zn(NO3)2Zinc nitrate + 11H+Hydrogen ion
⟶
11K+Potassium ion + 5HIO3Iodic acid + 3N2↑Nitrogen + 3ZnI2Zinc iodide + 3H2OWater

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 zinc nitrate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide11
Reducing
Oxidizable
Zn(NO3)2Zinc nitrate3
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion11
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
K+Potassium ion11
–
–
HIO3Iodic acid5
Oxidized
–
N2Nitrogen3
Reduced
–
ZnI2Zinc iodide3
–
–
H2OWater3
–
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium iodide and zinc nitrate under acidic condition
◆
ΔrG−448.9 kJ/mol
K4.40 × 1078
pK−78.64
11KIIonized aqueous solution + 3Zn(NO3)2Ionized aqueous solution + 11H+Un-ionized aqueous solution
⟶
11K+Un-ionized aqueous solution + 5HIO3Un-ionized aqueous solution + 3N2↑Gas + 3ZnI2Ionized aqueous solution + 3H2OLiquid
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
−393.8−448.9184.2–
per 1 mol of
−35.80−40.8116.75–
per 1 mol of
−131.3−149.661.40–
per 1 mol of
Hydrogen ion
−35.80−40.8116.75–
per 1 mol of
Potassium ion
−35.80−40.8116.75–
per 1 mol of
−78.76−89.7836.84–
per 1 mol of
−131.3−149.661.40–
per 1 mol of
−131.3−149.661.40–
per 1 mol of
−131.3−149.661.40–

Changes in standard condition (2)

Reaction of potassium iodide and zinc nitrate under acidic condition
◆
ΔrG−420.1 kJ/mol
K3.97 × 1073
pK−73.60
11KIIonized aqueous solution + 3Zn(NO3)2Ionized aqueous solution + 11H+Un-ionized aqueous solution
⟶
11K+Un-ionized aqueous solution + 5HIO3Un-ionized aqueous solution + 3N2↑Gas + 3ZnI2Un-ionized aqueous solution + 3H2OLiquid
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
–−420.1––
per 1 mol of
–−38.19––
per 1 mol of
–−140.0––
per 1 mol of
Hydrogen ion
–−38.19––
per 1 mol of
Potassium ion
–−38.19––
per 1 mol of
–−84.02––
per 1 mol of
–−140.0––
per 1 mol of
–−140.0––
per 1 mol of
–−140.0––

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]
Zn(NO3)2 (cr)-483.7[1]–––
Zn(NO3)2 (ai)-568.61[1]-369.57[1]180.7[1]-126[1]
Zn(NO3)2 (cr)
1 hydrate
-805.0[1]–––
Zn(NO3)2 (cr)
2 hydrate
-1110.27[1]–––
Zn(NO3)2 (cr)
4 hydrate
-1699.12[1]–––
Zn(NO3)2 (cr)
6 hydrate
-2306.64[1]-1772.71[1]456.9[1]323.0[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]
HIO3 (cr)-230.1[1]–––
HIO3 (ao)-211.3[1]-132.6[1]166.9[1]–
N2 (g)0[1]0[1]191.61[1]29.125[1]
ZnI2 (cr)-208.03[1]-208.95[1]161.1[1]–
ZnI2 (ai)-264.26[1]-250.20[1]110.5[1]-238[1]
ZnI2 (ao)–-240.6[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)