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2NH4ClO3 + 3I2 → N2↑ + 6HI↑ + 2HClO3

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Reaction of ammonium chlorate and iodine
2NH4ClO3Ammonium chlorate + 3I2Iodine
⟶
N2↑Nitrogen + 6HI↑Hydrogen iodide + 2HClO3Chloric acid

The reaction of ammonium chlorate and iodine yields nitrogen, hydrogen iodide, and chloric acid (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 ammonium chlorate and iodine
2NH4ClO3Ammonium chlorate + 3I2Iodine
⟶
N2↑Nitrogen + 6HI↑Hydrogen iodide + 2HClO3Chloric acid

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of ammonium chlorate and iodine

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4ClO3Ammonium chlorate2
Reducing
Reducing
I2Iodine3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
N2Nitrogen1
Oxidized
–
HIHydrogen iodide6
Reduced
–
HClO3Chloric acid2
–
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of ammonium chlorate and iodine
◆
ΔrG119.62 kJ/mol
K0.11 × 10−20
pK20.96
2NH4ClO3Ionized aqueous solution + 3I2Un-ionized aqueous solution
⟶
N2↑Gas + 6HI↑Gas + 2HClO3Ionized aqueous 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
356.1119.62792.8–
per 1 mol of
178.159.810396.4–
per 1 mol of
118.739.873264.3–
per 1 mol of
356.1119.62792.8–
per 1 mol of
59.3519.937132.1–
per 1 mol of
178.159.810396.4–

Changes in aqueous solution (2)

Reaction of ammonium chlorate and iodine
◆
ΔrG−200.00 kJ/mol
K1.09 × 1035
pK−35.04
2NH4ClO3Ionized aqueous solution + 3I2Un-ionized aqueous solution
⟶
N2↑Gas + 6HI↑Ionized aqueous solution + 2HClO3Ionized aqueous 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
−133.9−200.00221.0–
per 1 mol of
−66.95−100.00110.5–
per 1 mol of
−44.63−66.66773.67–
per 1 mol of
−133.9−200.00221.0–
per 1 mol of
−22.32−33.33336.83–
per 1 mol of
−66.95−100.00110.5–

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
NH4ClO3 (ai)-236.48[1]-87.26[1]275.7[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]–
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (g):Gas, (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
N2 (g)0[1]0[1]191.61[1]29.125[1]
HI (g)26.48[1]1.70[1]206.594[1]29.158[1]
HI (ai)-55.19[1]-51.57[1]111.3[1]-142.3[1]
HClO3 (ai)-103.97[1]-7.95[1]162.3[1]–
* (g):Gas, (ai):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)