Home
Chemical reactions
8KI + 4NH4ClO4 🔥→ KCl + 4KOH + 3KClO4 + 4I2 + 4NH3↑

8KI + 4NH₄ClO₄ 🔥→ KCl + 4KOH + 3KClO₄ + 4I₂ + 4NH₃↑

Last updated: May 12, 2022

Reaction of potassium iodide and ammonium perchlorate: 8KIPotassium iodide + 4NH₄ClO₄Ammonium perchlorate
🔥
⟶
KClPotassium chloride + 4KOHPotassium hydroxide + 3KClO₄Potassium perchlorate + 4I₂Iodine + 4NH₃↑Ammonia

The reaction of potassium iodide and ammonium perchlorate yields potassium chloride, potassium hydroxide, potassium perchlorate, iodine, and ammonia (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of oxidizable species and oxidizing species

Table of contents

Reaction data

Chemical equation

Reaction of potassium iodide and ammonium perchlorate: 8KIPotassium iodide + 4NH₄ClO₄Ammonium perchlorate
🔥
⟶
KClPotassium chloride + 4KOHPotassium hydroxide + 3KClO₄Potassium perchlorate + 4I₂Iodine + 4NH₃↑Ammonia

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 ammonium perchlorate

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
KI	Potassium iodide	8	Reducing	Oxidizable
NH₄ClO₄	Ammonium perchlorate	4	Oxidizing	Oxidizing

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
KCl	Potassium chloride	1	Reduced	–
KOH	Potassium hydroxide	4	–	–
KClO₄	Potassium perchlorate	3	–	–
I₂	Iodine	4	Oxidized	–
NH₃	Ammonia	4	–	–

Thermodynamic changes

Changes in standard condition

Reaction of potassium iodide and ammonium perchlorate ◆ Δ_rG 53.61 kJ/mol K 0.41 × 10⁻⁹ pK 9.39: 8KICrystalline solid + 4NH₄ClO₄Crystalline solid
🔥
⟶
KClCrystalline solid + 4KOHCrystalline solid + 3KClO₄Crystalline solid + 4I₂Crystalline solid + 4NH₃↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	185.95	53.61	490.2	–
per 1 mol of Potassium iodide	23.244	6.701	61.27	–
per 1 mol of Ammonium perchlorate	46.487	13.40	122.5	–
per 1 mol of Potassium chloride	185.95	53.61	490.2	–
per 1 mol of Potassium hydroxide	46.487	13.40	122.5	–
per 1 mol of Potassium perchlorate	61.983	17.87	163.4	–
per 1 mol of Iodine	46.487	13.40	122.5	–
per 1 mol of Ammonia	46.487	13.40	122.5	–

Changes in aqueous solution (1)

Reaction of potassium iodide and ammonium perchlorate ◆ Δ_rG −21.94 kJ/mol K 6.98 × 10³ pK −3.84: 8KIIonized aqueous solution + 4NH₄ClO₄Ionized aqueous solution
🔥
⟶
KClIonized aqueous solution + 4KOHIonized aqueous solution + 3KClO₄Ionized aqueous solution + 4I₂Un-ionized aqueous solution + 4NH₃↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−80.3	−21.94	−194.5	–
per 1 mol of Potassium iodide	−10.0	−2.743	−24.31	–
per 1 mol of Ammonium perchlorate	−20.1	−5.485	−48.63	–
per 1 mol of Potassium chloride	−80.3	−21.94	−194.5	–
per 1 mol of Potassium hydroxide	−20.1	−5.485	−48.63	–
per 1 mol of Potassium perchlorate	−26.8	−7.313	−64.83	–
per 1 mol of Iodine	−20.1	−5.485	−48.63	–
per 1 mol of Ammonia	−20.1	−5.485	−48.63	–

Changes in aqueous solution (2)

Reaction of potassium iodide and ammonium perchlorate ◆ Δ_rG −62.14 kJ/mol K 7.70 × 10¹⁰ pK −10.89: 8KIIonized aqueous solution + 4NH₄ClO₄Ionized aqueous solution
🔥
⟶
KClIonized aqueous solution + 4KOHIonized aqueous solution + 3KClO₄Ionized aqueous solution + 4I₂Un-ionized aqueous solution + 4NH₃↑Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−217.0	−62.14	−519.1	–
per 1 mol of Potassium iodide	−27.13	−7.768	−64.89	–
per 1 mol of Ammonium perchlorate	−54.25	−15.54	−129.8	–
per 1 mol of Potassium chloride	−217.0	−62.14	−519.1	–
per 1 mol of Potassium hydroxide	−54.25	−15.54	−129.8	–
per 1 mol of Potassium perchlorate	−72.33	−20.71	−173.0	–
per 1 mol of Iodine	−54.25	−15.54	−129.8	–
per 1 mol of Ammonia	−54.25	−15.54	−129.8	–

Thermodynamic data of reactants

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° 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]
NH₄ClO₄ (cr)	-295.31^[1]	-88.75^[1]	186.2^[1]	–
NH₄ClO₄ (ai)	-261.83^[1]	-87.83^[1]	295.4^[1]	–

* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

Thermodynamic data of products

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
KCl (cr)	-436.747^[1]	-409.14^[1]	82.59^[1]	51.30^[1]
KCl (g)	-214.14^[1]	-233.0^[1]	239.10^[1]	36.48^[1]
KCl (ai)	-419.53^[1]	-414.49^[1]	159.0^[1]	-114.6^[1]
KOH (cr)	-424.764^[1]	-379.08^[1]	78.9^[1]	64.9^[1]
KOH (g)	-231.0^[1]	-232.6^[1]	238.3^[1]	49.20^[1]
KOH (ai)	-482.37^[1]	-440.50^[1]	91.6^[1]	-126.8^[1]
KOH (cr) 1 hydrate	-748.9^[1]	-645.1^[1]	117.2^[1]	–
KOH (cr) 2 hydrate	-1051.0^[1]	-887.3^[1]	150.6^[1]	–
KClO₄ (cr)	-432.75^[1]	-303.09^[1]	151.0^[1]	112.38^[1]
KClO₄ (ai)	-381.71^[1]	-291.79^[1]	284.5^[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]	–
NH₃ (g)	-46.11^[1]	-16.45^[1]	192.45^[1]	35.06^[1]
NH₃ (ao)	-80.29^[1]	-26.50^[1]	111.3^[1]	–

* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

References

List of references

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
https://doi.org/10.18434/M32124
National Institute of Standards and Technology (NIST)
Citation list