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NH4ClO4 🔥→ NH3↑ + HCl↑ + 2O2↑

NH₄ClO₄ 🔥→ NH₃↑ + HCl↑ + 2O₂↑

Last updated: June 13, 2022

Decomposition of ammonium perchlorate: NH₄ClO₄Ammonium perchlorate
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NH₃↑Ammonia + HCl↑Hydrogen chloride + 2O₂↑Oxygen

Decomposition of ammonium perchlorate yields ammonia, hydrogen chloride, and oxygen (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents

Reaction data

Chemical equation

Decomposition of ammonium perchlorate: NH₄ClO₄Ammonium perchlorate
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NH₃↑Ammonia + HCl↑Hydrogen chloride + 2O₂↑Oxygen

General equation

Thermal decomposition with redox: Thermally decomposable substanceSelf redox agent
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ProductOxidation product + ProductReduction product

Thermal decomposition of oxoacid salt with redox: Oxoacid saltSelf redox agent
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ProductOxidation product + ProductReduction product

Oxidation state of each atom

Decomposition of ammonium perchlorate

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
NH₄ClO₄	Ammonium perchlorate	1	Self redox agent	Thermally decomposable Oxoacid salt

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
NH₃	Ammonia	1	–	–
HCl	Hydrogen chloride	1	Reduced	–
O₂	Oxygen	2	Oxidized	–

Thermodynamic changes

Changes in standard condition

Decomposition of ammonium perchlorate ◆ Δ_rG −23.00 kJ/mol K 1.07 × 10⁴ pK −4.03: NH₄ClO₄Crystalline solid
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NH₃↑Gas + HCl↑Gas + 2O₂↑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	156.89	−23.00	603.4	–
per 1 mol of Ammonium perchlorate	156.89	−23.00	603.4	–
per 1 mol of Ammonia	156.89	−23.00	603.4	–
per 1 mol of Hydrogen chloride	156.89	−23.00	603.4	–
per 1 mol of Oxygen	78.445	−11.50	301.7	–

Changes in aqueous solution (1)

Decomposition of ammonium perchlorate ◆ Δ_rG −23.92 kJ/mol K 1.55 × 10⁴ pK −4.19: NH₄ClO₄Ionized aqueous solution
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NH₃↑Gas + HCl↑Gas + 2O₂↑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	123.41	−23.92	494.2	–
per 1 mol of Ammonium perchlorate	123.41	−23.92	494.2	–
per 1 mol of Ammonia	123.41	−23.92	494.2	–
per 1 mol of Hydrogen chloride	123.41	−23.92	494.2	–
per 1 mol of Oxygen	61.705	−11.96	247.1	–

Changes in aqueous solution (2)

Decomposition of ammonium perchlorate ◆ Δ_rG 8.9 kJ/mol K 0.28 × 10⁻¹ pK 1.56: NH₄ClO₄Ionized aqueous solution
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NH₃↑Gas + HCl↑Gas + 2O₂↑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	100.0	8.9	305.8	–
per 1 mol of Ammonium perchlorate	100.0	8.9	305.8	–
per 1 mol of Ammonia	100.0	8.9	305.8	–
per 1 mol of Hydrogen chloride	100.0	8.9	305.8	–
per 1 mol of Oxygen	50.00	4.5	152.9	–

Changes in aqueous solution (3)

Decomposition of ammonium perchlorate ◆ Δ_rG −59.85 kJ/mol K 3.06 × 10¹⁰ pK −10.49: NH₄ClO₄Ionized aqueous solution
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NH₃↑Gas + HCl↑Ionized aqueous solution + 2O₂↑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	48.56	−59.85	363.8	–
per 1 mol of Ammonium perchlorate	48.56	−59.85	363.8	–
per 1 mol of Ammonia	48.56	−59.85	363.8	–
per 1 mol of Hydrogen chloride	48.56	−59.85	363.8	–
per 1 mol of Oxygen	24.28	−29.93	181.9	–

Changes in aqueous solution (4)

Decomposition of ammonium perchlorate ◆ Δ_rG −27.0 kJ/mol K 5.37 × 10⁴ pK −4.73: NH₄ClO₄Ionized aqueous solution
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NH₃↑Gas + HCl↑Ionized aqueous solution + 2O₂↑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	25.2	−27.0	175.4	–
per 1 mol of Ammonium perchlorate	25.2	−27.0	175.4	–
per 1 mol of Ammonia	25.2	−27.0	175.4	–
per 1 mol of Hydrogen chloride	25.2	−27.0	175.4	–
per 1 mol of Oxygen	12.6	−13.5	87.70	–

Changes in aqueous solution (5)

Decomposition of ammonium perchlorate ◆ Δ_rG −33.97 kJ/mol K 8.94 × 10⁵ pK −5.95: NH₄ClO₄Ionized aqueous solution
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NH₃↑Un-ionized aqueous solution + HCl↑Gas + 2O₂↑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	89.23	−33.97	413.1	–
per 1 mol of Ammonium perchlorate	89.23	−33.97	413.1	–
per 1 mol of Ammonia	89.23	−33.97	413.1	–
per 1 mol of Hydrogen chloride	89.23	−33.97	413.1	–
per 1 mol of Oxygen	44.62	−16.98	206.6	–

Changes in aqueous solution (6)

Decomposition of ammonium perchlorate ◆ Δ_rG −1.2 kJ/mol K 1.62 × 10⁰ pK −0.21: NH₄ClO₄Ionized aqueous solution
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NH₃↑Un-ionized aqueous solution + HCl↑Gas + 2O₂↑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	65.8	−1.2	224.6	–
per 1 mol of Ammonium perchlorate	65.8	−1.2	224.6	–
per 1 mol of Ammonia	65.8	−1.2	224.6	–
per 1 mol of Hydrogen chloride	65.8	−1.2	224.6	–
per 1 mol of Oxygen	32.9	−0.60	112.3	–

Changes in aqueous solution (7)

Decomposition of ammonium perchlorate ◆ Δ_rG −69.90 kJ/mol K 1.76 × 10¹² pK −12.25: NH₄ClO₄Ionized aqueous solution
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NH₃↑Un-ionized aqueous solution + HCl↑Ionized aqueous solution + 2O₂↑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	14.38	−69.90	282.7	–
per 1 mol of Ammonium perchlorate	14.38	−69.90	282.7	–
per 1 mol of Ammonia	14.38	−69.90	282.7	–
per 1 mol of Hydrogen chloride	14.38	−69.90	282.7	–
per 1 mol of Oxygen	7.190	−34.95	141.3	–

Changes in aqueous solution (8)

Decomposition of ammonium perchlorate ◆ Δ_rG −37.1 kJ/mol K 3.16 × 10⁶ pK −6.50: NH₄ClO₄Ionized aqueous solution
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NH₃↑Un-ionized aqueous solution + HCl↑Ionized aqueous solution + 2O₂↑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	−9.0	−37.1	94.2	–
per 1 mol of Ammonium perchlorate	−9.0	−37.1	94.2	–
per 1 mol of Ammonia	−9.0	−37.1	94.2	–
per 1 mol of Hydrogen chloride	−9.0	−37.1	94.2	–
per 1 mol of Oxygen	−4.5	−18.6	47.1	–

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
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, (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
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]	–
HCl (g)	-92.307^[1]	-95.299^[1]	186.908^[1]	29.12^[1]
HCl (ai)	-167.159^[1]	-131.228^[1]	56.5^[1]	-136.4^[1]
O₂ (g)	0^[1]	0^[1]	205.138^[1]	29.355^[1]
O₂ (ao)	-11.7^[1]	16.4^[1]	110.9^[1]	–

* (g):Gas, (ao):Un-ionized aqueous solution, (ai):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

Δ_rG	−23.00 kJ/mol
K	1.07 × 10⁴
pK	−4.03

Δ_rG	−23.92 kJ/mol
K	1.55 × 10⁴
pK	−4.19

Δ_rG	8.9 kJ/mol
K	0.28 × 10⁻¹
pK	1.56

Δ_rG	−59.85 kJ/mol
K	3.06 × 10¹⁰
pK	−10.49

NH4ClO4 🔥→ NH3↑ + HCl↑ + 2O2↑

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Products

Thermodynamic changes

Changes in standard condition

Changes in aqueous solution (1)

Changes in aqueous solution (2)

Changes in aqueous solution (3)

Changes in aqueous solution (4)

Changes in aqueous solution (5)

Changes in aqueous solution (6)

Changes in aqueous solution (7)

Changes in aqueous solution (8)

Thermodynamic data of reactants

Thermodynamic data of products

References

List of references

Related reactions

Reactions with same reactants

Related categories

Type of reaction

General equation

Reactant

Product

NH₄ClO₄ 🔥→ NH₃↑ + HCl↑ + 2O₂↑