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2CH3COONH4 + 11MnO2 → N2↑ + 4MnCO3 + 7MnO + 7H2O

2CH₃COONH₄ + 11MnO₂ → N₂↑ + 4MnCO₃ + 7MnO + 7H₂O

Last updated: June 13, 2022

Reaction of ammonium acetate and manganese(IV) oxide: 2CH₃COONH₄Ammonium acetate + 11MnO₂Manganese(IV) oxide
⟶
N₂↑Nitrogen + 4MnCO₃Manganese(II) carbonate + 7MnOManganese(II) oxide + 7H₂OWater

The reaction of ammonium acetate and manganese(IV) oxide yields nitrogen, manganese(II) carbonate, manganese(II) oxide, and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of reducing species and reducible species

Table of contents

Reaction data

Chemical equation

Reaction of ammonium acetate and manganese(IV) oxide: 2CH₃COONH₄Ammonium acetate + 11MnO₂Manganese(IV) oxide
⟶
N₂↑Nitrogen + 4MnCO₃Manganese(II) carbonate + 7MnOManganese(II) oxide + 7H₂OWater

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 acetate and manganese(IV) oxide

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
CH₃COONH₄	Ammonium acetate	2	Reducing	Reducing
MnO₂	Manganese(IV) oxide	11	Oxidizing	Reducible

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
N₂	Nitrogen	1	Oxidized	–
MnCO₃	Manganese(II) carbonate	4	Redoxed product	–
MnO	Manganese(II) oxide	7	Reduced	–
H₂O	Water	7	–	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of ammonium acetate and manganese(IV) oxide: 2CH₃COONH₄Crystalline solid + 11MnO₂Crystalline solid
⟶
N₂↑Gas + 4MnCO₃Crystalline solidnatural + 7MnOCrystalline solid + 7H₂OLiquid

	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	−1321.1	–	–	–
per 1 mol of Ammonium acetate	−660.55	–	–	–
per 1 mol of Manganese(IV) oxide	−120.10	–	–	–
per 1 mol of Nitrogen	−1321.1	–	–	–
per 1 mol of Manganese(II) carbonate	−330.27	–	–	–
per 1 mol of Manganese(II) oxide	−188.73	–	–	–
per 1 mol of Water	−188.73	–	–	–

Changes in standard condition (2)

Reaction of ammonium acetate and manganese(IV) oxide: 2CH₃COONH₄Crystalline solid + 11MnO₂Crystalline solid
⟶
N₂↑Gas + 4MnCO₃Crystalline solidprecipitated + 7MnOCrystalline solid + 7H₂OLiquid

	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	−1277.5	–	–	–
per 1 mol of Ammonium acetate	−638.75	–	–	–
per 1 mol of Manganese(IV) oxide	−116.14	–	–	–
per 1 mol of Nitrogen	−1277.5	–	–	–
per 1 mol of Manganese(II) carbonate	−319.38	–	–	–
per 1 mol of Manganese(II) oxide	−182.50	–	–	–
per 1 mol of Water	−182.50	–	–	–

Changes in standard condition (3)

Reaction of ammonium acetate and manganese(IV) oxide: 2CH₃COONH₄Crystalline solid + 11MnO₂Amorphous solidprecipitated
⟶
N₂↑Gas + 4MnCO₃Crystalline solidnatural + 7MnOCrystalline solid + 7H₂OLiquid

	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	−1514.0	–	–	–
per 1 mol of Ammonium acetate	−757.00	–	–	–
per 1 mol of Manganese(IV) oxide	−137.64	–	–	–
per 1 mol of Nitrogen	−1514.0	–	–	–
per 1 mol of Manganese(II) carbonate	−378.50	–	–	–
per 1 mol of Manganese(II) oxide	−216.29	–	–	–
per 1 mol of Water	−216.29	–	–	–

Changes in standard condition (4)

Reaction of ammonium acetate and manganese(IV) oxide: 2CH₃COONH₄Crystalline solid + 11MnO₂Amorphous solidprecipitated
⟶
N₂↑Gas + 4MnCO₃Crystalline solidprecipitated + 7MnOCrystalline solid + 7H₂OLiquid

	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	−1470.4	–	–	–
per 1 mol of Ammonium acetate	−735.20	–	–	–
per 1 mol of Manganese(IV) oxide	−133.67	–	–	–
per 1 mol of Nitrogen	−1470.4	–	–	–
per 1 mol of Manganese(II) carbonate	−367.60	–	–	–
per 1 mol of Manganese(II) oxide	−210.06	–	–	–
per 1 mol of Water	−210.06	–	–	–

Changes in aqueous solution

Reaction of ammonium acetate and manganese(IV) oxide ◆ Δ_rG −1453.2 kJ/mol K 3.89 × 10²⁵⁴ pK −254.59: 2CH₃COONH₄Ionized aqueous solution + 11MnO₂Crystalline solid
⟶
N₂↑Gas + 4MnCO₃Crystalline solidnatural + 7MnOCrystalline solid + 7H₂OLiquid

	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	−1316.4	−1453.2	458.6	457.5
per 1 mol of Ammonium acetate	−658.20	−726.60	229.3	228.8
per 1 mol of Manganese(IV) oxide	−119.67	−132.11	41.69	41.59
per 1 mol of Nitrogen	−1316.4	−1453.2	458.6	457.5
per 1 mol of Manganese(II) carbonate	−329.10	−363.30	114.7	114.4
per 1 mol of Manganese(II) oxide	−188.06	−207.60	65.51	65.36
per 1 mol of Water	−188.06	−207.60	65.51	65.36

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
CH₃COONH₄ (cr)	-616.14^[1]	–	–	–
CH₃COONH₄ (ai)	-618.52^[1]	-448.61^[1]	200.0^[1]	73.6^[1]
MnO₂ (cr)	-520.03^[1]	-465.14^[1]	53.05^[1]	54.14^[1]
MnO₂ (am) precipitated	-502.5^[1]	–	–	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid

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
N₂ (g)	0^[1]	0^[1]	191.61^[1]	29.125^[1]
MnCO₃ (cr) natural	-894.1^[1]	-816.7^[1]	85.8^[1]	81.50^[1]
MnCO₃ (cr) precipitated	-883.2^[1]	–	–	–
MnO (cr)	-385.22^[1]	-362.90^[1]	59.71^[1]	45.44^[1]
MnO (g)	124.22^[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, (cr):Crystalline solid, (l):Liquid

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	−1453.2 kJ/mol
K	3.89 × 10²⁵⁴
pK	−254.59

2CH3COONH4 + 11MnO2 → N2↑ + 4MnCO3 + 7MnO + 7H2O

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Products

Thermodynamic changes

Changes in standard condition (1)

Changes in standard condition (2)

Changes in standard condition (3)

Changes in standard condition (4)

Changes in aqueous solution

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

2CH₃COONH₄ + 11MnO₂ → N₂↑ + 4MnCO₃ + 7MnO + 7H₂O