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2LiBr + 2KMnO4 + H2O → 2LiOH + KBrO3 + 2MnO2 + KBr

2LiBr + 2KMnO₄ + H₂O → 2LiOH + KBrO₃ + 2MnO₂ + KBr

Last updated: June 13, 2022

Reaction of lithium bromide and potassium permanganate under neutral condition: 2LiBrLithium bromide + 2KMnO₄Potassium permanganate + H₂OWater
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2LiOHLithium hydroxide + KBrO₃Potassium bromate + 2MnO₂Manganese(IV) oxide + KBrPotassium bromide

The reaction of lithium bromide, potassium permanganate, and water yields lithium hydroxide, potassium bromate, manganese(IV) oxide, and potassium bromide (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of hardly oxidizable species and oxidizing species under neutral condition

Table of contents

Reaction data

Chemical equation

Reaction of lithium bromide and potassium permanganate under neutral condition: 2LiBrLithium bromide + 2KMnO₄Potassium permanganate + H₂OWater
⟶
2LiOHLithium hydroxide + KBrO₃Potassium bromate + 2MnO₂Manganese(IV) oxide + KBrPotassium bromide

General equation

Reaction of hardly oxidizable species and oxidizing species under neutral condition: Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H₂ONon-redox agent
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ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of lithium bromide and potassium permanganate under neutral condition

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
LiBr	Lithium bromide	2	Reducing	Hardly oxidizable
KMnO₄	Potassium permanganate	2	Oxidizing	Oxidizing
H₂O	Water	1	–	Water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
LiOH	Lithium hydroxide	2	–	–
KBrO₃	Potassium bromate	1	Oxidized	–
MnO₂	Manganese(IV) oxide	2	Reduced	–
KBr	Potassium bromide	1	–	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of lithium bromide and potassium permanganate under neutral condition ◆ Δ_rG −63.7 kJ/mol K 1.44 × 10¹¹ pK −11.16: 2LiBrCrystalline solid + 2KMnO₄Crystalline solid + H₂OLiquid
⟶
2LiOHCrystalline solid + KBrO₃Crystalline solid + 2MnO₂Crystalline solid + KBrCrystalline solid

	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	−101.3	−63.7	−125.11	–
per 1 mol of Lithium bromide	−50.65	−31.9	−62.555	–
per 1 mol of Potassium permanganate	−50.65	−31.9	−62.555	–
per 1 mol of Water	−101.3	−63.7	−125.11	–
per 1 mol of Lithium hydroxide	−50.65	−31.9	−62.555	–
per 1 mol of Potassium bromate	−101.3	−63.7	−125.11	–
per 1 mol of Manganese(IV) oxide	−50.65	−31.9	−62.555	–
per 1 mol of Potassium bromide	−101.3	−63.7	−125.11	–

Changes in standard condition (2)

Reaction of lithium bromide and potassium permanganate under neutral condition: 2LiBrCrystalline solid + 2KMnO₄Crystalline solid + H₂OLiquid
⟶
2LiOHCrystalline solid + KBrO₃Crystalline solid + 2MnO₂Amorphous solidprecipitated + KBrCrystalline solid

	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	−66.2	–	–	–
per 1 mol of Lithium bromide	−33.1	–	–	–
per 1 mol of Potassium permanganate	−33.1	–	–	–
per 1 mol of Water	−66.2	–	–	–
per 1 mol of Lithium hydroxide	−33.1	–	–	–
per 1 mol of Potassium bromate	−66.2	–	–	–
per 1 mol of Manganese(IV) oxide	−33.1	–	–	–
per 1 mol of Potassium bromide	−66.2	–	–	–

Changes in aqueous solution (1)

Reaction of lithium bromide and potassium permanganate under neutral condition ◆ Δ_rG 9.3 kJ/mol K 0.23 × 10⁻¹ pK 1.63: 2LiBrIonized aqueous solution + 2KMnO₄Ionized aqueous solution + H₂OLiquid
⟶
2LiOHIonized aqueous solution + KBrO₃Ionized aqueous solution + 2MnO₂Crystalline solid + KBrIonized 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	−76.9	9.3	−288.1	–
per 1 mol of Lithium bromide	−38.5	4.7	−144.1	–
per 1 mol of Potassium permanganate	−38.5	4.7	−144.1	–
per 1 mol of Water	−76.9	9.3	−288.1	–
per 1 mol of Lithium hydroxide	−38.5	4.7	−144.1	–
per 1 mol of Potassium bromate	−76.9	9.3	−288.1	–
per 1 mol of Manganese(IV) oxide	−38.5	4.7	−144.1	–
per 1 mol of Potassium bromide	−76.9	9.3	−288.1	–

Changes in aqueous solution (2)

Reaction of lithium bromide and potassium permanganate under neutral condition ◆ Δ_rG 6.9 kJ/mol K 0.62 × 10⁻¹ pK 1.21: 2LiBrIonized aqueous solution + 2KMnO₄Ionized aqueous solution + H₂OLiquid
⟶
2LiOHUn-ionized aqueous solution + KBrO₃Ionized aqueous solution + 2MnO₂Crystalline solid + KBrIonized 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	−76.7	6.9	−279.5	–
per 1 mol of Lithium bromide	−38.4	3.5	−139.8	–
per 1 mol of Potassium permanganate	−38.4	3.5	−139.8	–
per 1 mol of Water	−76.7	6.9	−279.5	–
per 1 mol of Lithium hydroxide	−38.4	3.5	−139.8	–
per 1 mol of Potassium bromate	−76.7	6.9	−279.5	–
per 1 mol of Manganese(IV) oxide	−38.4	3.5	−139.8	–
per 1 mol of Potassium bromide	−76.7	6.9	−279.5	–

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
LiBr (cr)	-351.213^[1]	-342.00^[1]	74.27^[1]	–
LiBr (g)	–	–	224.33^[1]	33.93^[1]
LiBr (ai)	-400.041^[1]	-397.27^[1]	95.8^[1]	-73.2^[1]
LiBr (cr) 1 hydrate	-662.58^[1]	-594.29^[1]	109.6^[1]	–
LiBr (cr) 2 hydrate	-962.7^[1]	-840.5^[1]	162.3^[1]	–
KMnO₄ (cr)	-837.2^[1]	-737.6^[1]	171.71^[1]	117.57^[1]
KMnO₄ (ai)	-793.8^[1]	-730.5^[1]	293.7^[1]	-60.2^[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]

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

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
LiOH (cr)	-484.93^[1]	-438.95^[1]	42.80^[1]	49.66^[1]
LiOH (g)	-238.1^[1]	-242.3^[1]	210.90^[1]	46.02^[1]
LiOH (ai)	-508.48^[1]	-450.58^[1]	2.80^[1]	-79.9^[1]
LiOH (ao)	-508.4^[1]	-451.8^[1]	7.1^[1]	–
LiOH (cr) 1 hydrate	-788.01^[1]	-680.95^[1]	71.21^[1]	79.50^[1]
KBrO₃ (cr)	-360.24^[1]	-271.16^[1]	149.16^[1]	105.19^[1]
KBrO₃ (ai)	-319.45^[1]	-264.67^[1]	264.22^[1]	–
MnO₂ (cr)	-520.03^[1]	-465.14^[1]	53.05^[1]	54.14^[1]
MnO₂ (am) precipitated	-502.5^[1]	–	–	–
KBr (cr)	-393.798^[1]	-380.66^[1]	95.90^[1]	52.30^[1]
KBr (g)	-180.08^[1]	-212.96^[1]	250.52^[1]	36.920^[1]
KBr (ai)	-373.92^[1]	-387.23^[1]	184.9^[1]	-120.1^[1]

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

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