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2ZnBr2 + 6KMnO4 + 3H2O 🔥→ 2Zn(OH)2 + 4KBrO3 + 3Mn2O3 + 2KOH

2ZnBr₂ + 6KMnO₄ + 3H₂O 🔥→ 2Zn(OH)₂ + 4KBrO₃ + 3Mn₂O₃ + 2KOH

Last updated: May 12, 2022

Reaction of zinc bromide and potassium permanganate under neutral condition: 2ZnBr₂Zinc bromide + 6KMnO₄Potassium permanganate + 3H₂OWater
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2Zn(OH)₂Zinc hydroxide + 4KBrO₃Potassium bromate + 3Mn₂O₃Manganese(III) oxide + 2KOHPotassium hydroxide

The reaction of zinc bromide, potassium permanganate, and water yields zinc hydroxide, potassium bromate, manganese(III) oxide, and potassium hydroxide (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 zinc bromide and potassium permanganate under neutral condition: 2ZnBr₂Zinc bromide + 6KMnO₄Potassium permanganate + 3H₂OWater
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2Zn(OH)₂Zinc hydroxide + 4KBrO₃Potassium bromate + 3Mn₂O₃Manganese(III) oxide + 2KOHPotassium hydroxide

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 zinc bromide and potassium permanganate under neutral condition

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
ZnBr₂	Zinc bromide	2	Reducing	Hardly oxidizable
KMnO₄	Potassium permanganate	6	Oxidizing	Oxidizing
H₂O	Water	3	–	Water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Zn(OH)₂	Zinc hydroxide	2	–	–
KBrO₃	Potassium bromate	4	Oxidized	–
Mn₂O₃	Manganese(III) oxide	3	Reduced	–
KOH	Potassium hydroxide	2	–	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of zinc bromide and potassium permanganate under neutral condition ◆ Δ_rG 167.5 kJ/mol K 0.45 × 10⁻²⁹ pK 29.34: 2ZnBr₂Crystalline solid + 6KMnO₄Crystalline solid + 3H₂OLiquid
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2Zn(OH)₂Crystalline solidγ + 4KBrO₃Crystalline solid + 3Mn₂O₃Crystalline solid + 2KOHCrystalline 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	–	167.5	–	–
per 1 mol of Zinc bromide	–	83.75	–	–
per 1 mol of Potassium permanganate	–	27.92	–	–
per 1 mol of Water	–	55.83	–	–
per 1 mol of Zinc hydroxide	–	83.75	–	–
per 1 mol of Potassium bromate	–	41.88	–	–
per 1 mol of Manganese(III) oxide	–	55.83	–	–
per 1 mol of Potassium hydroxide	–	83.75	–	–

Changes in standard condition (2)

Reaction of zinc bromide and potassium permanganate under neutral condition ◆ Δ_rG 168.1 kJ/mol K 0.35 × 10⁻²⁹ pK 29.45: 2ZnBr₂Crystalline solid + 6KMnO₄Crystalline solid + 3H₂OLiquid
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2Zn(OH)₂Crystalline solidβ + 4KBrO₃Crystalline solid + 3Mn₂O₃Crystalline solid + 2KOHCrystalline 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	86.7	168.1	−268.7	–
per 1 mol of Zinc bromide	43.4	84.05	−134.3	–
per 1 mol of Potassium permanganate	14.5	28.02	−44.78	–
per 1 mol of Water	28.9	56.03	−89.57	–
per 1 mol of Zinc hydroxide	43.4	84.05	−134.3	–
per 1 mol of Potassium bromate	21.7	42.02	−67.17	–
per 1 mol of Manganese(III) oxide	28.9	56.03	−89.57	–
per 1 mol of Potassium hydroxide	43.4	84.05	−134.3	–

Changes in standard condition (3)

Reaction of zinc bromide and potassium permanganate under neutral condition ◆ Δ_rG 165.0 kJ/mol K 0.12 × 10⁻²⁸ pK 28.91: 2ZnBr₂Crystalline solid + 6KMnO₄Crystalline solid + 3H₂OLiquid
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2Zn(OH)₂Crystalline solidε + 4KBrO₃Crystalline solid + 3Mn₂O₃Crystalline solid + 2KOHCrystalline 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	84.0	165.0	−267.9	–
per 1 mol of Zinc bromide	42.0	82.50	−133.9	–
per 1 mol of Potassium permanganate	14.0	27.50	−44.65	–
per 1 mol of Water	28.0	55.00	−89.30	–
per 1 mol of Zinc hydroxide	42.0	82.50	−133.9	–
per 1 mol of Potassium bromate	21.0	41.25	−66.97	–
per 1 mol of Manganese(III) oxide	28.0	55.00	−89.30	–
per 1 mol of Potassium hydroxide	42.0	82.50	−133.9	–

Changes in standard condition (4)

Reaction of zinc bromide and potassium permanganate under neutral condition: 2ZnBr₂Crystalline solid + 6KMnO₄Crystalline solid + 3H₂OLiquid
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2Zn(OH)₂Crystalline solidprecipitated + 4KBrO₃Crystalline solid + 3Mn₂O₃Crystalline solid + 2KOHCrystalline 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	86.1	–	–	–
per 1 mol of Zinc bromide	43.0	–	–	–
per 1 mol of Potassium permanganate	14.3	–	–	–
per 1 mol of Water	28.7	–	–	–
per 1 mol of Zinc hydroxide	43.0	–	–	–
per 1 mol of Potassium bromate	21.5	–	–	–
per 1 mol of Manganese(III) oxide	28.7	–	–	–
per 1 mol of Potassium hydroxide	43.0	–	–	–

Changes in aqueous solution (1)

Reaction of zinc bromide and potassium permanganate under neutral condition ◆ Δ_rG 175.9 kJ/mol K 0.15 × 10⁻³⁰ pK 30.82: 2ZnBr₂Ionized aqueous solution + 6KMnO₄Ionized aqueous solution + 3H₂OLiquid
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2Zn(OH)₂Un-ionized aqueous solution + 4KBrO₃Ionized aqueous solution + 3Mn₂O₃Crystalline solid + 2KOHIonized 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	–	175.9	–	–
per 1 mol of Zinc bromide	–	87.95	–	–
per 1 mol of Potassium permanganate	–	29.32	–	–
per 1 mol of Water	–	58.63	–	–
per 1 mol of Zinc hydroxide	–	87.95	–	–
per 1 mol of Potassium bromate	–	43.98	–	–
per 1 mol of Manganese(III) oxide	–	58.63	–	–
per 1 mol of Potassium hydroxide	–	87.95	–	–

Changes in aqueous solution (2)

Reaction of zinc bromide and potassium permanganate under neutral condition ◆ Δ_rG 113.7 kJ/mol K 0.12 × 10⁻¹⁹ pK 19.92: 2ZnBr₂Ionized aqueous solution + 6KMnO₄Ionized aqueous solution + 3H₂OLiquid
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2Zn(OH)₂Crystalline solidγ + 4KBrO₃Ionized aqueous solution + 3Mn₂O₃Crystalline solid + 2KOHIonized 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	–	113.7	–	–
per 1 mol of Zinc bromide	–	56.85	–	–
per 1 mol of Potassium permanganate	–	18.95	–	–
per 1 mol of Water	–	37.90	–	–
per 1 mol of Zinc hydroxide	–	56.85	–	–
per 1 mol of Potassium bromate	–	28.43	–	–
per 1 mol of Manganese(III) oxide	–	37.90	–	–
per 1 mol of Potassium hydroxide	–	56.85	–	–

Changes in aqueous solution (3)

Reaction of zinc bromide and potassium permanganate under neutral condition ◆ Δ_rG 114.3 kJ/mol K 0.95 × 10⁻²⁰ pK 20.02: 2ZnBr₂Ionized aqueous solution + 6KMnO₄Ionized aqueous solution + 3H₂OLiquid
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2Zn(OH)₂Crystalline solidβ + 4KBrO₃Ionized aqueous solution + 3Mn₂O₃Crystalline solid + 2KOHIonized 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	10.9	114.3	−343.4	–
per 1 mol of Zinc bromide	5.45	57.15	−171.7	–
per 1 mol of Potassium permanganate	1.82	19.05	−57.23	–
per 1 mol of Water	3.63	38.10	−114.5	–
per 1 mol of Zinc hydroxide	5.45	57.15	−171.7	–
per 1 mol of Potassium bromate	2.73	28.57	−85.85	–
per 1 mol of Manganese(III) oxide	3.63	38.10	−114.5	–
per 1 mol of Potassium hydroxide	5.45	57.15	−171.7	–

Changes in aqueous solution (4)

Reaction of zinc bromide and potassium permanganate under neutral condition ◆ Δ_rG 111.2 kJ/mol K 0.33 × 10⁻¹⁹ pK 19.48: 2ZnBr₂Ionized aqueous solution + 6KMnO₄Ionized aqueous solution + 3H₂OLiquid
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2Zn(OH)₂Crystalline solidε + 4KBrO₃Ionized aqueous solution + 3Mn₂O₃Crystalline solid + 2KOHIonized 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	8.2	111.2	−342.6	–
per 1 mol of Zinc bromide	4.1	55.60	−171.3	–
per 1 mol of Potassium permanganate	1.4	18.53	−57.10	–
per 1 mol of Water	2.7	37.07	−114.2	–
per 1 mol of Zinc hydroxide	4.1	55.60	−171.3	–
per 1 mol of Potassium bromate	2.0	27.80	−85.65	–
per 1 mol of Manganese(III) oxide	2.7	37.07	−114.2	–
per 1 mol of Potassium hydroxide	4.1	55.60	−171.3	–

Changes in aqueous solution (5)

Reaction of zinc bromide and potassium permanganate under neutral condition: 2ZnBr₂Ionized aqueous solution + 6KMnO₄Ionized aqueous solution + 3H₂OLiquid
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2Zn(OH)₂Crystalline solidprecipitated + 4KBrO₃Ionized aqueous solution + 3Mn₂O₃Crystalline solid + 2KOHIonized 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	10.3	–	–	–
per 1 mol of Zinc bromide	5.15	–	–	–
per 1 mol of Potassium permanganate	1.72	–	–	–
per 1 mol of Water	3.43	–	–	–
per 1 mol of Zinc hydroxide	5.15	–	–	–
per 1 mol of Potassium bromate	2.58	–	–	–
per 1 mol of Manganese(III) oxide	3.43	–	–	–
per 1 mol of Potassium hydroxide	5.15	–	–	–

Changes in aqueous solution (6)

Reaction of zinc bromide and potassium permanganate under neutral condition ◆ Δ_rG 164.7 kJ/mol K 0.14 × 10⁻²⁸ pK 28.85: 2ZnBr₂Un-ionized aqueous solution + 6KMnO₄Ionized aqueous solution + 3H₂OLiquid
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2Zn(OH)₂Un-ionized aqueous solution + 4KBrO₃Ionized aqueous solution + 3Mn₂O₃Crystalline solid + 2KOHIonized 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	–	164.7	–	–
per 1 mol of Zinc bromide	–	82.35	–	–
per 1 mol of Potassium permanganate	–	27.45	–	–
per 1 mol of Water	–	54.90	–	–
per 1 mol of Zinc hydroxide	–	82.35	–	–
per 1 mol of Potassium bromate	–	41.17	–	–
per 1 mol of Manganese(III) oxide	–	54.90	–	–
per 1 mol of Potassium hydroxide	–	82.35	–	–

Changes in aqueous solution (7)

Reaction of zinc bromide and potassium permanganate under neutral condition ◆ Δ_rG 102.6 kJ/mol K 0.11 × 10⁻¹⁷ pK 17.97: 2ZnBr₂Un-ionized aqueous solution + 6KMnO₄Ionized aqueous solution + 3H₂OLiquid
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2Zn(OH)₂Crystalline solidγ + 4KBrO₃Ionized aqueous solution + 3Mn₂O₃Crystalline solid + 2KOHIonized 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	–	102.6	–	–
per 1 mol of Zinc bromide	–	51.30	–	–
per 1 mol of Potassium permanganate	–	17.10	–	–
per 1 mol of Water	–	34.20	–	–
per 1 mol of Zinc hydroxide	–	51.30	–	–
per 1 mol of Potassium bromate	–	25.65	–	–
per 1 mol of Manganese(III) oxide	–	34.20	–	–
per 1 mol of Potassium hydroxide	–	51.30	–	–

Changes in aqueous solution (8)

Reaction of zinc bromide and potassium permanganate under neutral condition ◆ Δ_rG 103.2 kJ/mol K 0.83 × 10⁻¹⁸ pK 18.08: 2ZnBr₂Un-ionized aqueous solution + 6KMnO₄Ionized aqueous solution + 3H₂OLiquid
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2Zn(OH)₂Crystalline solidβ + 4KBrO₃Ionized aqueous solution + 3Mn₂O₃Crystalline solid + 2KOHIonized 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	–	103.2	–	–
per 1 mol of Zinc bromide	–	51.60	–	–
per 1 mol of Potassium permanganate	–	17.20	–	–
per 1 mol of Water	–	34.40	–	–
per 1 mol of Zinc hydroxide	–	51.60	–	–
per 1 mol of Potassium bromate	–	25.80	–	–
per 1 mol of Manganese(III) oxide	–	34.40	–	–
per 1 mol of Potassium hydroxide	–	51.60	–	–

Changes in aqueous solution (9)

Reaction of zinc bromide and potassium permanganate under neutral condition ◆ Δ_rG 100.1 kJ/mol K 0.29 × 10⁻¹⁷ pK 17.54: 2ZnBr₂Un-ionized aqueous solution + 6KMnO₄Ionized aqueous solution + 3H₂OLiquid
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2Zn(OH)₂Crystalline solidε + 4KBrO₃Ionized aqueous solution + 3Mn₂O₃Crystalline solid + 2KOHIonized 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	–	100.1	–	–
per 1 mol of Zinc bromide	–	50.05	–	–
per 1 mol of Potassium permanganate	–	16.68	–	–
per 1 mol of Water	–	33.37	–	–
per 1 mol of Zinc hydroxide	–	50.05	–	–
per 1 mol of Potassium bromate	–	25.02	–	–
per 1 mol of Manganese(III) oxide	–	33.37	–	–
per 1 mol of Potassium hydroxide	–	50.05	–	–

Changes in aqueous solution (10)

Reaction of zinc bromide and potassium permanganate under neutral condition: 2ZnBr₂Un-ionized aqueous solution + 6KMnO₄Ionized aqueous solution + 3H₂OLiquid
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⟶
2Zn(OH)₂Crystalline solidprecipitated + 4KBrO₃Ionized aqueous solution + 3Mn₂O₃Crystalline solid + 2KOHIonized 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	–	–	–	–
per 1 mol of Zinc bromide	–	–	–	–
per 1 mol of Potassium permanganate	–	–	–	–
per 1 mol of Water	–	–	–	–
per 1 mol of Zinc hydroxide	–	–	–	–
per 1 mol of Potassium bromate	–	–	–	–
per 1 mol of Manganese(III) oxide	–	–	–	–
per 1 mol of Potassium hydroxide	–	–	–	–

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
ZnBr₂ (cr)	-328.65^[1]	-312.13^[1]	138.5^[1]	–
ZnBr₂ (ai)	-396.98^[1]	-354.97^[1]	52.7^[1]	-238^[1]
ZnBr₂ (ao)	–	-349.4^[1]	–	–
ZnBr₂ (cr) 2 hydrate	-937.2^[1]	-799.5^[1]	198.7^[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, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas

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
Zn(OH)₂ (cr) γ	–	-553.81^[1]	–	–
Zn(OH)₂ (cr) β	-641.91^[1]	-553.52^[1]	81.2^[1]	–
Zn(OH)₂ (cr) ε	-643.25^[1]	-555.07^[1]	81.6^[1]	72.4^[1]
Zn(OH)₂ (cr) precipitated	-642.2^[1]	–	–	–
Zn(OH)₂ (ai)	-613.88^[1]	-461.56^[1]	-133.5^[1]	-251^[1]
Zn(OH)₂ (ao)	–	-522.73^[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]	–
Mn₂O₃ (cr)	-959.0^[1]	-881.1^[1]	110.5^[1]	107.65^[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]	–

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

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	167.5 kJ/mol
K	0.45 × 10⁻²⁹
pK	29.34

Δ_rG	168.1 kJ/mol
K	0.35 × 10⁻²⁹
pK	29.45

Δ_rG	165.0 kJ/mol
K	0.12 × 10⁻²⁸
pK	28.91

Δ_rG	175.9 kJ/mol
K	0.15 × 10⁻³⁰
pK	30.82

2ZnBr2 + 6KMnO4 + 3H2O 🔥→ 2Zn(OH)2 + 4KBrO3 + 3Mn2O3 + 2KOH

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 (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)

Changes in aqueous solution (9)

Changes in aqueous solution (10)

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

2ZnBr₂ + 6KMnO₄ + 3H₂O 🔥→ 2Zn(OH)₂ + 4KBrO₃ + 3Mn₂O₃ + 2KOH