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ZnBr2 + 4KMnO4 + 2H2O → Zn(OH)2 + 2KBrO3 + 4MnO2 + 2KOH

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Reaction of zinc bromide and potassium permanganate under neutral condition
ZnBr2Zinc bromide + 4KMnO4Potassium permanganate + 2H2OWater
⟶
Zn(OH)2Zinc hydroxide + 2KBrO3Potassium bromate + 4MnO2Manganese(IV) oxide + 2KOHPotassium hydroxide

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

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

Reaction of zinc bromide and potassium permanganate under neutral condition
ZnBr2Zinc bromide + 4KMnO4Potassium permanganate + 2H2OWater
⟶
Zn(OH)2Zinc hydroxide + 2KBrO3Potassium bromate + 4MnO2Manganese(IV) 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
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of zinc bromide and potassium permanganate under neutral condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
ZnBr2Zinc bromide1
Reducing
Hardly oxidizable
KMnO4Potassium permanganate4
Oxidizing
Oxidizing
H2OWater2
–
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Zn(OH)2Zinc hydroxide1
–
–
KBrO3Potassium bromate2
Oxidized
–
MnO2Manganese(IV) oxide4
Reduced
–
KOHPotassium hydroxide2
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of zinc bromide and potassium permanganate under neutral condition
◆
ΔrG21.9 kJ/mol
K0.15 × 10−3
pK3.84
ZnBr2Crystalline solid + 4KMnO4Crystalline solid + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidγ + 2KBrO3Crystalline solid + 4MnO2Crystalline solid + 2KOHCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
–21.9––
per 1 mol of
–21.9––
–5.47––
per 1 mol of
–10.9––
per 1 mol of
–21.9––
per 1 mol of
–10.9––
–5.47––
–10.9––

Changes in standard condition (2)

Reaction of zinc bromide and potassium permanganate under neutral condition
ZnBr2Crystalline solid + 4KMnO4Crystalline solid + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidγ + 2KBrO3Crystalline solid + 4MnO2Amorphous solidprecipitated + 2KOHCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
––––
per 1 mol of
––––
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––
––––
––––

Changes in standard condition (3)

Reaction of zinc bromide and potassium permanganate under neutral condition
◆
ΔrG22.2 kJ/mol
K0.13 × 10−3
pK3.89
ZnBr2Crystalline solid + 4KMnO4Crystalline solid + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidβ + 2KBrO3Crystalline solid + 4MnO2Crystalline solid + 2KOHCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−42.922.2−215.6–
per 1 mol of
−42.922.2−215.6–
−10.75.55−53.90–
per 1 mol of
−21.411.1−107.8–
per 1 mol of
−42.922.2−215.6–
per 1 mol of
−21.411.1−107.8–
−10.75.55−53.90–
−21.411.1−107.8–

Changes in standard condition (4)

Reaction of zinc bromide and potassium permanganate under neutral condition
ZnBr2Crystalline solid + 4KMnO4Crystalline solid + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidβ + 2KBrO3Crystalline solid + 4MnO2Amorphous solidprecipitated + 2KOHCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
27.2–––
per 1 mol of
27.2–––
6.80–––
per 1 mol of
13.6–––
per 1 mol of
27.2–––
per 1 mol of
13.6–––
6.80–––
13.6–––

Changes in standard condition (5)

Reaction of zinc bromide and potassium permanganate under neutral condition
◆
ΔrG20.7 kJ/mol
K0.24 × 10−3
pK3.63
ZnBr2Crystalline solid + 4KMnO4Crystalline solid + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidε + 2KBrO3Crystalline solid + 4MnO2Crystalline solid + 2KOHCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−44.320.7−215.2–
per 1 mol of
−44.320.7−215.2–
−11.15.17−53.80–
per 1 mol of
−22.110.3−107.6–
per 1 mol of
−44.320.7−215.2–
per 1 mol of
−22.110.3−107.6–
−11.15.17−53.80–
−22.110.3−107.6–

Changes in standard condition (6)

Reaction of zinc bromide and potassium permanganate under neutral condition
ZnBr2Crystalline solid + 4KMnO4Crystalline solid + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidε + 2KBrO3Crystalline solid + 4MnO2Amorphous solidprecipitated + 2KOHCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
25.9–––
per 1 mol of
25.9–––
6.47–––
per 1 mol of
12.9–––
per 1 mol of
25.9–––
per 1 mol of
12.9–––
6.47–––
12.9–––

Changes in standard condition (7)

Reaction of zinc bromide and potassium permanganate under neutral condition
ZnBr2Crystalline solid + 4KMnO4Crystalline solid + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidprecipitated + 2KBrO3Crystalline solid + 4MnO2Crystalline solid + 2KOHCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−43.2–––
per 1 mol of
−43.2–––
−10.8–––
per 1 mol of
−21.6–––
per 1 mol of
−43.2–––
per 1 mol of
−21.6–––
−10.8–––
−21.6–––

Changes in standard condition (8)

Reaction of zinc bromide and potassium permanganate under neutral condition
ZnBr2Crystalline solid + 4KMnO4Crystalline solid + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidprecipitated + 2KBrO3Crystalline solid + 4MnO2Amorphous solidprecipitated + 2KOHCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
26.9–––
per 1 mol of
26.9–––
6.72–––
per 1 mol of
13.4–––
per 1 mol of
26.9–––
per 1 mol of
13.4–––
6.72–––
13.4–––

Changes in aqueous solution (1)

Reaction of zinc bromide and potassium permanganate under neutral condition
◆
ΔrG−42.4 kJ/mol
K2.68 × 107
pK−7.43
ZnBr2Ionized aqueous solution + 4KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
Zn(OH)2Un-ionized aqueous solution + 2KBrO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
–−42.4––
per 1 mol of
–−42.4––
–−10.6––
per 1 mol of
–−21.2––
per 1 mol of
–−42.4––
per 1 mol of
–−21.2––
–−10.6––
–−21.2––

Changes in aqueous solution (2)

Reaction of zinc bromide and potassium permanganate under neutral condition
◆
ΔrG−73.5 kJ/mol
K7.53 × 1012
pK−12.88
ZnBr2Ionized aqueous solution + 4KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidγ + 2KBrO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
–−73.5––
per 1 mol of
–−73.5––
–−18.4––
per 1 mol of
–−36.8––
per 1 mol of
–−73.5––
per 1 mol of
–−36.8––
–−18.4––
–−36.8––

Changes in aqueous solution (3)

Reaction of zinc bromide and potassium permanganate under neutral condition
◆
ΔrG−73.2 kJ/mol
K6.67 × 1012
pK−12.82
ZnBr2Ionized aqueous solution + 4KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidβ + 2KBrO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−181.8−73.2−362.3–
per 1 mol of
−181.8−73.2−362.3–
−45.45−18.3−90.58–
per 1 mol of
−90.90−36.6−181.2–
per 1 mol of
−181.8−73.2−362.3–
per 1 mol of
−90.90−36.6−181.2–
−45.45−18.3−90.58–
−90.90−36.6−181.2–

Changes in aqueous solution (4)

Reaction of zinc bromide and potassium permanganate under neutral condition
◆
ΔrG−74.7 kJ/mol
K1.22 × 1013
pK−13.09
ZnBr2Ionized aqueous solution + 4KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidε + 2KBrO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−183.2−74.7−361.9–
per 1 mol of
−183.2−74.7−361.9–
−45.80−18.7−90.47–
per 1 mol of
−91.60−37.4−180.9–
per 1 mol of
−183.2−74.7−361.9–
per 1 mol of
−91.60−37.4−180.9–
−45.80−18.7−90.47–
−91.60−37.4−180.9–

Changes in aqueous solution (5)

Reaction of zinc bromide and potassium permanganate under neutral condition
ZnBr2Ionized aqueous solution + 4KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidprecipitated + 2KBrO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−182.1–––
per 1 mol of
−182.1–––
−45.52–––
per 1 mol of
−91.05–––
per 1 mol of
−182.1–––
per 1 mol of
−91.05–––
−45.52–––
−91.05–––

Changes in aqueous solution (6)

Reaction of zinc bromide and potassium permanganate under neutral condition
◆
ΔrG−48.0 kJ/mol
K2.57 × 108
pK−8.41
ZnBr2Un-ionized aqueous solution + 4KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
Zn(OH)2Un-ionized aqueous solution + 2KBrO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
–−48.0––
per 1 mol of
–−48.0––
–−12.0––
per 1 mol of
–−24.0––
per 1 mol of
–−48.0––
per 1 mol of
–−24.0––
–−12.0––
–−24.0––

Changes in aqueous solution (7)

Reaction of zinc bromide and potassium permanganate under neutral condition
◆
ΔrG−79.1 kJ/mol
K7.21 × 1013
pK−13.86
ZnBr2Un-ionized aqueous solution + 4KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidγ + 2KBrO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
–−79.1––
per 1 mol of
–−79.1––
–−19.8––
per 1 mol of
–−39.5––
per 1 mol of
–−79.1––
per 1 mol of
–−39.5––
–−19.8––
–−39.5––

Changes in aqueous solution (8)

Reaction of zinc bromide and potassium permanganate under neutral condition
◆
ΔrG−78.8 kJ/mol
K6.39 × 1013
pK−13.81
ZnBr2Un-ionized aqueous solution + 4KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidβ + 2KBrO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
–−78.8––
per 1 mol of
–−78.8––
–−19.7––
per 1 mol of
–−39.4––
per 1 mol of
–−78.8––
per 1 mol of
–−39.4––
–−19.7––
–−39.4––

Changes in aqueous solution (9)

Reaction of zinc bromide and potassium permanganate under neutral condition
◆
ΔrG−80.3 kJ/mol
K1.17 × 1014
pK−14.07
ZnBr2Un-ionized aqueous solution + 4KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidε + 2KBrO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
–−80.3––
per 1 mol of
–−80.3––
–−20.1––
per 1 mol of
–−40.1––
per 1 mol of
–−80.3––
per 1 mol of
–−40.1––
–−20.1––
–−40.1––

Changes in aqueous solution (10)

Reaction of zinc bromide and potassium permanganate under neutral condition
ZnBr2Un-ionized aqueous solution + 4KMnO4Ionized aqueous solution + 2H2OLiquid
⟶
Zn(OH)2Crystalline solidprecipitated + 2KBrO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
––––
per 1 mol of
––––
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––
––––
––––

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
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 formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
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]–
MnO2 (cr)-520.03[1]-465.14[1]53.05[1]54.14[1]
MnO2 (am)
precipitated
-502.5[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, (am):Amorphous solid, (g):Gas

References

List of references

  1. 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
    National Institute of Standards and Technology (NIST)