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3ZnBr2 + 6KMnO4 + 9H2O 🔥→ 3Zn(OH)2 + 5KBrO3 + 6Mn(OH)2 + KBr

The reaction of zinc bromide, potassium permanganate, and water yields zinc hydroxide, potassium bromate, manganese(II) hydroxide, and potassium bromide (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

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 bromide3
Reducing
Hardly oxidizable
KMnO4Potassium permanganate6
Oxidizing
Oxidizing
H2OWater9
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Zn(OH)2Zinc hydroxide3
KBrO3Potassium bromate5
Oxidized
Mn(OH)2Manganese(II) hydroxide6
Reduced
KBrPotassium bromide1

Thermodynamic changes

Changes in standard condition (1)

Reaction of zinc bromide and potassium permanganate under neutral condition
ΔrG408.3 kJ/mol
K0.29 × 10−71
pK71.53
3ZnBr2Crystalline solid + 6KMnO4Crystalline solid + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidγ + 5KBrO3Crystalline solid + 6Mn(OH)2Amorphous solidprecipitated + KBrCrystalline 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
408.3
per 1 mol of
136.1
68.05
per 1 mol of
45.37
per 1 mol of
136.1
per 1 mol of
81.66
68.05
per 1 mol of
408.3

Changes in standard condition (2)

Reaction of zinc bromide and potassium permanganate under neutral condition
ΔrG409.1 kJ/mol
K0.21 × 10−71
pK71.67
3ZnBr2Crystalline solid + 6KMnO4Crystalline solid + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidβ + 5KBrO3Crystalline solid + 6Mn(OH)2Amorphous solidprecipitated + KBrCrystalline 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
288.5409.1−394.5
per 1 mol of
96.17136.4−131.5
48.0868.18−65.75
per 1 mol of
32.0645.46−43.83
per 1 mol of
96.17136.4−131.5
per 1 mol of
57.7081.82−78.90
48.0868.18−65.75
per 1 mol of
288.5409.1−394.5

Changes in standard condition (3)

Reaction of zinc bromide and potassium permanganate under neutral condition
ΔrG404.5 kJ/mol
K0.14 × 10−70
pK70.87
3ZnBr2Crystalline solid + 6KMnO4Crystalline solid + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidε + 5KBrO3Crystalline solid + 6Mn(OH)2Amorphous solidprecipitated + KBrCrystalline 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
284.5404.5−393.3
per 1 mol of
94.83134.8−131.1
47.4267.42−65.55
per 1 mol of
31.6144.94−43.70
per 1 mol of
94.83134.8−131.1
per 1 mol of
56.9080.90−78.66
47.4267.42−65.55
per 1 mol of
284.5404.5−393.3

Changes in standard condition (4)

Reaction of zinc bromide and potassium permanganate under neutral condition
3ZnBr2Crystalline solid + 6KMnO4Crystalline solid + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidprecipitated + 5KBrO3Crystalline solid + 6Mn(OH)2Amorphous solidprecipitated + KBrCrystalline 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
287.6
per 1 mol of
95.87
47.93
per 1 mol of
31.96
per 1 mol of
95.87
per 1 mol of
57.52
47.93
per 1 mol of
287.6

Changes in aqueous solution (1)

Reaction of zinc bromide and potassium permanganate under neutral condition
ΔrG613.3 kJ/mol
K0.36 × 10−107
pK107.45
3ZnBr2Ionized aqueous solution + 6KMnO4Ionized aqueous solution + 9H2OLiquid
🔥
3Zn(OH)2Un-ionized aqueous solution + 5KBrO3Ionized aqueous solution + 6Mn(OH)2Amorphous solidprecipitated + KBrIonized 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
613.3
per 1 mol of
204.4
102.2
per 1 mol of
68.14
per 1 mol of
204.4
per 1 mol of
122.7
102.2
per 1 mol of
613.3

Changes in aqueous solution (2)

Reaction of zinc bromide and potassium permanganate under neutral condition
ΔrG520.1 kJ/mol
K0.76 × 10−91
pK91.12
3ZnBr2Ionized aqueous solution + 6KMnO4Ionized aqueous solution + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidγ + 5KBrO3Ionized aqueous solution + 6Mn(OH)2Amorphous solidprecipitated + KBrIonized 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
520.1
per 1 mol of
173.4
86.68
per 1 mol of
57.79
per 1 mol of
173.4
per 1 mol of
104.0
86.68
per 1 mol of
520.1

Changes in aqueous solution (3)

Reaction of zinc bromide and potassium permanganate under neutral condition
ΔrG520.9 kJ/mol
K0.55 × 10−91
pK91.26
3ZnBr2Ionized aqueous solution + 6KMnO4Ionized aqueous solution + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidβ + 5KBrO3Ionized aqueous solution + 6Mn(OH)2Amorphous solidprecipitated + KBrIonized 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
456.9520.9−204.7
per 1 mol of
152.3173.6−68.23
76.1586.82−34.12
per 1 mol of
50.7757.88−22.74
per 1 mol of
152.3173.6−68.23
per 1 mol of
91.38104.2−40.94
76.1586.82−34.12
per 1 mol of
456.9520.9−204.7

Changes in aqueous solution (4)

Reaction of zinc bromide and potassium permanganate under neutral condition
ΔrG516.3 kJ/mol
K0.35 × 10−90
pK90.45
3ZnBr2Ionized aqueous solution + 6KMnO4Ionized aqueous solution + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidε + 5KBrO3Ionized aqueous solution + 6Mn(OH)2Amorphous solidprecipitated + KBrIonized 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
452.9516.3−203.5
per 1 mol of
151.0172.1−67.83
75.4886.05−33.92
per 1 mol of
50.3257.37−22.61
per 1 mol of
151.0172.1−67.83
per 1 mol of
90.58103.3−40.70
75.4886.05−33.92
per 1 mol of
452.9516.3−203.5

Changes in aqueous solution (5)

Reaction of zinc bromide and potassium permanganate under neutral condition
3ZnBr2Ionized aqueous solution + 6KMnO4Ionized aqueous solution + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidprecipitated + 5KBrO3Ionized aqueous solution + 6Mn(OH)2Amorphous solidprecipitated + KBrIonized 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
456.0
per 1 mol of
152.0
76.00
per 1 mol of
50.67
per 1 mol of
152.0
per 1 mol of
91.20
76.00
per 1 mol of
456.0

Changes in aqueous solution (6)

Reaction of zinc bromide and potassium permanganate under neutral condition
ΔrG596.6 kJ/mol
K0.30 × 10−104
pK104.52
3ZnBr2Un-ionized aqueous solution + 6KMnO4Ionized aqueous solution + 9H2OLiquid
🔥
3Zn(OH)2Un-ionized aqueous solution + 5KBrO3Ionized aqueous solution + 6Mn(OH)2Amorphous solidprecipitated + KBrIonized 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
596.6
per 1 mol of
198.9
99.43
per 1 mol of
66.29
per 1 mol of
198.9
per 1 mol of
119.3
99.43
per 1 mol of
596.6

Changes in aqueous solution (7)

Reaction of zinc bromide and potassium permanganate under neutral condition
ΔrG503.4 kJ/mol
K0.64 × 10−88
pK88.19
3ZnBr2Un-ionized aqueous solution + 6KMnO4Ionized aqueous solution + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidγ + 5KBrO3Ionized aqueous solution + 6Mn(OH)2Amorphous solidprecipitated + KBrIonized 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
503.4
per 1 mol of
167.8
83.90
per 1 mol of
55.93
per 1 mol of
167.8
per 1 mol of
100.7
83.90
per 1 mol of
503.4

Changes in aqueous solution (8)

Reaction of zinc bromide and potassium permanganate under neutral condition
ΔrG504.2 kJ/mol
K0.47 × 10−88
pK88.33
3ZnBr2Un-ionized aqueous solution + 6KMnO4Ionized aqueous solution + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidβ + 5KBrO3Ionized aqueous solution + 6Mn(OH)2Amorphous solidprecipitated + KBrIonized 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
504.2
per 1 mol of
168.1
84.03
per 1 mol of
56.02
per 1 mol of
168.1
per 1 mol of
100.8
84.03
per 1 mol of
504.2

Changes in aqueous solution (9)

Reaction of zinc bromide and potassium permanganate under neutral condition
ΔrG499.6 kJ/mol
K0.30 × 10−87
pK87.53
3ZnBr2Un-ionized aqueous solution + 6KMnO4Ionized aqueous solution + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidε + 5KBrO3Ionized aqueous solution + 6Mn(OH)2Amorphous solidprecipitated + KBrIonized 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
499.6
per 1 mol of
166.5
83.27
per 1 mol of
55.51
per 1 mol of
166.5
per 1 mol of
99.92
83.27
per 1 mol of
499.6

Changes in aqueous solution (10)

Reaction of zinc bromide and potassium permanganate under neutral condition
3ZnBr2Un-ionized aqueous solution + 6KMnO4Ionized aqueous solution + 9H2OLiquid
🔥
3Zn(OH)2Crystalline solidprecipitated + 5KBrO3Ionized aqueous solution + 6Mn(OH)2Amorphous solidprecipitated + KBrIonized 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
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]
Mn(OH)2 (am)
precipitated
-695.4[1]-615.0[1]99.2[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, (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)