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5FeBr2 + KMnO4 + 18H+ → 5Fe3+ + Mn2+ + 10HBr↑ + K+ + 4H2O

Reaction of iron(II) bromide and potassium permanganate under acidic condition
5FeBr2Iron(II) bromide + KMnO4Potassium permanganate + 18H+Hydrogen ion
5Fe3+Iron(III) ion + Mn2+Manganese(II) ion + 10HBrHydrogen bromide + K+Potassium ion + 4H2OWater

The reaction of iron(II) bromide, potassium permanganate, and hydrogen ion yields iron(III) ion, manganese(II) ion, hydrogen bromide, potassium ion, and water (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 iron(II) bromide and potassium permanganate under acidic condition
5FeBr2Iron(II) bromide + KMnO4Potassium permanganate + 18H+Hydrogen ion
5Fe3+Iron(III) ion + Mn2+Manganese(II) ion + 10HBrHydrogen bromide + K+Potassium ion + 4H2OWater

General equation

Reaction of oxidizable species and oxidizing species under acidic condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent
ProductOxidation product + ProductReduction product + H2ONon-redox product

Oxidation state of each atom

Reaction of iron(II) bromide and potassium permanganate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeBr2Iron(II) bromide5
Reducing
Oxidizable
KMnO4Potassium permanganate1
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion18
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe3+Iron(III) ion5
Oxidized
Mn2+Manganese(II) ion1
Reduced
HBrHydrogen bromide10
K+Potassium ion1
H2OWater4
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) bromide and potassium permanganate under acidic condition
ΔrG146.7 kJ/mol
K0.20 × 10−25
pK25.70
5FeBr2Ionized aqueous solution + KMnO4Ionized aqueous solution + 18H+Un-ionized aqueous solution
5Fe3+Un-ionized aqueous solution + Mn2+Un-ionized aqueous solution + 10HBrGas + K+Un-ionized aqueous solution + 4H2OLiquid
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
231.9146.7286.3
per 1 mol of
46.3829.3457.26
231.9146.7286.3
per 1 mol of
Hydrogen ion
12.888.15015.91
per 1 mol of
Iron(III) ion
46.3829.3457.26
per 1 mol of
Manganese(II) ion
231.9146.7286.3
per 1 mol of
23.1914.6728.63
per 1 mol of
Potassium ion
231.9146.7286.3
per 1 mol of
57.9836.6771.58

Changes in standard condition (2)

Reaction of iron(II) bromide and potassium permanganate under acidic condition
ΔrG−358.4 kJ/mol
K6.15 × 1062
pK−62.79
5FeBr2Ionized aqueous solution + KMnO4Ionized aqueous solution + 18H+Un-ionized aqueous solution
5Fe3+Un-ionized aqueous solution + Mn2+Un-ionized aqueous solution + 10HBrIonized aqueous solution + K+Un-ionized aqueous solution + 4H2OLiquid
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
−619.7−358.4−876.7
per 1 mol of
−123.9−71.68−175.3
−619.7−358.4−876.7
per 1 mol of
Hydrogen ion
−34.43−19.91−48.71
per 1 mol of
Iron(III) ion
−123.9−71.68−175.3
per 1 mol of
Manganese(II) ion
−619.7−358.4−876.7
per 1 mol of
−61.97−35.84−87.67
per 1 mol of
Potassium ion
−619.7−358.4−876.7
per 1 mol of
−154.9−89.60−219.2

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
FeBr2 (cr)-249.8[1]-238.1[1]140.6[1]
FeBr2 (g)-46[1]
FeBr2 (ai)-332.2[1]-286.81[1]27.2[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]
H+ (g)1536.202[1]
H+ (ao)0[1]0[1]0[1]0[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

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
Fe3+ (g)5712.8[1]
Fe3+ (ao)-48.5[1]-4.7[1]-315.9[1]
Mn2+ (g)2519.69[1]
Mn2+ (ao)-220.75[1]-228.1[1]-73.6[1]50[1]
HBr (g)-36.40[1]-53.45[1]198.695[1]29.142[1]
HBr (ai)-121.55[1]-103.96[1]82.4[1]-141.8[1]
K+ (g)514.26[1]
K+ (ao)-252.38[1]-283.27[1]102.5[1]21.8[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, (ao):Un-ionized aqueous solution, (ai):Ionized aqueous solution, (cr):Crystalline solid, (l):Liquid

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)