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5SrBr2 + 2KMnO4 🔥→ 5SrO + 5Br2 + 2MnO + K2O

The reaction of strontium bromide and potassium permanganate yields strontium oxide, bromine, manganese(II) oxide, and potassium oxide (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
Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
SrBr2Strontium bromide5
Reducing
Hardly oxidizable
KMnO4Potassium permanganate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SrOStrontium oxide5
Br2Bromine5
Oxidized
MnOManganese(II) oxide2
Reduced
K2OPotassium oxide1

Thermodynamic changes

Changes in standard condition

Reaction of strontium bromide and potassium permanganate
ΔrG1103.3 kJ/mol
K0.51 × 10−193
pK193.29
5SrBr2Crystalline solid + 2KMnO4Crystalline solid
🔥
5SrOCrystalline solid + 5Br2Liquid + 2MnOCrystalline solid + K2OCrystalline 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
1170.51103.3227.8166.2
per 1 mol of
234.10220.6645.5633.24
585.25551.65113.983.10
per 1 mol of
234.10220.6645.5633.24
per 1 mol of
234.10220.6645.5633.24
585.25551.65113.983.10
per 1 mol of
1170.51103.3227.8166.2

Changes in aqueous solution

Reaction of strontium bromide and potassium permanganate
ΔrG1460.2 kJ/mol
K0.15 × 10−255
pK255.82
5SrBr2Ionized aqueous solution + 2KMnO4Ionized aqueous solution
🔥
5SrOCrystalline solid + 5Br2Un-ionized aqueous solution + 2MnOCrystalline solid + K2OCrystalline 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
1427.21460.2−110.4
per 1 mol of
285.44292.04−22.08
713.60730.10−55.20
per 1 mol of
285.44292.04−22.08
per 1 mol of
285.44292.04−22.08
713.60730.10−55.20
per 1 mol of
1427.21460.2−110.4

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
SrBr2 (cr)-717.6[1]-697.1[1]135.10[1]75.35[1]
SrBr2 (g)-410[1]-444[1]323.5[1]60.7[1]
SrBr2 (ai)-788.89[1]-767.39[1]132.2[1]
SrBr2 (cr)
1 hydrate
-1031.4[1]-954.3[1]180[1]120.9[1]
SrBr2 (cr)
6 hydrate
-2531.3[1]-2174.1[1]406[1]343.5[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]
* (cr):Crystalline solid, (g):Gas, (ai):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
SrO (cr)-592.0[1]-561.9[1]54.4[1]45.02[1]
SrO (g)-8[1]
Br2 (cr)
Br2 (l)0[1]0[1]152.231[1]75.689[1]
Br2 (g)30.907[1]3.110[1]245.463[1]36.02[1]
Br2 (ao)-2.59[1]3.93[1]130.5[1]
MnO (cr)-385.22[1]-362.90[1]59.71[1]45.44[1]
MnO (g)124.22[1]
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]
* (cr):Crystalline solid, (g):Gas, (l):Liquid, (ao):Un-ionized aqueous solution

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)

  2. 2
    James G. Speight (2017)
    Lange's Handbook of Chemistry, 17th edition
    McGraw Hill Education