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3SrS + 8KMnO4 → 3SrSO4 + 8MnO2 + 4K2O

The reaction of strontium sulfide and potassium permanganate yields strontium sulfate, manganese(IV) 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 reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
SrSStrontium sulfide3
Reducing
Reducing
KMnO4Potassium permanganate8
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SrSO4Strontium sulfate3
Oxidized
MnO2Manganese(IV) oxide8
Reduced
K2OPotassium oxide4

Thermodynamic changes

Changes in standard condition (1)

Reaction of strontium sulfide and potassium permanganate
ΔrG−1728.0 kJ/mol
K5.40 × 10302
pK−302.73
3SrSCrystalline solid + 8KMnO4Crystalline solid
3SrSO4Crystalline solid + 8MnO2Crystalline solid + 4K2OCrystalline 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
−1850.7−1728.0−426
per 1 mol of
−616.90−576.00−142
−231.34−216.00−53.3
per 1 mol of
−616.90−576.00−142
−231.34−216.00−53.3
per 1 mol of
−462.68−432.00−107

Changes in standard condition (2)

Reaction of strontium sulfide and potassium permanganate
3SrSCrystalline solid + 8KMnO4Crystalline solid
3SrSO4Crystalline solid + 8MnO2Amorphous solidprecipitated + 4K2OCrystalline 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
−1710.5
per 1 mol of
−570.17
−213.81
per 1 mol of
−570.17
−213.81
per 1 mol of
−427.63

Changes in standard condition (3)

Reaction of strontium sulfide and potassium permanganate
3SrSCrystalline solid + 8KMnO4Crystalline solid
3SrSO4Crystalline solidprecipitated + 8MnO2Crystalline solid + 4K2OCrystalline 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
−1840.8
per 1 mol of
−613.60
−230.10
per 1 mol of
−613.60
−230.10
per 1 mol of
−460.20

Changes in standard condition (4)

Reaction of strontium sulfide and potassium permanganate
3SrSCrystalline solid + 8KMnO4Crystalline solid
3SrSO4Crystalline solidprecipitated + 8MnO2Amorphous solidprecipitated + 4K2OCrystalline 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
−1700.6
per 1 mol of
−566.87
−212.57
per 1 mol of
−566.87
−212.57
per 1 mol of
−425.15

Changes in aqueous solution (1)

Reaction of strontium sulfide and potassium permanganate
ΔrG−1784.8 kJ/mol
K4.82 × 10312
pK−312.68
3SrSCrystalline solid + 8KMnO4Ionized aqueous solution
3SrSO4Crystalline solid + 8MnO2Crystalline solid + 4K2OCrystalline 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
−2197.9−1784.8−1402
per 1 mol of
−732.63−594.93−467.3
−274.74−223.10−175.3
per 1 mol of
−732.63−594.93−467.3
−274.74−223.10−175.3
per 1 mol of
−549.48−446.20−350.5

Changes in aqueous solution (2)

Reaction of strontium sulfide and potassium permanganate
3SrSCrystalline solid + 8KMnO4Ionized aqueous solution
3SrSO4Crystalline solidprecipitated + 8MnO2Crystalline solid + 4K2OCrystalline 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
−2188.0
per 1 mol of
−729.33
−273.50
per 1 mol of
−729.33
−273.50
per 1 mol of
−547.00

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
SrS (cr)-472.4[1]-467.8[1]68.2[1]48.70[1]
SrS (g)109[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
SrSO4 (cr)-1453.1[1]-1340.9[1]117[1]
SrSO4 (cr)
precipitated
-1449.8[1]
SrSO4 (ai)-1455.07[1]-1304.00[1]-12.6[1]
MnO2 (cr)-520.03[1]-465.14[1]53.05[1]54.14[1]
MnO2 (am)
precipitated
-502.5[1]
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid, (g):Gas

References

List of references

  1. 1
  2. 2
    James G. Speight (2017)
    Lange's Handbook of Chemistry, 17th edition
    McGraw Hill Education