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7SnS + 4KMnO4 → 7SnO2 + SO2↑ + 4MnS + 2K2S

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Reaction of tin(II) sulfide and potassium permanganate
7SnSTin(II) sulfide + 4KMnO4Potassium permanganate
⟶
7SnO2Tin(IV) oxide + SO2↑Sulfur dioxide + 4MnSManganese(II) sulfide + 2K2SPotassium sulfide

The reaction of tin(II) sulfide and potassium permanganate yields tin(IV) oxide, sulfur dioxide, manganese(II) sulfide, and potassium sulfide (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 tin(II) sulfide and potassium permanganate
7SnSTin(II) sulfide + 4KMnO4Potassium permanganate
⟶
7SnO2Tin(IV) oxide + SO2↑Sulfur dioxide + 4MnSManganese(II) sulfide + 2K2SPotassium sulfide

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of tin(II) sulfide and potassium permanganate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
SnSTin(II) sulfide7
Reducing
Reducing
KMnO4Potassium permanganate4
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SnO2Tin(IV) oxide7
Oxidized
–
SO2Sulfur dioxide1
Oxidized
–
MnSManganese(II) sulfide4
Reduced
–
K2SPotassium sulfide2
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of tin(II) sulfide and potassium permanganate
◆
ΔrG−1900.5 kJ/mol
K8.98 × 10332
pK−332.95
7SnSCrystalline solid + 4KMnO4Crystalline solid
⟶
7SnO2Crystalline solid + SO2↑Gas + 4MnSCrystalline solidgreen + 2K2SCrystalline 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
−1931−1900.5−89–
per 1 mol of
−275.9−271.50−13–
−482.8−475.13−22–
per 1 mol of
−275.9−271.50−13–
per 1 mol of
−1931−1900.5−89–
−482.8−475.13−22–
per 1 mol of
−965.5−950.25−45–

Changes in standard condition (2)

Reaction of tin(II) sulfide and potassium permanganate
7SnSCrystalline solid + 4KMnO4Crystalline solid
⟶
7SnO2Crystalline solid + SO2↑Gas + 4MnSAmorphous solidprecipitated, pink + 2K2SCrystalline 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
−1930–––
per 1 mol of
−275.7–––
−482.5–––
per 1 mol of
−275.7–––
per 1 mol of
−1930–––
−482.5–––
per 1 mol of
−965.0–––

Changes in aqueous solution (1)

Reaction of tin(II) sulfide and potassium permanganate
◆
ΔrG−2162.3 kJ/mol
K6.59 × 10378
pK−378.82
7SnSCrystalline solid + 4KMnO4Ionized aqueous solution
⟶
7SnO2Crystalline solid + SO2↑Gas + 4MnSCrystalline solidgreen + 2K2SIonized 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
−2286−2162.3−405.9–
per 1 mol of
−326.6−308.90−57.99–
−571.5−540.58−101.5–
per 1 mol of
−326.6−308.90−57.99–
per 1 mol of
−2286−2162.3−405.9–
−571.5−540.58−101.5–
per 1 mol of
−1143−1081.2−202.9–

Changes in aqueous solution (2)

Reaction of tin(II) sulfide and potassium permanganate
◆
ΔrG−2162.8 kJ/mol
K8.06 × 10378
pK−378.91
7SnSCrystalline solid + 4KMnO4Ionized aqueous solution
⟶
7SnO2Crystalline solid + SO2↑Un-ionized aqueous solution + 4MnSCrystalline solidgreen + 2K2SIonized 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
−2312−2162.8−492.2–
per 1 mol of
−330.3−308.97−70.31–
−578.0−540.70−123.0–
per 1 mol of
−330.3−308.97−70.31–
per 1 mol of
−2312−2162.8−492.2–
−578.0−540.70−123.0–
per 1 mol of
−1156−1081.4−246.1–

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
SnS (cr)-100[1]-98.3[1]77.0[1]49.25[1]
SnS (g)119.2[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]
* (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
SnO2 (cr)-580.7[1]-519.6[1]52.3[1]52.59[1]
SO2 (l)-320.5[1]–––
SO2 (g)-296.830[1]-300.194[1]248.22[1]39.87[1]
SO2 (ao)-322.980[1]-300.676[1]161.9[1]–
MnS (cr)
green
-214.2[1]-218.4[1]78.2[1]49.96[1]
MnS (am)
precipitated, pink
-213.8[1]–––
K2S (cr)-380.7[1]-364.0[1]105[1]–
K2S (ai)-471.5[1]-480.7[1]190.4[1]–
K2S (cr)
2 hydrate
-975.3[1]–––
K2S (cr)
5 hydrate
-1871.5[1]–––
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (am):Amorphous solid, (ai):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)