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3H2S + K2CO3 🔥→ S + 2KHS + CO + 2H2O

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Reaction of hydrogen sulfide and potassium carbonate
3H2SHydrogen sulfide + K2CO3Potassium carbonate
🔥
⟶
SSulfur + 2KHSPotassium hydrogensulfide + COCarbon monoxide + 2H2OWater

The reaction of hydrogen sulfide and potassium carbonate yields sulfur, potassium hydrogensulfide, carbon monoxide, 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 hydrogen sulfide and potassium carbonate
3H2SHydrogen sulfide + K2CO3Potassium carbonate
🔥
⟶
SSulfur + 2KHSPotassium hydrogensulfide + COCarbon monoxide + 2H2OWater

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of hydrogen sulfide and potassium carbonate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide3
Reducing
Reducing
K2CO3Potassium carbonate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
SSulfur1
Oxidized
–
KHSPotassium hydrogensulfide2
–
–
COCarbon monoxide1
Reduced
–
H2OWater2
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and potassium carbonate
3H2SGas + K2CO3Crystalline solid
🔥
⟶
SCrystalline solidrhombic + 2KHSCrystalline solid + COGas + 2H2OLiquid
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
0.53––135.86
per 1 mol of
0.177––45.287
0.530––135.86
per 1 mol of
0.530––135.86
0.265––67.930
per 1 mol of
0.530––135.86
per 1 mol of
0.265––67.930

Changes in standard condition (2)

Reaction of hydrogen sulfide and potassium carbonate
3H2SGas + K2CO3Crystalline solid
🔥
⟶
SCrystalline solidmonoclinic + 2KHSCrystalline solid + COGas + 2H2OLiquid
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
0.86–––
per 1 mol of
0.287–––
0.860–––
per 1 mol of
0.860–––
0.430–––
per 1 mol of
0.860–––
per 1 mol of
0.430–––

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and potassium carbonate
◆
ΔrG24.04 kJ/mol
K0.61 × 10−4
pK4.21
3H2SUn-ionized aqueous solution + K2CO3Ionized aqueous solution
🔥
⟶
SCrystalline solidrhombic + 2KHSIonized aqueous solution + COGas + 2H2OLiquid
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
79.024.04189–
per 1 mol of
26.38.01363.0–
79.024.04189–
per 1 mol of
79.024.04189–
39.512.0294.5–
per 1 mol of
79.024.04189–
per 1 mol of
39.512.0294.5–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and potassium carbonate
◆
ΔrG41.31 kJ/mol
K0.58 × 10−7
pK7.24
3H2SUn-ionized aqueous solution + K2CO3Ionized aqueous solution
🔥
⟶
SCrystalline solidrhombic + 2KHSIonized aqueous solution + COUn-ionized aqueous solution + 2H2OLiquid
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
68.641.3196–
per 1 mol of
22.913.7732–
68.641.3196–
per 1 mol of
68.641.3196–
34.320.6648–
per 1 mol of
68.641.3196–
per 1 mol of
34.320.6648–

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
H2S (g)-20.63[1]-33.56[1]205.79[1]34.23[1]
H2S (ao)-39.7[1]-27.83[1]121[1]–
K2CO3 (cr)-1151.02[1]-1063.5[1]155.52[1]114.43[1]
K2CO3 (ai)-1181.90[1]-1094.36[1]148.1[1]–
K2CO3 (cr)
1.5 hydrate
-1609.2[1]-1432.5[1]203.3[1]–
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]–––
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
KHS (cr)-265.10[1]––75.31[1]
KHS (ai)-269.9[1]-271.19[1]165.3[1]–
KHS (cr)
0.25 hydrate
-337.2[1]–––
CO (g)-110.525[1]-137.168[1]197.674[1]29.142[1]
CO (ao)-120.96[1]-119.90[1]104.6[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, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (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)