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H2S + 3CO2 🔥→ SO2 + 3CO + H2O

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Reaction of hydrogen sulfide and carbon dioxide
H2SHydrogen sulfide + 3CO2Carbon dioxide
🔥
⟶
SO2Sulfur dioxide + 3COCarbon monoxide + H2OWater

The reaction of hydrogen sulfide and carbon dioxide yields sulfur dioxide, 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 carbon dioxide
H2SHydrogen sulfide + 3CO2Carbon dioxide
🔥
⟶
SO2Sulfur dioxide + 3COCarbon monoxide + H2OWater

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 carbon dioxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide1
Reducing
Reducing
CO2Carbon dioxide3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide1
Oxidized
–
COCarbon monoxide3
Reduced
–
H2OWater1
–
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and carbon dioxide
◆
ΔrG267.81 kJ/mol
K0.12 × 10−46
pK46.92
H2SGas + 3CO2Gas
🔥
⟶
SO2Gas + 3COGas + H2OLiquid
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
286.92267.8164.1457.03
per 1 mol of
286.92267.8164.1457.03
per 1 mol of
95.64089.27021.3819.01
per 1 mol of
286.92267.8164.1457.03
per 1 mol of
95.64089.27021.3819.01
per 1 mol of
286.92267.8164.1457.03

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and carbon dioxide
◆
ΔrG236.94 kJ/mol
K0.31 × 10−41
pK41.51
H2SUn-ionized aqueous solution + 3CO2Un-ionized aqueous solution
🔥
⟶
SO2Gas + 3COGas + H2OLiquid
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
366.9236.94437–
per 1 mol of
366.9236.94437–
per 1 mol of
122.378.980146–
per 1 mol of
366.9236.94437–
per 1 mol of
122.378.980146–
per 1 mol of
366.9236.94437–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and carbon dioxide
◆
ΔrG288.75 kJ/mol
K0.26 × 10−50
pK50.59
H2SUn-ionized aqueous solution + 3CO2Un-ionized aqueous solution
🔥
⟶
SO2Gas + 3COUn-ionized aqueous solution + H2OLiquid
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
335.6288.75158–
per 1 mol of
335.6288.75158–
per 1 mol of
111.996.25052.7–
per 1 mol of
335.6288.75158–
per 1 mol of
111.996.25052.7–
per 1 mol of
335.6288.75158–

Changes in aqueous solution (3)

Reaction of hydrogen sulfide and carbon dioxide
◆
ΔrG236.46 kJ/mol
K0.37 × 10−41
pK41.43
H2SUn-ionized aqueous solution + 3CO2Un-ionized aqueous solution
🔥
⟶
SO2Un-ionized aqueous solution + 3COGas + H2OLiquid
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
340.7236.46351–
per 1 mol of
340.7236.46351–
per 1 mol of
113.678.820117–
per 1 mol of
340.7236.46351–
per 1 mol of
113.678.820117–
per 1 mol of
340.7236.46351–

Changes in aqueous solution (4)

Reaction of hydrogen sulfide and carbon dioxide
◆
ΔrG288.27 kJ/mol
K0.31 × 10−50
pK50.50
H2SUn-ionized aqueous solution + 3CO2Un-ionized aqueous solution
🔥
⟶
SO2Un-ionized aqueous solution + 3COUn-ionized aqueous solution + H2OLiquid
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
309.4288.2772–
per 1 mol of
309.4288.2772–
per 1 mol of
103.196.09024–
per 1 mol of
309.4288.2772–
per 1 mol of
103.196.09024–
per 1 mol of
309.4288.2772–

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]–
CO2 (g)-393.509[1]-394.359[1]213.74[1]37.11[1]
CO2 (ao)-413.80[1]-385.98[1]117.6[1]–
* (g):Gas, (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
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]–
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]
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid

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)