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  3. 2H2S + 3ZnCO3 🔥→ 2SO2 + 3Zn + 3CO + 2H2O

2H2S + 3ZnCO3 🔥→ 2SO2 + 3Zn + 3CO + 2H2O

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Reaction of hydrogen sulfide and zinc carbonate
2H2SHydrogen sulfide + 3ZnCO3Zinc carbonate
🔥
⟶
2SO2Sulfur dioxide + 3ZnZinc + 3COCarbon monoxide + 2H2OWater

The reaction of hydrogen sulfide and zinc carbonate yields sulfur dioxide, zinc, 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 zinc carbonate
2H2SHydrogen sulfide + 3ZnCO3Zinc carbonate
🔥
⟶
2SO2Sulfur dioxide + 3ZnZinc + 3COCarbon 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 zinc carbonate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide2
Reducing
Reducing
ZnCO3Zinc carbonate3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide2
Oxidized
–
ZnZinc3
Reduced
–
COCarbon monoxide3
Reduced
–
H2OWater2
–
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and zinc carbonate
◆
ΔrG775.53 kJ/mol
K0.14 × 10−135
pK135.87
2H2SGas + 3ZnCO3Crystalline solid
🔥
⟶
2SO2Gas + 3ZnCrystalline solid + 3COGas + 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
982.71775.53695.486.36
per 1 mol of
491.36387.76347.743.18
per 1 mol of
327.57258.51231.828.79
per 1 mol of
491.36387.76347.743.18
per 1 mol of
327.57258.51231.828.79
per 1 mol of
327.57258.51231.828.79
per 1 mol of
491.36387.76347.743.18

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and zinc carbonate
◆
ΔrG764.07 kJ/mol
K0.14 × 10−133
pK133.86
2H2SUn-ionized aqueous solution + 3ZnCO3Crystalline solid
🔥
⟶
2SO2Gas + 3ZnCrystalline solid + 3COGas + 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
1020.8764.07865–
per 1 mol of
510.40382.04433–
per 1 mol of
340.27254.69288–
per 1 mol of
510.40382.04433–
per 1 mol of
340.27254.69288–
per 1 mol of
340.27254.69288–
per 1 mol of
510.40382.04433–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and zinc carbonate
◆
ΔrG815.87 kJ/mol
K0.12 × 10−142
pK142.93
2H2SUn-ionized aqueous solution + 3ZnCO3Crystalline solid
🔥
⟶
2SO2Gas + 3ZnCrystalline solid + 3COUn-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
989.5815.87586–
per 1 mol of
494.8407.94293–
per 1 mol of
329.8271.96195–
per 1 mol of
494.8407.94293–
per 1 mol of
329.8271.96195–
per 1 mol of
329.8271.96195–
per 1 mol of
494.8407.94293–

Changes in aqueous solution (3)

Reaction of hydrogen sulfide and zinc carbonate
◆
ΔrG763.11 kJ/mol
K0.20 × 10−133
pK133.69
2H2SUn-ionized aqueous solution + 3ZnCO3Crystalline solid
🔥
⟶
2SO2Un-ionized aqueous solution + 3ZnCrystalline solid + 3COGas + 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
968.5763.11692–
per 1 mol of
484.3381.56346–
per 1 mol of
322.8254.37231–
per 1 mol of
484.3381.56346–
per 1 mol of
322.8254.37231–
per 1 mol of
322.8254.37231–
per 1 mol of
484.3381.56346–

Changes in aqueous solution (4)

Reaction of hydrogen sulfide and zinc carbonate
◆
ΔrG814.91 kJ/mol
K0.17 × 10−142
pK142.77
2H2SUn-ionized aqueous solution + 3ZnCO3Crystalline solid
🔥
⟶
2SO2Un-ionized aqueous solution + 3ZnCrystalline solid + 3COUn-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
937.2814.91413–
per 1 mol of
468.6407.45207–
per 1 mol of
312.4271.64138–
per 1 mol of
468.6407.45207–
per 1 mol of
312.4271.64138–
per 1 mol of
312.4271.64138–
per 1 mol of
468.6407.45207–

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]–
ZnCO3 (cr)-812.78[1]-731.52[1]82.4[1]79.71[1]
ZnCO3 (cr)
1 hydrate
–-970.6[1]––
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid

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]–
Zn (cr)0[1]0[1]41.63[1]25.40[1]
Zn (g)130.729[1]95.145[1]160.984[1]20.786[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)