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H2 + S → H2S

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Reaction of hydrogen and sulfur
H2Hydrogen + SSulfur
⟶
H2SHydrogen sulfide

The reaction of hydrogen and sulfur yields hydrogen sulfide. 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 categories

Reaction data

Chemical equation

Reaction of hydrogen and sulfur
H2Hydrogen + SSulfur
⟶
H2SHydrogen sulfide

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product
Reaction of nonmetal and nonmetal
NonmetalReducing agent + NonmetalOxidizing agent
⟶
Binary compoundOxidation reduction product

Oxidation state of each atom

Reaction of hydrogen and sulfur

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2Hydrogen1
Reducing
Reducing
Nonmetal
SSulfur1
Oxidizing
Reducible
Nonmetal

Products

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide1
Redoxed product
–
Binary compound

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen and sulfur
◆
ΔrG−33.56 kJ/mol
K7.58 × 105
pK−5.88
H2Gas + SCrystalline solidrhombic
⟶
H2SGas
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
−20.63−33.5643.31−17.23
per 1 mol of
−20.63−33.5643.31−17.23
per 1 mol of
−20.63−33.5643.31−17.23
per 1 mol of
−20.63−33.5643.31−17.23

Changes in standard condition (2)

Reaction of hydrogen and sulfur
H2Gas + SCrystalline solidmonoclinic
⟶
H2SGas
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
−20.96–––
per 1 mol of
−20.96–––
per 1 mol of
−20.96–––
per 1 mol of
−20.96–––

Changes in aqueous solution (1)

Reaction of hydrogen and sulfur
◆
ΔrG−51.2 kJ/mol
K9.33 × 108
pK−8.97
H2Un-ionized aqueous solution + SCrystalline solidrhombic
⟶
H2SGas
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
−16.4−51.2−403–
per 1 mol of
−16.4−51.2−403–
per 1 mol of
−16.4−51.2−403–
per 1 mol of
−16.4−51.2−403–

Changes in aqueous solution (2)

Reaction of hydrogen and sulfur
◆
ΔrG−45.4 kJ/mol
K8.99 × 107
pK−7.95
H2Un-ionized aqueous solution + SCrystalline solidrhombic
⟶
H2SUn-ionized 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
−35.5−45.4−488–
per 1 mol of
−35.5−45.4−488–
per 1 mol of
−35.5−45.4−488–
per 1 mol of
−35.5−45.4−488–

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
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[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]
* (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
H2S (g)-20.63[1]-33.56[1]205.79[1]34.23[1]
H2S (ao)-39.7[1]-27.83[1]121[1]–
* (g):Gas, (ao):Un-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)