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H2 + Ag2S 🔥→ 2Ag + H2S

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Reaction of hydrogen and silver(I) sulfide
H2Hydrogen + Ag2SSilver(I) sulfide
🔥
⟶
2AgSilver + H2SHydrogen sulfide

The reaction of hydrogen and silver(I) sulfide yields silver and 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 silver(I) sulfide
H2Hydrogen + Ag2SSilver(I) sulfide
🔥
⟶
2AgSilver + H2SHydrogen sulfide

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 and silver(I) sulfide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2Hydrogen1
Reducing
Reducing
Ag2SSilver(I) sulfide1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
AgSilver2
Reduced
–
H2SHydrogen sulfide1
Oxidized
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen and silver(I) sulfide
◆
ΔrG7.11 kJ/mol
K0.57 × 10−1
pK1.25
H2Gas + Ag2SCrystalline solidα, orthorhombic
🔥
⟶
2AgCrystalline solid + 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
11.967.1116.20−20.42
per 1 mol of
11.967.1116.20−20.42
per 1 mol of
11.967.1116.20−20.42
per 1 mol of
5.9803.568.100−10.21
per 1 mol of
11.967.1116.20−20.42

Changes in standard condition (2)

Reaction of hydrogen and silver(I) sulfide
◆
ΔrG5.90 kJ/mol
K0.93 × 10−1
pK1.03
H2Gas + Ag2SCrystalline solidβ
🔥
⟶
2AgCrystalline solid + 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
8.785.909.6–
per 1 mol of
8.785.909.6–
per 1 mol of
8.785.909.6–
per 1 mol of
4.392.954.8–
per 1 mol of
8.785.909.6–

Changes in aqueous solution (1)

Reaction of hydrogen and silver(I) sulfide
◆
ΔrG−10.5 kJ/mol
K6.91 × 101
pK−1.84
H2Un-ionized aqueous solution + Ag2SCrystalline solidα, orthorhombic
🔥
⟶
2AgCrystalline solid + 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
16.2−10.5−430–
per 1 mol of
16.2−10.5−430–
per 1 mol of
16.2−10.5−430–
per 1 mol of
8.10−5.25−215–
per 1 mol of
16.2−10.5−430–

Changes in aqueous solution (2)

Reaction of hydrogen and silver(I) sulfide
◆
ΔrG−4.8 kJ/mol
K6.93 × 100
pK−0.84
H2Un-ionized aqueous solution + Ag2SCrystalline solidα, orthorhombic
🔥
⟶
2AgCrystalline solid + 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
−2.9−4.8−515–
per 1 mol of
−2.9−4.8−515–
per 1 mol of
−2.9−4.8−515–
per 1 mol of
−1.4−2.4−258–
per 1 mol of
−2.9−4.8−515–

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]–
Ag2S (cr)
α, orthorhombic
-32.59[1]-40.67[1]144.01[1]76.53[1]
Ag2S (cr)
β
-29.41[1]-39.46[1]150.6[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
Ag (cr)0[1]0[1]42.55[1]25.351[1]
Ag (g)284.55[1]245.65[1]172.997[1]20.786[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]–
* (cr):Crystalline solid, (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)