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4H2 + Ag2SO4 → Ag2S + 4H2O

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Reaction of hydrogen and silver(I) sulfate
4H2Hydrogen + Ag2SO4Silver(I) sulfate
⟶
Ag2SSilver(I) sulfide + 4H2OWater

The reaction of hydrogen and silver(I) sulfate yields silver(I) sulfide 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 and silver(I) sulfate
4H2Hydrogen + Ag2SO4Silver(I) sulfate
⟶
Ag2SSilver(I) sulfide + 4H2OWater

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) sulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2Hydrogen4
Reducing
Reducing
Ag2SO4Silver(I) sulfate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Ag2SSilver(I) sulfide1
Reduced
–
H2OWater4
Oxidized
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen and silver(I) sulfate
◆
ΔrG−370.78 kJ/mol
K9.07 × 1064
pK−64.96
4H2Gas + Ag2SO4Crystalline solid
⟶
Ag2SCrystalline solidα, orthorhombic + 4H2OLiquid
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
−460.03−370.78−299.5131.02
per 1 mol of
−115.01−92.695−74.8832.755
per 1 mol of
−460.03−370.78−299.5131.02
per 1 mol of
−460.03−370.78−299.5131.02
per 1 mol of
−115.01−92.695−74.8832.755

Changes in standard condition (2)

Reaction of hydrogen and silver(I) sulfate
◆
ΔrG−369.57 kJ/mol
K5.57 × 1064
pK−64.75
4H2Gas + Ag2SO4Crystalline solid
⟶
Ag2SCrystalline solidβ + 4H2OLiquid
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
−456.85−369.57−292.9–
per 1 mol of
−114.21−92.392−73.22–
per 1 mol of
−456.85−369.57−292.9–
per 1 mol of
−456.85−369.57−292.9–
per 1 mol of
−114.21−92.392−73.22–

Changes in aqueous solution

Reaction of hydrogen and silver(I) sulfate
◆
ΔrG−469.3 kJ/mol
K1.65 × 1082
pK−82.22
4H2Un-ionized aqueous solution + Ag2SO4Ionized aqueous solution
⟶
Ag2SCrystalline solidα, orthorhombic + 4H2OLiquid
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
−461.0−469.3−2050–
per 1 mol of
−115.3−117.3−512.5–
per 1 mol of
−461.0−469.3−2050–
per 1 mol of
−461.0−469.3−2050–
per 1 mol of
−115.3−117.3−512.5–

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]–
Ag2SO4 (cr)-715.88[1]-618.41[1]200.4[1]131.38[1]
Ag2SO4 (ai)-698.10[1]-590.30[1]165.7[1]-251[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
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]–
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, (l):Liquid, (g):Gas

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)