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14H2S + 6AgNO3 → 2H2SO3 + 6SO2 + 3(NH4)2S + 3Ag2S

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Reaction of hydrogen sulfide and silver(I) nitrate
14H2SHydrogen sulfide + 6AgNO3Silver(I) nitrate
⟶
2H2SO3Sulfurous acid + 6SO2Sulfur dioxide + 3(NH4)2SAmmonium sulfide + 3Ag2SSilver(I) sulfide

The reaction of hydrogen sulfide and silver(I) nitrate yields sulfurous acid, sulfur dioxide, ammonium sulfide, and silver(I) sulfide (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 silver(I) nitrate
14H2SHydrogen sulfide + 6AgNO3Silver(I) nitrate
⟶
2H2SO3Sulfurous acid + 6SO2Sulfur dioxide + 3(NH4)2SAmmonium sulfide + 3Ag2SSilver(I) sulfide

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of hydrogen sulfide and silver(I) nitrate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide14
Reducing
Reducing
AgNO3Silver(I) nitrate6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
H2SO3Sulfurous acid2
Oxidized
–
SO2Sulfur dioxide6
Oxidized
–
(NH4)2SAmmonium sulfide3
Reduced
–
Ag2SSilver(I) sulfide3
–
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and silver(I) nitrate
◆
ΔrG−2622.0 kJ/mol
K2.26 × 10459
pK−459.35
14H2SUn-ionized aqueous solution + 6AgNO3Ionized aqueous solution
⟶
2H2SO3Un-ionized aqueous solution + 6SO2Gas + 3(NH4)2SIonized aqueous solution + 3Ag2SCrystalline solidα, orthorhombic
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
−2625.2−2622.013–
per 1 mol of
−187.51−187.290.93–
per 1 mol of
−437.53−437.002.2–
per 1 mol of
−1312.6−1311.06.5–
per 1 mol of
−437.53−437.002.2–
per 1 mol of
−875.07−874.004.3–
per 1 mol of
−875.07−874.004.3–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and silver(I) nitrate
◆
ΔrG−2624.9 kJ/mol
K7.29 × 10459
pK−459.86
14H2SUn-ionized aqueous solution + 6AgNO3Ionized aqueous solution
⟶
2H2SO3Un-ionized aqueous solution + 6SO2Un-ionized aqueous solution + 3(NH4)2SIonized aqueous solution + 3Ag2SCrystalline solidα, orthorhombic
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
−2782.1−2624.9−505–
per 1 mol of
−198.72−187.49−36.1–
per 1 mol of
−463.68−437.48−84.2–
per 1 mol of
−1391.0−1312.5−253–
per 1 mol of
−463.68−437.48−84.2–
per 1 mol of
−927.37−874.97−168–
per 1 mol of
−927.37−874.97−168–

Changes in aqueous solution (3)

Reaction of hydrogen sulfide and silver(I) nitrate
◆
ΔrG−2632.0 kJ/mol
K1.28 × 10461
pK−461.11
14H2SUn-ionized aqueous solution + 6AgNO3Un-ionized aqueous solution
⟶
2H2SO3Un-ionized aqueous solution + 6SO2Gas + 3(NH4)2SIonized aqueous solution + 3Ag2SCrystalline solidα, orthorhombic
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
–−2632.0––
per 1 mol of
–−188.00––
per 1 mol of
–−438.67––
per 1 mol of
–−1316.0––
per 1 mol of
–−438.67––
per 1 mol of
–−877.33––
per 1 mol of
–−877.33––

Changes in aqueous solution (4)

Reaction of hydrogen sulfide and silver(I) nitrate
◆
ΔrG−2634.9 kJ/mol
K4.12 × 10461
pK−461.61
14H2SUn-ionized aqueous solution + 6AgNO3Un-ionized aqueous solution
⟶
2H2SO3Un-ionized aqueous solution + 6SO2Un-ionized aqueous solution + 3(NH4)2SIonized aqueous solution + 3Ag2SCrystalline solidα, orthorhombic
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
–−2634.9––
per 1 mol of
–−188.21––
per 1 mol of
–−439.15––
per 1 mol of
–−1317.5––
per 1 mol of
–−439.15––
per 1 mol of
–−878.30––
per 1 mol of
–−878.30––

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]–
AgNO3 (cr)-124.39[1]-33.41[1]140.92[1]93.05[1]
AgNO3 (ai)-101.80[1]-34.16[1]219.2[1]-64.9[1]
AgNO3 (ao)–-32.49[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
H2SO3 (ao)-608.81[1]-537.81[1]232.2[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]–
(NH4)2S (ai)-231.8[1]-72.6[1]212.1[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]–
* (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas, (ai):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)