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  3. 7H2S + 8NH4ClO4 → 4(NH4)2SO4 + 3SO3 + 4Cl2 + 7H2O

7H2S + 8NH4ClO4 → 4(NH4)2SO4 + 3SO3 + 4Cl2 + 7H2O

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Reaction of hydrogen sulfide and ammonium perchlorate
7H2SHydrogen sulfide + 8NH4ClO4Ammonium perchlorate
⟶
4(NH4)2SO4Ammonium sulfate + 3SO3Sulfur trioxide + 4Cl2Chlorine + 7H2OWater

The reaction of hydrogen sulfide and ammonium perchlorate yields ammonium sulfate, sulfur trioxide, chlorine, 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 ammonium perchlorate
7H2SHydrogen sulfide + 8NH4ClO4Ammonium perchlorate
⟶
4(NH4)2SO4Ammonium sulfate + 3SO3Sulfur trioxide + 4Cl2Chlorine + 7H2OWater

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 ammonium perchlorate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide7
Reducing
Reducing
NH4ClO4Ammonium perchlorate8
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2SO4Ammonium sulfate4
Oxidized
–
SO3Sulfur trioxide3
Oxidized
–
Cl2Chlorine4
Reduced
–
H2OWater7
–
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−5442.91 kJ/mol
K3.60 × 10953
pK−953.56
7H2SGas + 8NH4ClO4Crystalline solid
⟶
4(NH4)2SO4Crystalline solid + 3SO3Liquid + 4Cl2Gas + 7H2OLiquid
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
−5540.44−5442.91−326.7–
per 1 mol of
−791.491−777.559−46.67–
−692.555−680.364−40.84–
per 1 mol of
−1385.11−1360.73−81.67–
per 1 mol of
−1846.81−1814.30−108.9–
per 1 mol of
−1385.11−1360.73−81.67–
per 1 mol of
−791.491−777.559−46.67–

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−5497.64 kJ/mol
K1.40 × 10963
pK−963.14
7H2SUn-ionized aqueous solution + 8NH4ClO4Ionized aqueous solution
⟶
4(NH4)2SO4Ionized aqueous solution + 3SO3Crystalline solidβ + 4Cl2Gas + 7H2OLiquid
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
−5688.9−5497.64−629–
per 1 mol of
−812.70−785.377−89.9–
−711.11−687.205−78.6–
per 1 mol of
−1422.2−1374.41−157–
per 1 mol of
−1896.3−1832.55−210–
per 1 mol of
−1422.2−1374.41−157–
per 1 mol of
−812.70−785.377−89.9–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−5469.88 kJ/mol
K1.91 × 10958
pK−958.28
7H2SUn-ionized aqueous solution + 8NH4ClO4Ionized aqueous solution
⟶
4(NH4)2SO4Ionized aqueous solution + 3SO3Crystalline solidβ + 4Cl2Un-ionized aqueous solution + 7H2OLiquid
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
−5782.5−5469.88−1037–
per 1 mol of
−826.07−781.411−148.1–
−722.81−683.735−129.6–
per 1 mol of
−1445.6−1367.47−259.3–
per 1 mol of
−1927.5−1823.29−345.7–
per 1 mol of
−1445.6−1367.47−259.3–
per 1 mol of
−826.07−781.411−148.1–

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]–
NH4ClO4 (cr)-295.31[1]-88.75[1]186.2[1]–
NH4ClO4 (ai)-261.83[1]-87.83[1]295.4[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
(NH4)2SO4 (cr)-1180.85[1]-901.67[1]220.1[1]187.49[1]
(NH4)2SO4 (ai)-1174.28[1]-903.14[1]246.9[1]-133.1[1]
SO3 (cr)
β
-454.51[1]-374.21[1]70.7[1]–
SO3 (l)-441.04[1]-373.75[1]113.8[1]–
SO3 (g)-395.72[1]-371.06[1]256.76[1]50.67[1]
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[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, (ai):Ionized aqueous solution, (l):Liquid, (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)