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7H2S + 6NH4ClO4 → 3(NH4)2SO4 + 4SO3 + 6HCl + 4H2

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Reaction of hydrogen sulfide and ammonium perchlorate
7H2SHydrogen sulfide + 6NH4ClO4Ammonium perchlorate
⟶
3(NH4)2SO4Ammonium sulfate + 4SO3Sulfur trioxide + 6HClHydrogen chloride + 4H2Hydrogen

The reaction of hydrogen sulfide and ammonium perchlorate yields ammonium sulfate, sulfur trioxide, hydrogen chloride, and hydrogen (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 + 6NH4ClO4Ammonium perchlorate
⟶
3(NH4)2SO4Ammonium sulfate + 4SO3Sulfur trioxide + 6HClHydrogen chloride + 4H2Hydrogen

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 perchlorate6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2SO4Ammonium sulfate3
Oxidized
–
SO3Sulfur trioxide4
Oxidized
–
HClHydrogen chloride6
Reduced
–
H2Hydrogen4
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−4004.38 kJ/mol
K3.44 × 10701
pK−701.54
7H2SGas + 6NH4ClO4Crystalline solid
⟶
3(NH4)2SO4Crystalline solid + 4SO3Liquid + 6HClGas + 4H2Gas
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
−3944.28−4004.38202.0–
per 1 mol of
−563.469−572.05428.86–
−657.380−667.39733.67–
per 1 mol of
−1314.76−1334.7967.33–
per 1 mol of
−986.070−1001.1050.50–
per 1 mol of
−657.380−667.39733.67–
per 1 mol of
−986.070−1001.1050.50–

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−4056.26 kJ/mol
K4.23 × 10710
pK−710.63
7H2SUn-ionized aqueous solution + 6NH4ClO4Ionized aqueous solution
⟶
3(NH4)2SO4Ionized aqueous solution + 4SO3Crystalline solidβ + 6HClGas + 4H2Gas
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
−4045.8−4056.2648–
per 1 mol of
−577.97−579.4666.9–
−674.30−676.0438.0–
per 1 mol of
−1348.6−1352.0916–
per 1 mol of
−1011.5−1014.0712–
per 1 mol of
−674.30−676.0438.0–
per 1 mol of
−1011.5−1014.0712–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−3985.9 kJ/mol
K1.99 × 10698
pK−698.30
7H2SUn-ionized aqueous solution + 6NH4ClO4Ionized aqueous solution
⟶
3(NH4)2SO4Ionized aqueous solution + 4SO3Crystalline solidβ + 6HClGas + 4H2Un-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
−4062.6−3985.91834–
per 1 mol of
−580.37−569.41262.0–
−677.10−664.32305.7–
per 1 mol of
−1354.2−1328.6611.3–
per 1 mol of
−1015.6−996.48458.5–
per 1 mol of
−677.10−664.32305.7–
per 1 mol of
−1015.6−996.48458.5–

Changes in aqueous solution (3)

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−4271.84 kJ/mol
K2.48 × 10748
pK−748.39
7H2SUn-ionized aqueous solution + 6NH4ClO4Ionized aqueous solution
⟶
3(NH4)2SO4Ionized aqueous solution + 4SO3Crystalline solidβ + 6HClIonized aqueous solution + 4H2Gas
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
−4495.0−4271.84−734–
per 1 mol of
−642.14−610.263−105–
−749.17−711.973−122–
per 1 mol of
−1498.3−1423.95−245–
per 1 mol of
−1123.8−1067.96−184–
per 1 mol of
−749.17−711.973−122–
per 1 mol of
−1123.8−1067.96−184–

Changes in aqueous solution (4)

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−4201.4 kJ/mol
K1.13 × 10736
pK−736.05
7H2SUn-ionized aqueous solution + 6NH4ClO4Ionized aqueous solution
⟶
3(NH4)2SO4Ionized aqueous solution + 4SO3Crystalline solidβ + 6HClIonized aqueous solution + 4H2Un-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
−4511.8−4201.41051–
per 1 mol of
−644.54−600.20150.1–
−751.97−700.23175.2–
per 1 mol of
−1503.9−1400.5350.3–
per 1 mol of
−1128.0−1050.3262.8–
per 1 mol of
−751.97−700.23175.2–
per 1 mol of
−1128.0−1050.3262.8–

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]
HCl (g)-92.307[1]-95.299[1]186.908[1]29.12[1]
HCl (ai)-167.159[1]-131.228[1]56.5[1]-136.4[1]
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]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)