You-iggy
  1. Home
  2. Chemical reactions
  3. 2H2S + NH4ClO4 → 2SO2 + NH4Cl + 2H2

2H2S + NH4ClO4 → 2SO2 + NH4Cl + 2H2

Last updated:
Reaction of hydrogen sulfide and ammonium perchlorate
2H2SHydrogen sulfide + NH4ClO4Ammonium perchlorate
⟶
2SO2Sulfur dioxide + NH4ClAmmonium chloride + 2H2Hydrogen

The reaction of hydrogen sulfide and ammonium perchlorate yields sulfur dioxide, ammonium 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
2H2SHydrogen sulfide + NH4ClO4Ammonium perchlorate
⟶
2SO2Sulfur dioxide + NH4ClAmmonium chloride + 2H2Hydrogen

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 sulfide2
Reducing
Reducing
NH4ClO4Ammonium perchlorate1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide2
Oxidized
–
NH4ClAmmonium chloride1
Reduced
–
H2Hydrogen2
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−647.39 kJ/mol
K2.62 × 10113
pK−113.42
2H2SGas + NH4ClO4Crystalline solid
⟶
2SO2Gas + NH4ClCrystalline solid + 2H2Gas
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
−571.52−647.39254.6–
per 1 mol of
−285.76−323.69127.3–
−571.52−647.39254.6–
per 1 mol of
−285.76−323.69127.3–
per 1 mol of
−571.52−647.39254.6–
per 1 mol of
−285.76−323.69127.3–

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−667.42 kJ/mol
K8.45 × 10116
pK−116.93
2H2SUn-ionized aqueous solution + NH4ClO4Ionized aqueous solution
⟶
2SO2Gas + NH4ClIonized aqueous solution + 2H2Gas
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
−552.1−667.42390–
per 1 mol of
−276.1−333.71195–
−552.1−667.42390–
per 1 mol of
−276.1−333.71195–
per 1 mol of
−552.1−667.42390–
per 1 mol of
−276.1−333.71195–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−632.2 kJ/mol
K5.71 × 10110
pK−110.76
2H2SUn-ionized aqueous solution + NH4ClO4Ionized aqueous solution
⟶
2SO2Gas + NH4ClIonized aqueous solution + 2H2Un-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
−560.5−632.21283–
per 1 mol of
−280.3−316.1641.5–
−560.5−632.21283–
per 1 mol of
−280.3−316.1641.5–
per 1 mol of
−560.5−632.21283–
per 1 mol of
−280.3−316.1641.5–

Changes in aqueous solution (3)

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−668.38 kJ/mol
K1.24 × 10117
pK−117.10
2H2SUn-ionized aqueous solution + NH4ClO4Ionized aqueous solution
⟶
2SO2Un-ionized aqueous solution + NH4ClIonized aqueous solution + 2H2Gas
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
−604.4−668.38218–
per 1 mol of
−302.2−334.19109–
−604.4−668.38218–
per 1 mol of
−302.2−334.19109–
per 1 mol of
−604.4−668.38218–
per 1 mol of
−302.2−334.19109–

Changes in aqueous solution (4)

Reaction of hydrogen sulfide and ammonium perchlorate
◆
ΔrG−633.2 kJ/mol
K8.55 × 10110
pK−110.93
2H2SUn-ionized aqueous solution + NH4ClO4Ionized aqueous solution
⟶
2SO2Un-ionized aqueous solution + NH4ClIonized aqueous solution + 2H2Un-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
−612.8−633.21110–
per 1 mol of
−306.4−316.6555.0–
−612.8−633.21110–
per 1 mol of
−306.4−316.6555.0–
per 1 mol of
−612.8−633.21110–
per 1 mol of
−306.4−316.6555.0–

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
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]–
NH4Cl (cr)-314.43[1]-202.87[1]94.6[1]84.1[1]
NH4Cl (ai)-299.66[1]-210.52[1]169.9[1]-56.5[1]
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):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)