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8H2S + 2RbClO4 → 7S + Cl2 + Rb2S + 8H2O

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Reaction of hydrogen sulfide and rubidium perchlorate
8H2SHydrogen sulfide + 2RbClO4Rubidium perchlorate
⟶
7SSulfur + Cl2Chlorine + Rb2SRubidium sulfide + 8H2OWater

The reaction of hydrogen sulfide and rubidium perchlorate yields sulfur, chlorine, rubidium 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 sulfide and rubidium perchlorate
8H2SHydrogen sulfide + 2RbClO4Rubidium perchlorate
⟶
7SSulfur + Cl2Chlorine + Rb2SRubidium sulfide + 8H2OWater

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 rubidium perchlorate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide8
Reducing
Reducing
RbClO4Rubidium perchlorate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SSulfur7
Oxidized
–
Cl2Chlorine1
Reduced
–
Rb2SRubidium sulfide1
–
–
H2OWater8
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and rubidium perchlorate
8H2SGas + 2RbClO4Crystalline solid
⟶
7SCrystalline solidrhombic + Cl2Gas + Rb2SCrystalline solid + 8H2OLiquid
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
−1607.8–––
per 1 mol of
−200.97–––
−803.90–––
per 1 mol of
−229.69–––
per 1 mol of
−1607.8–––
per 1 mol of
−1607.8–––
per 1 mol of
−200.97–––

Changes in standard condition (2)

Reaction of hydrogen sulfide and rubidium perchlorate
8H2SGas + 2RbClO4Crystalline solid
⟶
7SCrystalline solidmonoclinic + Cl2Gas + Rb2SCrystalline solid + 8H2OLiquid
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
−1605.5–––
per 1 mol of
−200.69–––
−802.75–––
per 1 mol of
−229.36–––
per 1 mol of
−1605.5–––
per 1 mol of
−1605.5–––
per 1 mol of
−200.69–––

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and rubidium perchlorate
◆
ΔrG−1571.4 kJ/mol
K1.98 × 10275
pK−275.30
8H2SUn-ionized aqueous solution + 2RbClO4Ionized aqueous solution
⟶
7SCrystalline solidrhombic + Cl2Gas + Rb2SIonized aqueous solution + 8H2OLiquid
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
−1677.5−1571.4−341–
per 1 mol of
−209.69−196.43−42.6–
−838.75−785.70−171–
per 1 mol of
−239.64−224.49−48.7–
per 1 mol of
−1677.5−1571.4−341–
per 1 mol of
−1677.5−1571.4−341–
per 1 mol of
−209.69−196.43−42.6–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and rubidium perchlorate
◆
ΔrG−1564.4 kJ/mol
K1.18 × 10274
pK−274.07
8H2SUn-ionized aqueous solution + 2RbClO4Ionized aqueous solution
⟶
7SCrystalline solidrhombic + Cl2Un-ionized aqueous solution + Rb2SIonized aqueous solution + 8H2OLiquid
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
−1700.9−1564.4−443–
per 1 mol of
−212.61−195.55−55.4–
−850.45−782.20−222–
per 1 mol of
−242.99−223.49−63.3–
per 1 mol of
−1700.9−1564.4−443–
per 1 mol of
−1700.9−1564.4−443–
per 1 mol of
−212.61−195.55−55.4–

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]–
RbClO4 (cr)-437.23[1]-306.90[1]161.1[1]–
RbClO4 (ai)-380.49[1]-292.51[1]303.3[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
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]–––
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]–
Rb2S (cr)-360.7[1]–––
Rb2S (ai)-469.4[1]-482.0[1]228.4[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, (g):Gas, (ao):Un-ionized aqueous solution, (ai):Ionized aqueous solution, (l):Liquid

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)