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5H2S + 8CsClO3 → 4Cs2SO4 + H2SO4 + 4Cl2 + 4H2O

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Reaction of hydrogen sulfide and caesium chlorate
5H2SHydrogen sulfide + 8CsClO3Caesium chlorate
⟶
4Cs2SO4Caesium sulfate + H2SO4Sulfuric acid + 4Cl2Chlorine + 4H2OWater

The reaction of hydrogen sulfide and caesium chlorate yields caesium sulfate, sulfuric acid, 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 caesium chlorate
5H2SHydrogen sulfide + 8CsClO3Caesium chlorate
⟶
4Cs2SO4Caesium sulfate + H2SO4Sulfuric acid + 4Cl2Chlorine + 4H2OWater

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 caesium chlorate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide5
Reducing
Reducing
CsClO3Caesium chlorate8
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cs2SO4Caesium sulfate4
Oxidized
–
H2SO4Sulfuric acid1
Oxidized
–
Cl2Chlorine4
Reduced
–
H2OWater4
–
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and caesium chlorate
◆
ΔrG−4301.8 kJ/mol
K4.39 × 10753
pK−753.64
5H2SGas + 8CsClO3Crystalline solid
⟶
4Cs2SO4Crystalline solid + H2SO4Liquid + 4Cl2Gas + 4H2OLiquid
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
−4332.6−4301.8−101.3–
per 1 mol of
−866.52−860.36−20.26–
per 1 mol of
−541.58−537.73−12.66–
per 1 mol of
−1083.2−1075.5−25.32–
per 1 mol of
−4332.6−4301.8−101.3–
per 1 mol of
−1083.2−1075.5−25.32–
per 1 mol of
−1083.2−1075.5−25.32–

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and caesium chlorate
◆
ΔrG−4468.38 kJ/mol
K6.70 × 10782
pK−782.83
5H2SUn-ionized aqueous solution + 8CsClO3Ionized aqueous solution
⟶
4Cs2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 4Cl2Gas + 4H2OLiquid
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
−4659.4−4468.38−631–
per 1 mol of
−931.88−893.676−126–
per 1 mol of
−582.42−558.548−78.9–
per 1 mol of
−1164.8−1117.10−158–
per 1 mol of
−4659.4−4468.38−631–
per 1 mol of
−1164.8−1117.10−158–
per 1 mol of
−1164.8−1117.10−158–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and caesium chlorate
◆
ΔrG−4440.62 kJ/mol
K9.18 × 10777
pK−777.96
5H2SUn-ionized aqueous solution + 8CsClO3Ionized aqueous solution
⟶
4Cs2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 4Cl2Un-ionized aqueous solution + 4H2OLiquid
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
−4753.0−4440.62−1040–
per 1 mol of
−950.60−888.124−208.0–
per 1 mol of
−594.13−555.077−130.0–
per 1 mol of
−1188.3−1110.15−260.0–
per 1 mol of
−4753.0−4440.62−1040–
per 1 mol of
−1188.3−1110.15−260.0–
per 1 mol of
−1188.3−1110.15−260.0–

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]–
CsClO3 (cr)-411.7[1]-307.9[1]156.1[1]–
CsClO3 (ai)-362.25[1]-299.97[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
Cs2SO4 (cr)-1443.02[1]-1323.58[1]211.92[1]134.89[1]
Cs2SO4 (g)-1102.9[1]–––
Cs2SO4 (ai)-1425.82[1]-1328.56[1]286.2[1]–
H2SO4 (cr)––––
H2SO4 (l)-813.989[1]-690.003[1]156.904[1]138.91[1]
H2SO4 (ai)-909.27[1]-744.53[1]20.1[1]-293[1]
H2SO4 (l)
1 hydrate
-1127.621[1]-950.383[1]211.54[1]214.85[1]
H2SO4 (l)
2 hydrate
-1427.100[1]-1199.650[1]276.40[1]260.83[1]
H2SO4 (l)
3 hydrate
-1720.402[1]-1443.980[1]345.39[1]318.95[1]
H2SO4 (l)
4 hydrate
-2011.199[1]-1685.863[1]414.59[1]382.21[1]
H2SO4 (l)
6.5 hydrate
-2733.256[1]-2285.734[1]587.89[1]570.28[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, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (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)