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H2S + CsClO3 → SO2 + CsCl + H2O

The reaction of hydrogen sulfide and caesium chlorate yields sulfur dioxide, caesium chloride, 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

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide1
Reducing
Reducing
CsClO3Caesium chlorate1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide1
Oxidized
CsClCaesium chloride1
Reduced
H2OWater1

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and caesium chlorate
ΔrG−610.4 kJ/mol
K8.66 × 10106
pK−106.94
H2SGas + CsClO3Crystalline solid
SO2Gas + CsClCrystalline solid + H2OLiquid
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
−593.4−610.457.4
per 1 mol of
−593.4−610.457.4
per 1 mol of
−593.4−610.457.4
per 1 mol of
−593.4−610.457.4
per 1 mol of
−593.4−610.457.4
per 1 mol of
−593.4−610.457.4

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and caesium chlorate
ΔrG−632.76 kJ/mol
K7.16 × 10110
pK−110.85
H2SUn-ionized aqueous solution + CsClO3Ionized aqueous solution
SO2Gas + CsClIonized aqueous solution + H2OLiquid
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
−606.1−632.7691
per 1 mol of
−606.1−632.7691
per 1 mol of
−606.1−632.7691
per 1 mol of
−606.1−632.7691
per 1 mol of
−606.1−632.7691
per 1 mol of
−606.1−632.7691

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and caesium chlorate
ΔrG−633.25 kJ/mol
K8.72 × 10110
pK−110.94
H2SUn-ionized aqueous solution + CsClO3Ionized aqueous solution
SO2Un-ionized aqueous solution + CsClIonized aqueous solution + H2OLiquid
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
−632.3−633.255
per 1 mol of
−632.3−633.255
per 1 mol of
−632.3−633.255
per 1 mol of
−632.3−633.255
per 1 mol of
−632.3−633.255
per 1 mol of
−632.3−633.255

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
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]
CsCl (cr)-443.04[1]-414.53[1]101.17[1]52.47[1]
CsCl (g)-240.20[1]-257.80[1]255.96[1]36.94[1]
CsCl (ai)-425.43[1]-423.24[1]189.54[1]-146.9[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]
* (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)