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11H2S + 6NaBrO3 → 5SO2 + 3Br2 + 6NaHS + 8H2O

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Reaction of hydrogen sulfide and sodium bromate
11H2SHydrogen sulfide + 6NaBrO3Sodium bromate
⟶
5SO2Sulfur dioxide + 3Br2Bromine + 6NaHSSodium hydrogensulfide + 8H2OWater

The reaction of hydrogen sulfide and sodium bromate yields sulfur dioxide, bromine, sodium hydrogensulfide, 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 sodium bromate
11H2SHydrogen sulfide + 6NaBrO3Sodium bromate
⟶
5SO2Sulfur dioxide + 3Br2Bromine + 6NaHSSodium hydrogensulfide + 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 sodium bromate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide11
Reducing
Reducing
NaBrO3Sodium bromate6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide5
Oxidized
–
Br2Bromine3
Reduced
–
NaHSSodium hydrogensulfide6
–
–
H2OWater8
–
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and sodium bromate
11H2SGas + 6NaBrO3Crystalline solid
⟶
5SO2Gas + 3Br2Liquid + 6NaHSCrystalline 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
−2962.70–––
per 1 mol of
−269.336–––
per 1 mol of
−493.783–––
per 1 mol of
−592.540–––
per 1 mol of
−987.567–––
−493.783–––
per 1 mol of
−370.337–––

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and sodium bromate
◆
ΔrG−3119.20 kJ/mol
K2.89 × 10546
pK−546.46
11H2SUn-ionized aqueous solution + 6NaBrO3Ionized aqueous solution
⟶
5SO2Gas + 3Br2Un-ionized aqueous solution + 6NaHSIonized 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
−3045.1−3119.20266–
per 1 mol of
−276.83−283.56424.2–
per 1 mol of
−507.52−519.86744.3–
per 1 mol of
−609.02−623.84053.2–
per 1 mol of
−1015.0−1039.7388.7–
−507.52−519.86744.3–
per 1 mol of
−380.64−389.90033.3–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and sodium bromate
◆
ΔrG−3121.61 kJ/mol
K7.63 × 10546
pK−546.88
11H2SUn-ionized aqueous solution + 6NaBrO3Ionized aqueous solution
⟶
5SO2Un-ionized aqueous solution + 3Br2Un-ionized aqueous solution + 6NaHSIonized 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
−3175.9−3121.61−165–
per 1 mol of
−288.72−283.783−15.0–
per 1 mol of
−529.32−520.268−27.5–
per 1 mol of
−635.18−624.322−33.0–
per 1 mol of
−1058.6−1040.54−55.0–
−529.32−520.268−27.5–
per 1 mol of
−396.99−390.201−20.6–

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]–
NaBrO3 (cr)-334.09[1]-242.62[1]128.9[1]–
NaBrO3 (ai)-307.19[1]-243.29[1]220.9[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]–
Br2 (cr)––––
Br2 (l)0[1]0[1]152.231[1]75.689[1]
Br2 (g)30.907[1]3.110[1]245.463[1]36.02[1]
Br2 (ao)-2.59[1]3.93[1]130.5[1]–
NaHS (cr)-237.23[1]–––
NaHS (ai)-257.73[1]-249.81[1]121.8[1]–
NaHS (cr)
2 hydrate
-838.47[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)