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3H2S + 4NaBrO3 → 3NaHSO4 + NaBr + 3HBr

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Reaction of hydrogen sulfide and sodium bromate
3H2SHydrogen sulfide + 4NaBrO3Sodium bromate
⟶
3NaHSO4Sodium hydrogensulfate + NaBrSodium bromide + 3HBrHydrogen bromide

The reaction of hydrogen sulfide and sodium bromate yields sodium hydrogensulfate, sodium bromide, and hydrogen bromide (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
3H2SHydrogen sulfide + 4NaBrO3Sodium bromate
⟶
3NaHSO4Sodium hydrogensulfate + NaBrSodium bromide + 3HBrHydrogen bromide

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 sulfide3
Reducing
Reducing
NaBrO3Sodium bromate4
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaHSO4Sodium hydrogensulfate3
Oxidized
–
NaBrSodium bromide1
Reduced
–
HBrHydrogen bromide3
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and sodium bromate
◆
ΔrG−2416.6 kJ/mol
K2.34 × 10423
pK−423.37
3H2SGas + 4NaBrO3Crystalline solid
⟶
3NaHSO4Crystalline solid + NaBrCrystalline solid + 3HBrGas
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
−2448.5−2416.6−111.1–
per 1 mol of
−816.17−805.53−37.03–
per 1 mol of
−612.13−604.15−27.77–
−816.17−805.53−37.03–
per 1 mol of
−2448.5−2416.6−111.1–
per 1 mol of
−816.17−805.53−37.03–

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and sodium bromate
◆
ΔrG−2522.95 kJ/mol
K1.00 × 10442
pK−442.00
3H2SUn-ionized aqueous solution + 4NaBrO3Ionized aqueous solution
⟶
3NaHSO4Ionized aqueous solution + NaBrIonized aqueous solution + 3HBrGas
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
−2505.4−2522.9563–
per 1 mol of
−835.13−840.98321–
per 1 mol of
−626.35−630.73716–
−835.13−840.98321–
per 1 mol of
−2505.4−2522.9563–
per 1 mol of
−835.13−840.98321–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and sodium bromate
◆
ΔrG−2674.48 kJ/mol
K3.54 × 10468
pK−468.55
3H2SUn-ionized aqueous solution + 4NaBrO3Ionized aqueous solution
⟶
3NaHSO4Ionized aqueous solution + NaBrIonized aqueous solution + 3HBrIonized 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
−2760.8−2674.48−286–
per 1 mol of
−920.27−891.493−95.3–
per 1 mol of
−690.20−668.620−71.5–
−920.27−891.493−95.3–
per 1 mol of
−2760.8−2674.48−286–
per 1 mol of
−920.27−891.493−95.3–

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
NaHSO4 (cr)-1125.5[1]-992.8[1]113.0[1]–
NaHSO4 (ai)-1127.46[1]-1017.80[1]190.8[1]-38[1]
NaHSO4 (cr)
1 hydrate
-1421.7[1]-1231.6[1]155[1]–
NaBr (cr)-361.062[1]-348.983[1]86.82[1]51.38[1]
NaBr (g)-143.1[1]-177.06[1]241.19[1]36.32[1]
NaBr (ai)-361.665[1]-365.849[1]141.4[1]-95.4[1]
NaBr (cr)
2 hydrate
-951.94[1]-828.29[1]179.1[1]–
HBr (g)-36.40[1]-53.45[1]198.695[1]29.142[1]
HBr (ai)-121.55[1]-103.96[1]82.4[1]-141.8[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas

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)