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13H2S + 16KBrO3 → 10KHSO4 + 8Br2 + 3K2S + 8H2O

The reaction of hydrogen sulfide and potassium bromate yields potassium hydrogensulfate, bromine, potassium 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

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 sulfide13
Reducing
Reducing
KBrO3Potassium bromate16
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
KHSO4Potassium hydrogensulfate10
Oxidized
Br2Bromine8
Reduced
K2SPotassium sulfide3
H2OWater8

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and potassium bromate
ΔrG−8527.2 kJ/mol
K7.96 × 101493
pK−1493.90
13H2SGas + 16KBrO3Crystalline solid
10KHSO4Crystalline solid + 8Br2Liquid + 3K2SCrystalline 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
−9002.7−8527.2−1589
per 1 mol of
−692.52−655.94−122.2
per 1 mol of
−562.67−532.95−99.31
−900.27−852.72−158.9
per 1 mol of
−1125.3−1065.9−198.6
per 1 mol of
−3000.9−2842.4−529.7
per 1 mol of
−1125.3−1065.9−198.6

Changes in aqueous solution

Reaction of hydrogen sulfide and potassium bromate
ΔrG−9103.0 kJ/mol
K5.98 × 101594
pK−1594.78
13H2SUn-ionized aqueous solution + 16KBrO3Ionized aqueous solution
10KHSO4Ionized aqueous solution + 8Br2Un-ionized aqueous solution + 3K2SIonized 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
−9491.8−9103.0−1283
per 1 mol of
−730.14−700.23−98.69
per 1 mol of
−593.24−568.94−80.19
−949.18−910.30−128.3
per 1 mol of
−1186.5−1137.9−160.4
per 1 mol of
−3163.9−3034.3−427.7
per 1 mol of
−1186.5−1137.9−160.4

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]
KBrO3 (cr)-360.24[1]-271.16[1]149.16[1]105.19[1]
KBrO3 (ai)-319.45[1]-264.67[1]264.22[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
KHSO4 (cr)-1160.6[1]-1031.3[1]138.1[1]
KHSO4 (ai)-1139.72[1]-1039.18[1]234.3[1]-63[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]
K2S (cr)-380.7[1]-364.0[1]105[1]
K2S (ai)-471.5[1]-480.7[1]190.4[1]
K2S (cr)
2 hydrate
-975.3[1]
K2S (cr)
5 hydrate
-1871.5[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, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (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)