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5H2S + 10NaIO3 → 5Na2SO4 + 4I2 + 2HIO3 + 4H2O

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Reaction of hydrogen sulfide and sodium iodate
5H2SHydrogen sulfide + 10NaIO3Sodium iodate
⟶
5Na2SO4Sodium sulfate + 4I2Iodine + 2HIO3Iodic acid + 4H2OWater

The reaction of hydrogen sulfide and sodium iodate yields sodium sulfate, iodine, iodic acid, 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 iodate
5H2SHydrogen sulfide + 10NaIO3Sodium iodate
⟶
5Na2SO4Sodium sulfate + 4I2Iodine + 2HIO3Iodic acid + 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 sodium iodate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide5
Reducing
Reducing
NaIO3Sodium iodate10
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO4Sodium sulfate5
Oxidized
–
I2Iodine4
Reduced
–
HIO3Iodic acid2
–
–
H2OWater4
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and sodium iodate
5H2SGas + 10NaIO3Crystalline solid
⟶
5Na2SO4Crystalline solidorthorhombic + 4I2Crystalline solid + 2HIO3Crystalline solid + 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
−3617.9–––
per 1 mol of
−723.58–––
per 1 mol of
−361.79–––
per 1 mol of
−723.58–––
per 1 mol of
−904.48–––
per 1 mol of
−1809.0–––
per 1 mol of
−904.48–––

Changes in standard condition (2)

Reaction of hydrogen sulfide and sodium iodate
5H2SGas + 10NaIO3Crystalline solid
⟶
5Na2SO4Crystalline solidmetastable + 4I2Crystalline solid + 2HIO3Crystalline solid + 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
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––

Changes in aqueous solution

Reaction of hydrogen sulfide and sodium iodate
◆
ΔrG−3451.8 kJ/mol
K5.36 × 10604
pK−604.73
5H2SUn-ionized aqueous solution + 10NaIO3Ionized aqueous solution
⟶
5Na2SO4Ionized aqueous solution + 4I2Un-ionized aqueous solution + 2HIO3Un-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
−3609.6−3451.8−526–
per 1 mol of
−721.92−690.36−105–
per 1 mol of
−360.96−345.18−52.6–
per 1 mol of
−721.92−690.36−105–
per 1 mol of
−902.40−862.95−132–
per 1 mol of
−1804.8−1725.9−263–
per 1 mol of
−902.40−862.95−132–

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]–
NaIO3 (cr)-481.788[1]––92.0[1]
NaIO3 (ai)-461.5[1]-389.9[1]177.4[1]–
NaIO3 (cr)
1 hydrate
-779.48[1]-634.03[1]162.3[1]–
NaIO3 (cr)
5 hydrate
-1952.25[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
Na2SO4 (cr)
orthorhombic
-1387.08[1]-1270.16[1]149.58[1]128.20[1]
Na2SO4 (cr)
metastable
––154.934[1]129.29[1]
Na2SO4 (ai)-1389.51[1]-1268.36[1]138.1[1]-201[1]
Na2SO4 (cr)
10 hydrate
-4327.26[1]-3646.85[1]592.0[1]–
I2 (cr)0[1]0[1]116.135[1]54.438[1]
I2 (g)62.438[1]19.327[1]260.69[1]36.90[1]
I2 (ao)22.6[1]16.40[1]137.2[1]–
HIO3 (cr)-230.1[1]–––
HIO3 (ao)-211.3[1]-132.6[1]166.9[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]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid

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)