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3H2S + 4NaIO3 → 2Na2SO4 + H2SO4 + 4HI

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Reaction of hydrogen sulfide and sodium iodate
3H2SHydrogen sulfide + 4NaIO3Sodium iodate
⟶
2Na2SO4Sodium sulfate + H2SO4Sulfuric acid + 4HIHydrogen iodide

The reaction of hydrogen sulfide and sodium iodate yields sodium sulfate, sulfuric acid, and hydrogen iodide (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
3H2SHydrogen sulfide + 4NaIO3Sodium iodate
⟶
2Na2SO4Sodium sulfate + H2SO4Sulfuric acid + 4HIHydrogen iodide

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 sulfide3
Reducing
Reducing
NaIO3Sodium iodate4
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO4Sodium sulfate2
Oxidized
–
H2SO4Sulfuric acid1
Oxidized
–
HIHydrogen iodide4
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and sodium iodate
3H2SGas + 4NaIO3Crystalline solid
⟶
2Na2SO4Crystalline solidorthorhombic + H2SO4Liquid + 4HIGas
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
−1493.19––41.3
per 1 mol of
−497.730––13.8
per 1 mol of
−373.298––10.3
per 1 mol of
−746.595––20.6
per 1 mol of
−1493.19––41.3
per 1 mol of
−373.298––10.3

Changes in standard condition (2)

Reaction of hydrogen sulfide and sodium iodate
3H2SGas + 4NaIO3Crystalline solid
⟶
2Na2SO4Crystalline solidmetastable + H2SO4Liquid + 4HIGas
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
–––43.4
per 1 mol of
–––14.5
per 1 mol of
–––10.8
per 1 mol of
–––21.7
per 1 mol of
–––43.4
per 1 mol of
–––10.8

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and sodium iodate
◆
ΔrG−1631.4 kJ/mol
K6.44 × 10285
pK−285.81
3H2SUn-ionized aqueous solution + 4NaIO3Ionized aqueous solution
⟶
2Na2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 4HIGas
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
−1617.3−1631.450–
per 1 mol of
−539.10−543.8017–
per 1 mol of
−404.32−407.8513–
per 1 mol of
−808.65−815.7025–
per 1 mol of
−1617.3−1631.450–
per 1 mol of
−404.32−407.8513–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and sodium iodate
◆
ΔrG−1844.4 kJ/mol
K1.33 × 10323
pK−323.12
3H2SUn-ionized aqueous solution + 4NaIO3Ionized aqueous solution
⟶
2Na2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 4HIIonized 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
−1944.0−1844.4−331–
per 1 mol of
−648.00−614.80−110–
per 1 mol of
−486.00−461.10−82.8–
per 1 mol of
−972.00−922.20−166–
per 1 mol of
−1944.0−1844.4−331–
per 1 mol of
−486.00−461.10−82.8–

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]–
H2SO4 (cr)––––
H2SO4 (l)-813.989[1]-690.003[1]156.904[1]138.91[1]
H2SO4 (ai)-909.27[1]-744.53[1]20.1[1]-293[1]
H2SO4 (l)
1 hydrate
-1127.621[1]-950.383[1]211.54[1]214.85[1]
H2SO4 (l)
2 hydrate
-1427.100[1]-1199.650[1]276.40[1]260.83[1]
H2SO4 (l)
3 hydrate
-1720.402[1]-1443.980[1]345.39[1]318.95[1]
H2SO4 (l)
4 hydrate
-2011.199[1]-1685.863[1]414.59[1]382.21[1]
H2SO4 (l)
6.5 hydrate
-2733.256[1]-2285.734[1]587.89[1]570.28[1]
HI (g)26.48[1]1.70[1]206.594[1]29.158[1]
HI (ai)-55.19[1]-51.57[1]111.3[1]-142.3[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (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)