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3HSO3− → S2O62− + H3O+ + SO2 + 2e−

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Oxidation of hydrogensulfurous ion
3HSO3−Hydrogensulfurous ion
⟶
S2O62−Dithionate ion + H3O+Hydronium ion + SO2Sulfur dioxide + 2e−Electron

Oxidation of hydrogensulfurous ion yields dithionate ion, hydronium ion, sulfur dioxide (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

Oxidation of hydrogensulfurous ion
3HSO3−Hydrogensulfurous ion
⟶
S2O62−Dithionate ion + H3O+Hydronium ion + SO2Sulfur dioxide + 2e−Electron

General equation

Oxidation of oxidizable species
ReactantReducing agent
⟶
ProductOxidation product + e−

Oxidation state of each atom

Oxidation of hydrogensulfurous ion

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HSO3−Hydrogensulfurous ion3
Reducing
–

Products

Chemical formulaNameCoefficientTypeType in general
equation
S2O62−Dithionate ion1
Oxidized
–
H3O+Hydronium ion1
–
–
SO2Sulfur dioxide1
–
–
e−Electron2
–
Electron

Thermodynamic changes

Changes in standard condition (1)

Oxidation of hydrogensulfurous ion
3HSO3−Un-ionized aqueous solution
⟶
S2O62−Aqueous solution + H3O+Un-ionized aqueous solution + SO2Gas + 2e−
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
97.7–––
per 1 mol of
Hydrogensulfurous ion
32.6–––
per 1 mol of
Dithionate ion
97.7–––
per 1 mol of
Hydronium ion
97.7–––
per 1 mol of
97.7–––
per 1 mol of
Electron
48.9–––

Changes in standard condition (2)

Oxidation of hydrogensulfurous ion
3HSO3−Un-ionized aqueous solution
⟶
S2O62−Aqueous solution + H3O+Un-ionized aqueous solution + SO2Un-ionized aqueous solution + 2e−
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
71.6–––
per 1 mol of
Hydrogensulfurous ion
23.9–––
per 1 mol of
Dithionate ion
71.6–––
per 1 mol of
Hydronium ion
71.6–––
per 1 mol of
71.6–––
per 1 mol of
Electron
35.8–––

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
HSO3− (ao)-626.22[1]-527.73[1]139.7[1]–
* (ao):Un-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
S2O62− (aq)-1198.3[1]–––
H3O+ (ao)-285.830[1]-237.129[1]69.91[1]75.291[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]–
e−––––
* (aq):Aqueous solution, (ao):Un-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)