You-iggy
  1. Home
  2. Chemical reactions
  3. 4HSO3^− → SO4^2− + 2H2O + 3SO2 + 2e^−

4HSO3− → SO42− + 2H2O + 3SO2 + 2e−

Last updated:
Oxidation of hydrogensulfurous ion
4HSO3−Hydrogensulfurous ion
⟶
SO42−Sulfate ion + 2H2OWater + 3SO2Sulfur dioxide + 2e−Electron

Oxidation of hydrogensulfurous ion yields sulfate ion, water, 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
4HSO3−Hydrogensulfurous ion
⟶
SO42−Sulfate ion + 2H2OWater + 3SO2Sulfur 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 ion4
Reducing
–

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO42−Sulfate ion1
Oxidized
–
H2OWater2
–
–
SO2Sulfur dioxide3
–
–
e−Electron2
–
Electron

Thermodynamic changes

Changes in standard condition (1)

Oxidation of hydrogensulfurous ion
◆
ΔrG−8.45 kJ/mol
K3.02 × 101
pK−1.48
4HSO3−Un-ionized aqueous solution
⟶
SO42−Un-ionized aqueous solution + 2H2OLiquid + 3SO2Gas + 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
133.46−8.45345.8–
per 1 mol of
Hydrogensulfurous ion
33.365−2.1186.45–
per 1 mol of
Sulfate ion
133.46−8.45345.8–
per 1 mol of
66.730−4.22172.9–
per 1 mol of
44.487−2.82115.3–
per 1 mol of
Electron
66.730−4.22172.9–

Changes in standard condition (2)

Oxidation of hydrogensulfurous ion
◆
ΔrG−9.90 kJ/mol
K5.43 × 101
pK−1.73
4HSO3−Un-ionized aqueous solution
⟶
SO42−Un-ionized aqueous solution + 2H2OLiquid + 3SO2Un-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
55.01−9.9086.8–
per 1 mol of
Hydrogensulfurous ion
13.75−2.4821.7–
per 1 mol of
Sulfate ion
55.01−9.9086.8–
per 1 mol of
27.50−4.9543.4–
per 1 mol of
18.34−3.3028.9–
per 1 mol of
Electron
27.50−4.9543.4–

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
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
SO42− (ao)-909.27[1]-744.53[1]20.1[1]-293[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]
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−––––
* (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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)