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2HSO4− → O2 + 2SO3 + 2H+ + 4e−

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Oxidation of hydrogensulfate ion
2HSO4−Hydrogensulfate ion
⟶
O2Oxygen + 2SO3Sulfur trioxide + 2H+Hydrogen ion + 4e−Electron

Oxidation of hydrogensulfate ion yields oxygen, sulfur trioxide, hydrogen ion (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 hydrogensulfate ion
2HSO4−Hydrogensulfate ion
⟶
O2Oxygen + 2SO3Sulfur trioxide + 2H+Hydrogen ion + 4e−Electron

General equation

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

Oxidation state of each atom

Oxidation of hydrogensulfate ion

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HSO4−Hydrogensulfate ion2
Reducing
–

Products

Chemical formulaNameCoefficientTypeType in general
equation
O2Oxygen1
Oxidized
–
SO3Sulfur trioxide2
–
–
H+Hydrogen ion2
–
–
e−Electron4
–
Electron

Thermodynamic changes

Changes in standard condition (1)

Oxidation of hydrogensulfate ion
◆
ΔrG763.40 kJ/mol
K0.18 × 10−133
pK133.74
2HSO4−Un-ionized aqueous solution
⟶
O2Gas + 2SO3Crystalline solidβ + 2H+Un-ionized aqueous solution + 4e−
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
865.66763.4082.9–
per 1 mol of
Hydrogensulfate ion
432.83381.7041.5–
per 1 mol of
865.66763.4082.9–
per 1 mol of
432.83381.7041.5–
per 1 mol of
Hydrogen ion
432.83381.7041.5–
per 1 mol of
Electron
216.41190.8520.7–

Changes in standard condition (2)

Oxidation of hydrogensulfate ion
◆
ΔrG779.8 kJ/mol
K0.24 × 10−136
pK136.62
2HSO4−Un-ionized aqueous solution
⟶
O2Un-ionized aqueous solution + 2SO3Crystalline solidβ + 2H+Un-ionized aqueous solution + 4e−
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
854.0779.8−11.3–
per 1 mol of
Hydrogensulfate ion
427.0389.9−5.65–
per 1 mol of
854.0779.8−11.3–
per 1 mol of
427.0389.9−5.65–
per 1 mol of
Hydrogen ion
427.0389.9−5.65–
per 1 mol of
Electron
213.5194.9−2.83–

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
HSO4− (ao)-887.34[1]-755.91[1]131.8[1]-84[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
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[1]–
SO3 (cr)
β
-454.51[1]-374.21[1]70.7[1]–
SO3 (l)-441.04[1]-373.75[1]113.8[1]–
SO3 (g)-395.72[1]-371.06[1]256.76[1]50.67[1]
H+ (g)1536.202[1]–––
H+ (ao)0[1]0[1]0[1]0[1]
e−––––
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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)