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14KHSO4 + 8e− → 7K2SO4 + S2− + 6HSO4− + 4H2O

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Reduction of potassium hydrogensulfate
14KHSO4Potassium hydrogensulfate + 8e−Electron
⟶
7K2SO4Potassium sulfate + S2−Sulfide ion + 6HSO4−Hydrogensulfate ion + 4H2OWater

Reduction of potassium hydrogensulfate yields potassium sulfate, sulfide ion, hydrogensulfate ion, 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

Reduction of potassium hydrogensulfate
14KHSO4Potassium hydrogensulfate + 8e−Electron
⟶
7K2SO4Potassium sulfate + S2−Sulfide ion + 6HSO4−Hydrogensulfate ion + 4H2OWater

General equation

Reduction of reducible species
ReactantOxidizing agent + e−
⟶
ProductReduction product

Oxidation state of each atom

Reduction of potassium hydrogensulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KHSO4Potassium hydrogensulfate14
Oxidizing
–
e−Electron8
–
Electron

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2SO4Potassium sulfate7
–
–
S2−Sulfide ion1
Reduced
–
HSO4−Hydrogensulfate ion6
–
–
H2OWater4
–
–

Thermodynamic changes

Changes in standard condition

Reduction of potassium hydrogensulfate
◆
ΔrG−27.1 kJ/mol
K5.59 × 104
pK−4.75
14KHSO4Ionized aqueous solution + 8e−
⟶
7K2SO4Ionized aqueous solution + S2−Un-ionized aqueous solution + 6HSO4−Un-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
−376.3−27.1−648.7–
−26.88−1.94−46.34–
per 1 mol of
Electron
−47.04−3.39−81.09–
per 1 mol of
−53.76−3.87−92.67–
per 1 mol of
Sulfide ion
−376.3−27.1−648.7–
per 1 mol of
Hydrogensulfate ion
−62.72−4.52−108.1–
per 1 mol of
−94.08−6.78−162.2–

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
KHSO4 (cr)-1160.6[1]-1031.3[1]138.1[1]–
KHSO4 (ai)-1139.72[1]-1039.18[1]234.3[1]-63[1]
e−––––
* (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
K2SO4 (cr)-1437.79[1]-1321.37[1]175.56[1]131.46[1]
K2SO4 (g)-1096[1]-1033[1]364[1]108.8[1]
K2SO4 (ai)-1414.02[1]-1311.07[1]225.1[1]-251[1]
S2− (ao)33.1[1]85.8[1]-14.6[1]–
HSO4− (ao)-887.34[1]-755.91[1]131.8[1]-84[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, (g):Gas, (ai):Ionized aqueous solution, (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)