You-iggy
  1. Home
  2. Chemical reactions
  3. 12KHSO4 + 6e^− → 6K2SO4 + S + 4H3O^+ + 5SO4^2−

12KHSO4 + 6e− → 6K2SO4 + S + 4H3O+ + 5SO42−

Last updated:
Reduction of potassium hydrogensulfate
12KHSO4Potassium hydrogensulfate + 6e−Electron
⟶
6K2SO4Potassium sulfate + SSulfur + 4H3O+Hydronium ion + 5SO42−Sulfate ion

Reduction of potassium hydrogensulfate yields potassium sulfate, sulfur, hydronium ion, and sulfate 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

Reduction of potassium hydrogensulfate
12KHSO4Potassium hydrogensulfate + 6e−Electron
⟶
6K2SO4Potassium sulfate + SSulfur + 4H3O+Hydronium ion + 5SO42−Sulfate ion

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 hydrogensulfate12
Oxidizing
–
e−Electron6
–
Electron

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2SO4Potassium sulfate6
–
–
SSulfur1
Reduced
–
H3O+Hydronium ion4
–
–
SO42−Sulfate ion5
–
–

Thermodynamic changes

Changes in standard condition

Reduction of potassium hydrogensulfate
◆
ΔrG−67.43 kJ/mol
K6.50 × 1011
pK−11.81
12KHSO4Ionized aqueous solution + 6e−
⟶
6K2SO4Ionized aqueous solution + SCrystalline solidrhombic + 4H3O+Un-ionized aqueous solution + 5SO42−Un-ionized 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
−497.15−67.43−1049.1−1891
−41.429−5.619−87.425−157.6
per 1 mol of
Electron
−82.858−11.24−174.85−315.2
per 1 mol of
−82.858−11.24−174.85−315.2
per 1 mol of
−497.15−67.43−1049.1−1891
per 1 mol of
Hydronium ion
−124.29−16.86−262.27−472.8
per 1 mol of
Sulfate ion
−99.430−13.49−209.82−378.2

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]
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]–––
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
H3O+ (ao)-285.830[1]-237.129[1]69.91[1]75.291[1]
SO42− (ao)-909.27[1]-744.53[1]20.1[1]-293[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

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)