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2KHS + 2e− → 2K + S22− + H2↑

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Reduction of potassium hydrogensulfide
2KHSPotassium hydrogensulfide + 2e−Electron
⟶
2KPotassium + S22−Disulfide ion + H2↑Hydrogen

Reduction of potassium hydrogensulfide yields potassium, disulfide ion, and hydrogen (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 hydrogensulfide
2KHSPotassium hydrogensulfide + 2e−Electron
⟶
2KPotassium + S22−Disulfide ion + H2↑Hydrogen

General equation

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

Oxidation state of each atom

Reduction of potassium hydrogensulfide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KHSPotassium hydrogensulfide2
Oxidizing
–
e−Electron2
–
Electron

Products

Chemical formulaNameCoefficientTypeType in general
equation
KPotassium2
Reduced
–
S22−Disulfide ion1
–
–
H2Hydrogen1
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reduction of potassium hydrogensulfide
◆
ΔrG621.9 kJ/mol
K0.11 × 10−108
pK108.95
2KHSIonized aqueous solution + 2e−
⟶
2KCrystalline solid + S22−Un-ionized aqueous solution + H2↑Gas
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
569.9621.9−43.1–
284.9310.9−21.6–
per 1 mol of
Electron
284.9310.9−21.6–
per 1 mol of
284.9310.9−21.6–
per 1 mol of
Disulfide ion
569.9621.9−43.1–
per 1 mol of
569.9621.9−43.1–

Changes in standard condition (2)

Reduction of potassium hydrogensulfide
◆
ΔrG639.5 kJ/mol
K0.92 × 10−112
pK112.04
2KHSIonized aqueous solution + 2e−
⟶
2KCrystalline solid + S22−Un-ionized aqueous solution + H2↑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
565.7639.5403–
282.9319.8202–
per 1 mol of
Electron
282.9319.8202–
per 1 mol of
282.9319.8202–
per 1 mol of
Disulfide ion
565.7639.5403–
per 1 mol of
565.7639.5403–

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
KHS (cr)-265.10[1]––75.31[1]
KHS (ai)-269.9[1]-271.19[1]165.3[1]–
KHS (cr)
0.25 hydrate
-337.2[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
K (cr)0[1]0[1]64.18[1]29.58[1]
K (g)89.24[1]60.59[1]160.336[1]20.786[1]
S22− (ao)30.1[1]79.5[1]28.5[1]–
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
* (cr):Crystalline solid, (g):Gas, (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)