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18NaHSO4 + 16e− → 9Na2SO4 + 2HS− + 8H2O + 7SO42−

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Reduction of sodium hydrogensulfate
18NaHSO4Sodium hydrogensulfate + 16e−Electron
⟶
9Na2SO4Sodium sulfate + 2HS−Hydrogensulfide ion + 8H2OWater + 7SO42−Sulfate ion

Reduction of sodium hydrogensulfate yields sodium sulfate, hydrogensulfide ion, water, 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 sodium hydrogensulfate
18NaHSO4Sodium hydrogensulfate + 16e−Electron
⟶
9Na2SO4Sodium sulfate + 2HS−Hydrogensulfide ion + 8H2OWater + 7SO42−Sulfate ion

General equation

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

Oxidation state of each atom

Reduction of sodium hydrogensulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaHSO4Sodium hydrogensulfate18
Oxidizing
–
e−Electron16
–
Electron

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO4Sodium sulfate9
–
–
HS−Hydrogensulfide ion2
Reduced
–
H2OWater8
–
–
SO42−Sulfate ion7
–
–

Thermodynamic changes

Changes in standard condition

Reduction of sodium hydrogensulfate
◆
ΔrG−179.42 kJ/mol
K2.71 × 1031
pK−31.43
18NaHSO4Ionized aqueous solution + 16e−
⟶
9Na2SO4Ionized aqueous solution + 2HS−Un-ionized aqueous solution + 8H2OLiquid + 7SO42−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
−898.0−179.42−1365.9–
−49.89−9.9678−75.883–
per 1 mol of
Electron
−56.13−11.214−85.369–
per 1 mol of
−99.78−19.936−151.77–
per 1 mol of
Hydrogensulfide ion
−449.0−89.710−682.95–
per 1 mol of
−112.3−22.427−170.74–
per 1 mol of
Sulfate ion
−128.3−25.631−195.13–

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
NaHSO4 (cr)-1125.5[1]-992.8[1]113.0[1]–
NaHSO4 (ai)-1127.46[1]-1017.80[1]190.8[1]-38[1]
NaHSO4 (cr)
1 hydrate
-1421.7[1]-1231.6[1]155[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
Na2SO4 (cr)
orthorhombic
-1387.08[1]-1270.16[1]149.58[1]128.20[1]
Na2SO4 (cr)
metastable
––154.934[1]129.29[1]
Na2SO4 (ai)-1389.51[1]-1268.36[1]138.1[1]-201[1]
Na2SO4 (cr)
10 hydrate
-4327.26[1]-3646.85[1]592.0[1]–
HS− (ao)-17.6[1]12.08[1]62.8[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]
SO42− (ao)-909.27[1]-744.53[1]20.1[1]-293[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (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)