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16Na + 10KHSO4 → 8Na2SO4 + 2K2S + 3K2O + 5H2O

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Reaction of sodium and potassium hydrogensulfate
16NaSodium + 10KHSO4Potassium hydrogensulfate
⟶
8Na2SO4Sodium sulfate + 2K2SPotassium sulfide + 3K2OPotassium oxide + 5H2OWater

The reaction of sodium and potassium hydrogensulfate yields sodium sulfate, potassium sulfide, potassium oxide, 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

Reaction of sodium and potassium hydrogensulfate
16NaSodium + 10KHSO4Potassium hydrogensulfate
⟶
8Na2SO4Sodium sulfate + 2K2SPotassium sulfide + 3K2OPotassium oxide + 5H2OWater

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of sodium and potassium hydrogensulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium16
Reducing
Reducing
KHSO4Potassium hydrogensulfate10
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO4Sodium sulfate8
Oxidized
–
K2SPotassium sulfide2
Reduced
–
K2OPotassium oxide3
–
–
H2OWater5
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium and potassium hydrogensulfate
◆
ΔrG−2728.2 kJ/mol
K9.12 × 10477
pK−477.96
16NaCrystalline solid + 10KHSO4Crystalline solid
⟶
8Na2SO4Crystalline solidorthorhombic + 2K2SCrystalline solid + 3K2OCrystalline solid + 5H2OLiquid
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
−2765.7−2728.2−162–
per 1 mol of
−172.86−170.51−10.1–
−276.57−272.82−16.2–
per 1 mol of
−345.71−341.02−20.3–
per 1 mol of
−1382.8−1364.1−81.0–
per 1 mol of
−921.90−909.40−54.0–
per 1 mol of
−553.14−545.64−32.4–

Changes in standard condition (2)

Reaction of sodium and potassium hydrogensulfate
16NaCrystalline solid + 10KHSO4Crystalline solid
⟶
8Na2SO4Crystalline solidmetastable + 2K2SCrystalline solid + 3K2OCrystalline solid + 5H2OLiquid
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
––−119–
per 1 mol of
––−7.44–
––−11.9–
per 1 mol of
––−14.9–
per 1 mol of
––−59.5–
per 1 mol of
––−39.7–
per 1 mol of
––−23.8–

Changes in aqueous solution

Reaction of sodium and potassium hydrogensulfate
◆
ΔrG−2868.4 kJ/mol
K3.33 × 10502
pK−502.52
16NaCrystalline solid + 10KHSO4Ionized aqueous solution
⟶
8Na2SO4Ionized aqueous solution + 2K2SIonized aqueous solution + 3K2OCrystalline solid + 5H2OLiquid
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
−3175.5−2868.4−1044.9–
per 1 mol of
−198.47−179.28−65.306–
−317.55−286.84−104.49–
per 1 mol of
−396.94−358.55−130.61–
per 1 mol of
−1587.8−1434.2−522.45–
per 1 mol of
−1058.5−956.13−348.30–
per 1 mol of
−635.10−573.68−208.98–

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
Na (cr)0[1]0[1]51.21[1]28.24[1]
Na (g)107.32[1]76.761[1]153.712[1]20.786[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]
* (cr):Crystalline solid, (g):Gas, (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]–
K2S (cr)-380.7[1]-364.0[1]105[1]–
K2S (ai)-471.5[1]-480.7[1]190.4[1]–
K2S (cr)
2 hydrate
-975.3[1]–––
K2S (cr)
5 hydrate
-1871.5[1]–––
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[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, (ai):Ionized aqueous solution, (g):Gas, (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)
    • 2
      James G. Speight (2017)
      Lange's Handbook of Chemistry, 17th edition
      McGraw Hill Education