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6Na + 4KHSO4 → 3Na2SO4 + K2SO3 + K2O + 2H2↑

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Reaction of sodium and potassium hydrogensulfate
6NaSodium + 4KHSO4Potassium hydrogensulfate
⟶
3Na2SO4Sodium sulfate + K2SO3Potassium sulfite + K2OPotassium oxide + 2H2↑Hydrogen

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

Reaction of sodium and potassium hydrogensulfate
6NaSodium + 4KHSO4Potassium hydrogensulfate
⟶
3Na2SO4Sodium sulfate + K2SO3Potassium sulfite + K2OPotassium oxide + 2H2↑Hydrogen

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
NaSodium6
Reducing
Reducing
KHSO4Potassium hydrogensulfate4
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO4Sodium sulfate3
Oxidized
–
K2SO3Potassium sulfite1
Reduced
–
K2OPotassium oxide1
–
–
H2Hydrogen2
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium and potassium hydrogensulfate
6NaCrystalline solid + 4KHSO4Crystalline solid
⟶
3Na2SO4Crystalline solidorthorhombic + K2SO3Crystalline solid + K2OCrystalline solid + 2H2↑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
−1005.8–––
per 1 mol of
−167.63–––
−251.45–––
per 1 mol of
−335.27–––
per 1 mol of
−1005.8–––
per 1 mol of
−1005.8–––
per 1 mol of
−502.90–––

Changes in standard condition (2)

Reaction of sodium and potassium hydrogensulfate
6NaCrystalline solid + 4KHSO4Crystalline solid
⟶
3Na2SO4Crystalline solidmetastable + K2SO3Crystalline solid + K2OCrystalline solid + 2H2↑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
––––
per 1 mol of
––––
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––

Changes in aqueous solution (1)

Reaction of sodium and potassium hydrogensulfate
◆
ΔrG−1023.6 kJ/mol
K2.12 × 10179
pK−179.33
6NaCrystalline solid + 4KHSO4Ionized aqueous solution
⟶
3Na2SO4Ionized aqueous solution + K2SO3Ionized aqueous solution + K2OCrystalline solid + 2H2↑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
−1111.3−1023.6−299–
per 1 mol of
−185.22−170.60−49.8–
−277.82−255.90−74.8–
per 1 mol of
−370.43−341.20−99.7–
per 1 mol of
−1111.3−1023.6−299–
per 1 mol of
−1111.3−1023.6−299–
per 1 mol of
−555.65−511.80−150–

Changes in aqueous solution (2)

Reaction of sodium and potassium hydrogensulfate
◆
ΔrG−988.4 kJ/mol
K1.45 × 10173
pK−173.16
6NaCrystalline solid + 4KHSO4Ionized aqueous solution
⟶
3Na2SO4Ionized aqueous solution + K2SO3Ionized aqueous solution + K2OCrystalline solid + 2H2↑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
−1119.7−988.4594–
per 1 mol of
−186.62−164.799.0–
−279.93−247.1149–
per 1 mol of
−373.23−329.5198–
per 1 mol of
−1119.7−988.4594–
per 1 mol of
−1119.7−988.4594–
per 1 mol of
−559.85−494.2297–

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]–
K2SO3 (cr)-1125.5[1]–––
K2SO3 (ai)-1140.1[1]-1053.1[1]176[1]–
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[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, (ai):Ionized aqueous solution, (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)
    • 2
      James G. Speight (2017)
      Lange's Handbook of Chemistry, 17th edition
      McGraw Hill Education