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18Na + 2KHSO4 → Na2S + 8Na2O + K2S + H2↑

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Reaction of sodium and potassium hydrogensulfate
18NaSodium + 2KHSO4Potassium hydrogensulfate
⟶
Na2SSodium sulfide + 8Na2OSodium oxide + K2SPotassium sulfide + H2↑Hydrogen

The reaction of sodium and potassium hydrogensulfate yields sodium sulfide, sodium oxide, potassium sulfide, 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
18NaSodium + 2KHSO4Potassium hydrogensulfate
⟶
Na2SSodium sulfide + 8Na2OSodium oxide + K2SPotassium sulfide + H2↑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
NaSodium18
Reducing
Reducing
KHSO4Potassium hydrogensulfate2
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2SSodium sulfide1
Redoxed product
–
Na2OSodium oxide8
Oxidized
–
K2SPotassium sulfide1
Reduced
–
H2Hydrogen1
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of sodium and potassium hydrogensulfate
◆
ΔrG−1654.9 kJ/mol
K8.43 × 10289
pK−289.93
18NaCrystalline solid + 2KHSO4Crystalline solid
⟶
Na2SCrystalline solid + 8Na2OCrystalline solid + K2SCrystalline solid + 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
−1738.1−1654.9−278–
per 1 mol of
−96.561−91.939−15.4–
−869.05−827.45−139–
per 1 mol of
−1738.1−1654.9−278–
per 1 mol of
−217.26−206.86−34.8–
per 1 mol of
−1738.1−1654.9−278–
per 1 mol of
−1738.1−1654.9−278–

Changes in aqueous solution (1)

Reaction of sodium and potassium hydrogensulfate
◆
ΔrG−1844.1 kJ/mol
K1.18 × 10323
pK−323.07
18NaCrystalline solid + 2KHSO4Ionized aqueous solution
⟶
Na2SIonized aqueous solution + 8Na2OCrystalline solid + K2SIonized 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
−1953.1−1844.1−365.5–
per 1 mol of
−108.51−102.45−20.31–
−976.55−922.05−182.8–
per 1 mol of
−1953.1−1844.1−365.5–
per 1 mol of
−244.14−230.51−45.69–
per 1 mol of
−1953.1−1844.1−365.5–
per 1 mol of
−1953.1−1844.1−365.5–

Changes in aqueous solution (2)

Reaction of sodium and potassium hydrogensulfate
◆
ΔrG−1826.5 kJ/mol
K9.75 × 10319
pK−319.99
18NaCrystalline solid + 2KHSO4Ionized aqueous solution
⟶
Na2SIonized aqueous solution + 8Na2OCrystalline solid + K2SIonized 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
−1957.3−1826.581–
per 1 mol of
−108.74−101.474.5–
−978.65−913.2541–
per 1 mol of
−1957.3−1826.581–
per 1 mol of
−244.66−228.3110–
per 1 mol of
−1957.3−1826.581–
per 1 mol of
−1957.3−1826.581–

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
Na2S (cr)-364.8[1]-349.8[1]83.7[1]–
Na2S (ai)-447.3[1]-438.1[1]103.3[1]–
Na2S (cr)
4.5 hydrate
-1725.9[1]–––
Na2S (cr)
5 hydrate
-1886.6[1]–––
Na2S (cr)
9 hydrate
-3074.0[1]–––
Na2O (cr)-414.22[1]-375.46[1]75.06[1]69.12[1]
Na2O (g)-35.6[1]-52.3[1]261.2[1]55.2[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]–––
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)