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8Na + Rb2SO4 → 4Na2O + Rb2S

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Reaction of sodium and rubidium sulfate
8NaSodium + Rb2SO4Rubidium sulfate
⟶
4Na2OSodium oxide + Rb2SRubidium sulfide

The reaction of sodium and rubidium sulfate yields sodium oxide and rubidium sulfide (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 rubidium sulfate
8NaSodium + Rb2SO4Rubidium sulfate
⟶
4Na2OSodium oxide + Rb2SRubidium sulfide

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 rubidium sulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium8
Reducing
Reducing
Rb2SO4Rubidium sulfate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2OSodium oxide4
Oxidized
–
Rb2SRubidium sulfide1
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of sodium and rubidium sulfate
8NaCrystalline solid + Rb2SO4Crystalline solid
⟶
4Na2OCrystalline solid + Rb2SCrystalline solid
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
−582.0–––
per 1 mol of
−72.75–––
per 1 mol of
−582.0–––
per 1 mol of
−145.5–––
per 1 mol of
−582.0–––

Changes in aqueous solution

Reaction of sodium and rubidium sulfate
◆
ΔrG−671.3 kJ/mol
K4.04 × 10117
pK−117.61
8NaCrystalline solid + Rb2SO4Ionized aqueous solution
⟶
4Na2OCrystalline solid + Rb2SIonized 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
−714.7−671.3−144.2–
per 1 mol of
−89.34−83.91−18.02–
per 1 mol of
−714.7−671.3−144.2–
per 1 mol of
−178.7−167.8−36.05–
per 1 mol of
−714.7−671.3−144.2–

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]
Rb2SO4 (cr)-1435.61[1]-1316.89[1]197.44[1]134.06[1]
Rb2SO4 (g)-1068.6[1]–––
Rb2SO4 (ai)-1411.60[1]-1312.50[1]263.2[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
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]
Rb2S (cr)-360.7[1]–––
Rb2S (ai)-469.4[1]-482.0[1]228.4[1]–
* (cr):Crystalline solid, (g):Gas, (ai):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)