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10Na + Rb2SO4 → Na2S + 4Na2O + 2Rb

The reaction of sodium and rubidium sulfate yields sodium sulfide, sodium oxide, and rubidium (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

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
NaSodium10
Reducing
Reducing
Rb2SO4Rubidium sulfate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2SSodium sulfide1
Redoxed product
Na2OSodium oxide4
Oxidized
RbRubidium2
Reduced

Thermodynamic changes

Changes in standard condition

Reaction of sodium and rubidium sulfate
ΔrG−534.8 kJ/mol
K4.93 × 1093
pK−93.69
10NaCrystalline solid + Rb2SO4Crystalline solid
Na2SCrystalline solid + 4Na2OCrystalline solid + 2RbCrystalline 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
−586.1−534.8−172.0
per 1 mol of
−58.61−53.48−17.20
per 1 mol of
−586.1−534.8−172.0
per 1 mol of
−586.1−534.8−172.0
per 1 mol of
−146.5−133.7−43.00
per 1 mol of
−293.1−267.4−86.00

Changes in aqueous solution

Reaction of sodium and rubidium sulfate
ΔrG−627.4 kJ/mol
K8.24 × 10109
pK−109.92
10NaCrystalline solid + Rb2SO4Ionized aqueous solution
Na2SIonized aqueous solution + 4Na2OCrystalline solid + 2RbCrystalline 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
−692.6−627.4−218.2
per 1 mol of
−69.26−62.74−21.82
per 1 mol of
−692.6−627.4−218.2
per 1 mol of
−692.6−627.4−218.2
per 1 mol of
−173.2−156.8−54.55
per 1 mol of
−346.3−313.7−109.1

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
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]
Rb (cr)0[1]0[1]76.78[1]31.062[1]
Rb (g)80.88[1]53.06[1]170.089[1]20.786[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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)