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4H2 + Rb2SO4 → Rb2S + 4H2O

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Reaction of hydrogen and rubidium sulfate
4H2Hydrogen + Rb2SO4Rubidium sulfate
⟶
Rb2SRubidium sulfide + 4H2OWater

The reaction of hydrogen and rubidium sulfate yields rubidium sulfide 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 hydrogen and rubidium sulfate
4H2Hydrogen + Rb2SO4Rubidium sulfate
⟶
Rb2SRubidium sulfide + 4H2OWater

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 hydrogen and rubidium sulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2Hydrogen4
Reducing
Reducing
Rb2SO4Rubidium sulfate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Rb2SRubidium sulfide1
Reduced
–
H2OWater4
Oxidized
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen and rubidium sulfate
4H2Gas + Rb2SO4Crystalline solid
⟶
Rb2SCrystalline solid + 4H2OLiquid
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
−68.4–––
per 1 mol of
−17.1–––
per 1 mol of
−68.4–––
per 1 mol of
−68.4–––
per 1 mol of
−17.1–––

Changes in aqueous solution

Reaction of hydrogen and rubidium sulfate
◆
ΔrG−188.4 kJ/mol
K1.01 × 1033
pK−33.01
4H2Un-ionized aqueous solution + Rb2SO4Ionized aqueous solution
⟶
Rb2SIonized aqueous solution + 4H2OLiquid
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
−184.3−188.4−2063–
per 1 mol of
−46.08−47.10−515.8–
per 1 mol of
−184.3−188.4−2063–
per 1 mol of
−184.3−188.4−2063–
per 1 mol of
−46.08−47.10−515.8–

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
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[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]–
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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
Rb2S (cr)-360.7[1]–––
Rb2S (ai)-469.4[1]-482.0[1]228.4[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, (l):Liquid, (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)