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2H2S + 4RbNO3 → Rb2SO4 + 2N2O3 + Rb2S + 2H2O

The reaction of hydrogen sulfide and rubidium nitrate yields rubidium sulfate, dinitrogen trioxide, 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

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide2
Reducing
Reducing
RbNO3Rubidium nitrate4
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Rb2SO4Rubidium sulfate1
Oxidized
N2O3Dinitrogen trioxide2
Reduced
Rb2SRubidium sulfide1
H2OWater2

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and rubidium nitrate
2H2SGas + 4RbNO3Crystalline solid
Rb2SO4Crystalline solid + 2N2O3Gas + Rb2SCrystalline solid + 2H2OLiquid
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
−179.1
per 1 mol of
−89.55
per 1 mol of
−44.77
per 1 mol of
−179.1
−89.55
per 1 mol of
−179.1
per 1 mol of
−89.55

Changes in aqueous solution

Reaction of hydrogen sulfide and rubidium nitrate
ΔrG−353.2 kJ/mol
K7.55 × 1061
pK−61.88
2H2SUn-ionized aqueous solution + 4RbNO3Ionized aqueous solution
Rb2SO4Ionized aqueous solution + 2N2O3Gas + Rb2SIonized aqueous solution + 2H2OLiquid
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
−371.7−353.2−57
per 1 mol of
−185.8−176.6−29
per 1 mol of
−92.92−88.30−14
per 1 mol of
−371.7−353.2−57
−185.8−176.6−29
per 1 mol of
−371.7−353.2−57
per 1 mol of
−185.8−176.6−29

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
H2S (g)-20.63[1]-33.56[1]205.79[1]34.23[1]
H2S (ao)-39.7[1]-27.83[1]121[1]
RbNO3 (cr)-495.05[1]-395.78[1]147.3[1]102.1[1]
RbNO3 (ai)-458.52[1]-395.24[1]267.8[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
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]
N2O3 (l)50.29[1]
N2O3 (g)83.72[1]139.46[1]312.28[1]65.61[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, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid

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)