You-iggy

3Rb2S + 8HNO3 → 3Rb2SO4 + 8NO↑ + 4H2O

The reaction of rubidium sulfide and nitric acid yields rubidium sulfate, nitrogen monoxide, 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
Rb2SRubidium sulfide3
Reducing
Reducing
HNO3Nitric acid8
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Rb2SO4Rubidium sulfate3
Oxidized
NONitrogen monoxide8
Reduced
H2OWater4

Thermodynamic changes

Changes in standard condition

Reaction of rubidium sulfide and nitric acid
3Rb2SCrystalline solid + 8HNO3Liquid
3Rb2SO4Crystalline solid + 8NOGas + 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
−2253.3
per 1 mol of
−751.10
per 1 mol of
−281.66
per 1 mol of
−751.10
per 1 mol of
−281.66
per 1 mol of
−563.33

Changes in aqueous solution

Reaction of rubidium sulfide and nitric acid
ΔrG−1857.6 kJ/mol
K2.74 × 10325
pK−325.44
3Rb2SIonized aqueous solution + 8HNO3Ionized aqueous solution
3Rb2SO4Ionized aqueous solution + 8NOGas + 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
−1589.0−1857.6898.9
per 1 mol of
−529.67−619.20299.6
per 1 mol of
−198.63−232.20112.4
per 1 mol of
−529.67−619.20299.6
per 1 mol of
−198.63−232.20112.4
per 1 mol of
−397.25−464.40224.7

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
Rb2S (cr)-360.7[1]
Rb2S (ai)-469.4[1]-482.0[1]228.4[1]
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas

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]
NO (g)90.25[1]86.55[1]210.761[1]29.844[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)