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Rb2O + 2HF → 2RbF + H2O

The reaction of rubidium oxide and hydrogen fluoride yields rubidium fluoride and water. This reaction is an acid-base reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

General equation

Reaction of basic oxide and acid
Basic oxideBrønsted base + AcidBrønsted acid
SaltConjugate base + H2OConjugate acid

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Rb2ORubidium oxide1
Brønsted base
Basic oxide
Strongly basic oxide
HFHydrogen fluoride2
Brønsted acid
Acid
Weak acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
RbFRubidium fluoride2
Conjugate base
Salt
Salt of weak acid and strong base
H2OWater1
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of rubidium oxide and hydrogen fluoride
Rb2OCrystalline solid + 2HFGas
2RbFCrystalline solid + H2OLiquid
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
−520
per 1 mol of
−520
per 1 mol of
−260
per 1 mol of
−260
per 1 mol of
−520

Changes in aqueous solution (1)

Reaction of rubidium oxide and hydrogen fluoride
Rb2OCrystalline solid + 2HFUn-ionized aqueous solution
2RbFIonized aqueous solution + H2OLiquid
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
−474
per 1 mol of
−474
per 1 mol of
−237
per 1 mol of
−237
per 1 mol of
−474

Changes in aqueous solution (2)

Reaction of rubidium oxide and hydrogen fluoride
Rb2OCrystalline solid + 2HFIonized aqueous solution
2RbFIonized aqueous solution + H2OLiquid
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
−449
per 1 mol of
−449
per 1 mol of
−225
per 1 mol of
−225
per 1 mol of
−449

Changes in aqueous solution (3)

Reaction of rubidium oxide and hydrogen fluoride
Rb2OCrystalline solid + 2HFUn-ionized aqueous solution
2RbFIonized aqueous solution + H2OLiquid
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
−474
per 1 mol of
−474
per 1 mol of
−237
per 1 mol of
−237
per 1 mol of
−474

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
Rb2O (cr)-339[1]
Rb2O (g)-50[1]
HF (l)
x denotes undetermined zero point entropy
-299.78[1]75.40+x[1]
HF (g)-271.1[1]-273.2[1]173.779[1]29.133[1]
HF (ai)-332.63[1]-278.79[1]-13.8[1]-106.7[1]
HF (ao)-320.08[1]-296.82[1]88.7[1]
* (cr):Crystalline solid, (g):Gas, (l):Liquid, (ai):Ionized aqueous solution, (ao):Un-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
RbF (cr)-557.7[1]
RbF (g)-331.4[1]-349.0[1]237.09[1]35.69[1]
RbF (ai)-583.79[1]-562.77[1]107.5[1]
RbF (cr)
1.5 hydrate
-1013.8[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