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2AgOH + Li2O → Ag2O + 2LiOH

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Reaction of silver(I) hydroxide and lithium oxide
2AgOHSilver(I) hydroxide + Li2OLithium oxide
⟶
Ag2OSilver(I) oxide + 2LiOHLithium hydroxide

The reaction of silver(I) hydroxide and lithium oxide yields silver(I) oxide and lithium hydroxide. 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

Reaction of silver(I) hydroxide and lithium oxide
2AgOHSilver(I) hydroxide + Li2OLithium oxide
⟶
Ag2OSilver(I) oxide + 2LiOHLithium hydroxide

General equation

Reaction of hydroxide base and dehydrating basic oxide
Hydroxide baseLewis base + Dehydrating basic oxideLewis acid
⟶
Basic oxide + Hydroxide baseLewis conjugate

Oxidation state of each atom

Reaction of silver(I) hydroxide and lithium oxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
AgOHSilver(I) hydroxide2
Lewis base
Hydroxide base
Li2OLithium oxide1
Lewis acid
Dehydrating basic oxide

Products

Chemical formulaNameCoefficientTypeType in general
equation
Ag2OSilver(I) oxide1
–
Basic oxide
LiOHLithium hydroxide2
Lewis conjugate
Hydroxide base

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of silver(I) hydroxide and lithium oxide
◆
ΔrG−190.91 kJ/mol
K2.79 × 1033
pK−33.45
2AgOHIonized aqueous solution + Li2OCrystalline solid
⟶
Ag2OCrystalline solid + 2LiOHIonized aqueous solution
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
−201.24−190.91−34.5105.6
per 1 mol of
Silver(I) hydroxide
−100.62−95.455−17.352.80
per 1 mol of
−201.24−190.91−34.5105.6
per 1 mol of
−201.24−190.91−34.5105.6
per 1 mol of
−100.62−95.455−17.352.80

Changes in aqueous solution (2)

Reaction of silver(I) hydroxide and lithium oxide
◆
ΔrG−193.3 kJ/mol
K7.32 × 1033
pK−33.86
2AgOHIonized aqueous solution + Li2OCrystalline solid
⟶
Ag2OCrystalline solid + 2LiOHUn-ionized aqueous solution
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
−201.1−193.3−25.9–
per 1 mol of
Silver(I) hydroxide
−100.5−96.65−12.9–
per 1 mol of
−201.1−193.3−25.9–
per 1 mol of
−201.1−193.3−25.9–
per 1 mol of
−100.5−96.65−12.9–

Changes in aqueous solution (3)

Reaction of silver(I) hydroxide and lithium oxide
◆
ΔrG−167.2 kJ/mol
K1.96 × 1029
pK−29.29
2AgOHUn-ionized aqueous solution + Li2OCrystalline solid
⟶
Ag2OCrystalline solid + 2LiOHIonized aqueous solution
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
–−167.2––
per 1 mol of
Silver(I) hydroxide
–−83.60––
per 1 mol of
–−167.2––
per 1 mol of
–−167.2––
per 1 mol of
–−83.60––

Changes in aqueous solution (4)

Reaction of silver(I) hydroxide and lithium oxide
◆
ΔrG−169.6 kJ/mol
K5.16 × 1029
pK−29.71
2AgOHUn-ionized aqueous solution + Li2OCrystalline solid
⟶
Ag2OCrystalline solid + 2LiOHUn-ionized aqueous solution
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
–−169.6––
per 1 mol of
Silver(I) hydroxide
–−84.80––
per 1 mol of
–−169.6––
per 1 mol of
–−169.6––
per 1 mol of
–−84.80––

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
AgOH (ai)-124.415[1]-80.137[1]61.92[1]-126.8[1]
AgOH (ao)–-92.0[1]––
Li2O (cr)-597.94[1]-561.18[1]37.57[1]54.10[1]
Li2O (g)-160.7[1]-181.6[1]231.48[1]49.83[1]
* (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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
Ag2O (cr)-31.05[1]-11.20[1]121.3[1]65.86[1]
LiOH (cr)-484.93[1]-438.95[1]42.80[1]49.66[1]
LiOH (g)-238.1[1]-242.3[1]210.90[1]46.02[1]
LiOH (ai)-508.48[1]-450.58[1]2.80[1]-79.9[1]
LiOH (ao)-508.4[1]-451.8[1]7.1[1]–
LiOH (cr)
1 hydrate
-788.01[1]-680.95[1]71.21[1]79.50[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

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)