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8Cu + RbNO3 + 2H2O → 4Cu2O + NH3↑ + RbOH

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Reaction of copper and rubidium nitrate under neutral condition
8CuCopper + RbNO3Rubidium nitrate + 2H2OWater
⟶
4Cu2OCopper(I) oxide + NH3↑Ammonia + RbOHRubidium hydroxide

The reaction of copper, rubidium nitrate, and water yields copper(I) oxide, ammonia, and rubidium hydroxide (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 copper and rubidium nitrate under neutral condition
8CuCopper + RbNO3Rubidium nitrate + 2H2OWater
⟶
4Cu2OCopper(I) oxide + NH3↑Ammonia + RbOHRubidium hydroxide

General equation

Reaction of oxidizable species and oxidizing species under neutral condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of copper and rubidium nitrate under neutral condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper8
Reducing
Oxidizable
RbNO3Rubidium nitrate1
Oxidizing
Oxidizing
H2OWater2
–
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu2OCopper(I) oxide4
Oxidized
–
NH3Ammonia1
Reduced
–
RbOHRubidium hydroxide1
–
–

Thermodynamic changes

Changes in standard condition

Reaction of copper and rubidium nitrate under neutral condition
8CuCrystalline solid + RbNO3Crystalline solid + 2H2OLiquid
⟶
4Cu2OCrystalline solid + NH3↑Gas + RbOHCrystalline solid
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
−72.0–––
per 1 mol of
−9.00–––
per 1 mol of
−72.0–––
per 1 mol of
−36.0–––
per 1 mol of
−18.0–––
per 1 mol of
−72.0–––
per 1 mol of
−72.0–––

Changes in aqueous solution (1)

Reaction of copper and rubidium nitrate under neutral condition
◆
ΔrG−172.2 kJ/mol
K1.47 × 1030
pK−30.17
8CuCrystalline solid + RbNO3Ionized aqueous solution + 2H2OLiquid
⟶
4Cu2OCrystalline solid + NH3↑Gas + RbOHIonized 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
−171.5−172.22.9–
per 1 mol of
−21.44−21.520.36–
per 1 mol of
−171.5−172.22.9–
per 1 mol of
−85.75−86.101.4–
per 1 mol of
−42.88−43.050.72–
per 1 mol of
−171.5−172.22.9–
per 1 mol of
−171.5−172.22.9–

Changes in aqueous solution (2)

Reaction of copper and rubidium nitrate under neutral condition
◆
ΔrG−182.2 kJ/mol
K8.32 × 1031
pK−31.92
8CuCrystalline solid + RbNO3Ionized aqueous solution + 2H2OLiquid
⟶
4Cu2OCrystalline solid + NH3↑Un-ionized aqueous solution + RbOHIonized 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
−205.7−182.2−78.2–
per 1 mol of
−25.71−22.77−9.78–
per 1 mol of
−205.7−182.2−78.2–
per 1 mol of
−102.8−91.10−39.1–
per 1 mol of
−51.42−45.55−19.6–
per 1 mol of
−205.7−182.2−78.2–
per 1 mol of
−205.7−182.2−78.2–

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
Cu (cr)0[1]0[1]33.150[1]24.435[1]
Cu (g)338.32[1]298.58[1]166.38[1]20.786[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]–
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

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
Cu2O (cr)-168.6[1]-146.0[1]93.14[1]63.64[1]
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[1]–
RbOH (cr)-418.19[1]–––
RbOH (g)-238[1]–––
RbOH (ai)-481.16[1]-441.21[1]110.75[1]–
RbOH (cr)
1 hydrate
-748.85[1]–––
RbOH (cr)
2 hydrate
-1053.24[1]–––
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (ai):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)