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16P + 15Cu(OH)2 → 3Cu3(PO4)2 + 10PH3↑ + 6CuO

The reaction of phosphorus and copper(II) hydroxide yields copper(II) phosphate, phosphine, and copper(II) oxide. 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 categories

Reaction data

Chemical equation

General equation

Reaction of self redoxing species and base
Self-redoxing speciesSelf redox agent + BaseNon-redox agent
ProductOxidation product + ProductReduction product
Reaction of nonmetal and hydroxide base
NonmetalSelf redox agent + Hydroxide base
Oxoacid saltOxidation product + Salt of hydracid/HydrideReduction product + OxideNon-redox product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
PPhosphorus16
Self redoxing
Nonmetal
Cu(OH)2Copper(II) hydroxide15
Base
Hydroxide base

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu3(PO4)2Copper(II) phosphate3
Oxidized
Oxoacid salt
PH3Phosphine10
Reduced
Hydride
CuOCopper(II) oxide6
Oxide

Thermodynamic changes

Changes in standard condition (1)

Reaction of phosphorus and copper(II) hydroxide
16PCrystalline solidwhite + 15Cu(OH)2Crystalline solid
3Cu3(PO4)2Crystalline solid + 10PH3Gas + 6CuOCrystalline 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
per 1 mol of
per 1 mol of
per 1 mol of

Changes in standard condition (2)

Reaction of phosphorus and copper(II) hydroxide
16PCrystalline solidred, triclinic + 15Cu(OH)2Crystalline solid
3Cu3(PO4)2Crystalline solid + 10PH3Gas + 6CuOCrystalline 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
per 1 mol of
per 1 mol of
per 1 mol of

Changes in standard condition (3)

Reaction of phosphorus and copper(II) hydroxide
16PCrystalline solidblack + 15Cu(OH)2Crystalline solid
3Cu3(PO4)2Crystalline solid + 10PH3Gas + 6CuOCrystalline 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
per 1 mol of
per 1 mol of
per 1 mol of

Changes in standard condition (4)

Reaction of phosphorus and copper(II) hydroxide
16PAmorphous solidred + 15Cu(OH)2Crystalline solid
3Cu3(PO4)2Crystalline solid + 10PH3Gas + 6CuOCrystalline 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
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution (1)

Reaction of phosphorus and copper(II) hydroxide
ΔrG−3063.0 kJ/mol
K4.12 × 10536
pK−536.61
16PCrystalline solidwhite + 15Cu(OH)2Ionized aqueous solution
3Cu3(PO4)2Crystalline solid + 10PH3Gas + 6CuOCrystalline 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
−3063.0
per 1 mol of
−191.44
−204.20
−1021.0
per 1 mol of
−306.30
per 1 mol of
−510.50

Changes in aqueous solution (2)

Reaction of phosphorus and copper(II) hydroxide
ΔrG−2943.4 kJ/mol
K4.59 × 10515
pK−515.66
16PCrystalline solidwhite + 15Cu(OH)2Ionized aqueous solution
3Cu3(PO4)2Crystalline solid + 10PH3Un-ionized aqueous solution + 6CuOCrystalline 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
−2943.4
per 1 mol of
−183.96
−196.23
−981.13
per 1 mol of
−294.34
per 1 mol of
−490.57

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
P (cr)
white
0[1]0[1]41.09[1]23.84[1]
P (cr)
red, triclinic
-17.6[1]-12.1[1]22.80[1]21.21[1]
P (cr)
black
-39.3[1]
P (am)
red
-7.5[1]
P (g)314.64[1]278.25[1]163.193[1]20.786[1]
Cu(OH)2 (cr)-449.8[1]
Cu(OH)2 (ai)-395.22[1]-249.01[1]-120.9[1]
* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (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
Cu3(PO4)2 (cr)-2051.3[1]
PH3 (g)5.4[1]13.4[1]210.23[1]37.11[1]
PH3 (ao)-9.50[1]25.36[1]120.1[1]
CuO (cr)-157.3[1]-129.7[1]42.63[1]42.30[1]
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

  1. 1