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2Cu + Co3O4 + 3H2O 🔥→ Cu2O + 3Co(OH)2

2Cu + Co₃O₄ + 3H₂O 🔥→ Cu₂O + 3Co(OH)₂

Last updated: June 13, 2022

Reaction of copper and cobalt(II,III) oxide under neutral condition: 2CuCopper + Co₃O₄Cobalt(II,III) oxide + 3H₂OWater
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Cu₂OCopper(I) oxide + 3Co(OH)₂Cobalt(II) hydroxide

The reaction of copper, cobalt(II,III) oxide, and water yields copper(I) oxide and cobalt(II) hydroxide (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of oxidizable species and oxidizing species under neutral condition

Table of contents

Reaction data

Chemical equation

Reaction of copper and cobalt(II,III) oxide under neutral condition: 2CuCopper + Co₃O₄Cobalt(II,III) oxide + 3H₂OWater
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Cu₂OCopper(I) oxide + 3Co(OH)₂Cobalt(II) hydroxide

General equation

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

Oxidation state of each atom

Reaction of copper and cobalt(II,III) oxide under neutral condition

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
Cu	Copper	2	Reducing	Oxidizable
Co₃O₄	Cobalt(II,III) oxide	1	Oxidizing	Oxidizing
H₂O	Water	3	–	Water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Cu₂O	Copper(I) oxide	1	Oxidized	–
Co(OH)₂	Cobalt(II) hydroxide	3	Reduced	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of copper and cobalt(II,III) oxide under neutral condition ◆ Δ_rG −11 kJ/mol K 8.46 × 10¹ pK −1.93: 2CuCrystalline solid + Co₃O₄Crystalline solid + 3H₂OLiquid
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Cu₂OCrystalline solid + 3Co(OH)₂Crystalline solidblue, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−11	–	–
per 1 mol of Copper	–	−5.5	–	–
per 1 mol of Cobalt(II,III) oxide	–	−11	–	–
per 1 mol of Water	–	−3.7	–	–
per 1 mol of Copper(I) oxide	–	−11	–	–
per 1 mol of Cobalt(II) hydroxide	–	−3.7	–	–

Changes in standard condition (2)

Reaction of copper and cobalt(II,III) oxide under neutral condition ◆ Δ_rG −24 kJ/mol K 1.60 × 10⁴ pK −4.20: 2CuCrystalline solid + Co₃O₄Crystalline solid + 3H₂OLiquid
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Cu₂OCrystalline solid + 3Co(OH)₂Crystalline solidpink, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−39	−24	−48	–
per 1 mol of Copper	−20	−12	−24	–
per 1 mol of Cobalt(II,III) oxide	−39	−24	−48	–
per 1 mol of Water	−13	−8.0	−16	–
per 1 mol of Copper(I) oxide	−39	−24	−48	–
per 1 mol of Cobalt(II) hydroxide	−13	−8.0	−16	–

Changes in standard condition (3)

Reaction of copper and cobalt(II,III) oxide under neutral condition ◆ Δ_rG −35 kJ/mol K 1.35 × 10⁶ pK −6.13: 2CuCrystalline solid + Co₃O₄Crystalline solid + 3H₂OLiquid
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Cu₂OCrystalline solid + 3Co(OH)₂Crystalline solidpink, precipitated, aged

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−35	–	–
per 1 mol of Copper	–	−18	–	–
per 1 mol of Cobalt(II,III) oxide	–	−35	–	–
per 1 mol of Water	–	−12	–	–
per 1 mol of Copper(I) oxide	–	−35	–	–
per 1 mol of Cobalt(II) hydroxide	–	−12	–	–

Changes in aqueous solution (1)

Reaction of copper and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 74 kJ/mol K 0.11 × 10⁻¹² pK 12.96: 2CuCrystalline solid + Co₃O₄Crystalline solid + 3H₂OLiquid
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Cu₂OCrystalline solid + 3Co(OH)₂Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	74	–	–
per 1 mol of Copper	–	37	–	–
per 1 mol of Cobalt(II,III) oxide	–	74	–	–
per 1 mol of Water	–	25	–	–
per 1 mol of Copper(I) oxide	–	74	–	–
per 1 mol of Cobalt(II) hydroxide	–	25	–	–

Changes in aqueous solution (2)

Reaction of copper and cobalt(II,III) oxide under neutral condition ◆ Δ_rG −11 kJ/mol K 8.46 × 10¹ pK −1.93: 2CuCrystalline solid + Co₃O₄Crystalline solid + 3H₂OLiquid
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Cu₂OCrystalline solid + 3Co(OH)₂Crystalline solidblue, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−11	–	–
per 1 mol of Copper	–	−5.5	–	–
per 1 mol of Cobalt(II,III) oxide	–	−11	–	–
per 1 mol of Water	–	−3.7	–	–
per 1 mol of Copper(I) oxide	–	−11	–	–
per 1 mol of Cobalt(II) hydroxide	–	−3.7	–	–

Changes in aqueous solution (3)

Reaction of copper and cobalt(II,III) oxide under neutral condition ◆ Δ_rG −24 kJ/mol K 1.60 × 10⁴ pK −4.20: 2CuCrystalline solid + Co₃O₄Crystalline solid + 3H₂OLiquid
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Cu₂OCrystalline solid + 3Co(OH)₂Crystalline solidpink, precipitated

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−39	−24	−48	–
per 1 mol of Copper	−20	−12	−24	–
per 1 mol of Cobalt(II,III) oxide	−39	−24	−48	–
per 1 mol of Water	−13	−8.0	−16	–
per 1 mol of Copper(I) oxide	−39	−24	−48	–
per 1 mol of Cobalt(II) hydroxide	−13	−8.0	−16	–

Changes in aqueous solution (4)

Reaction of copper and cobalt(II,III) oxide under neutral condition ◆ Δ_rG −35 kJ/mol K 1.35 × 10⁶ pK −6.13: 2CuCrystalline solid + Co₃O₄Crystalline solid + 3H₂OLiquid
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Cu₂OCrystalline solid + 3Co(OH)₂Crystalline solidpink, precipitated, aged

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−35	–	–
per 1 mol of Copper	–	−18	–	–
per 1 mol of Cobalt(II,III) oxide	–	−35	–	–
per 1 mol of Water	–	−12	–	–
per 1 mol of Copper(I) oxide	–	−35	–	–
per 1 mol of Cobalt(II) hydroxide	–	−12	–	–

Thermodynamic data of reactants

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° 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]
Co₃O₄ (cr)	-891^[1]	-774^[1]	102.5^[1]	123.4^[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, (l):Liquid

Thermodynamic data of products

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
Cu₂O (cr)	-168.6^[1]	-146.0^[1]	93.14^[1]	63.64^[1]
Co(OH)₂ (cr) blue, precipitated	–	-450.1^[1]	–	–
Co(OH)₂ (cr) pink, precipitated	-539.7^[1]	-454.3^[1]	79^[1]	–
Co(OH)₂ (cr) pink, precipitated, aged	–	-458.1^[1]	–	–
Co(OH)₂ (ai)	-518.0^[1]	-369.0^[1]	-134^[1]	–
Co(OH)₂ (ao)	–	-421.7^[1]	–	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

References

List of references

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
https://doi.org/10.18434/M32124
National Institute of Standards and Technology (NIST)
Citation list

Δ_rG	−11 kJ/mol
K	8.46 × 10¹
pK	−1.93

Δ_rG	−24 kJ/mol
K	1.60 × 10⁴
pK	−4.20

Δ_rG	−35 kJ/mol
K	1.35 × 10⁶
pK	−6.13

Δ_rG	74 kJ/mol
K	0.11 × 10⁻¹²
pK	12.96

2Cu + Co3O4 + 3H2O 🔥→ Cu2O + 3Co(OH)2

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Products

Thermodynamic changes

Changes in standard condition (1)

Changes in standard condition (2)

Changes in standard condition (3)

Changes in aqueous solution (1)

Changes in aqueous solution (2)

Changes in aqueous solution (3)

Changes in aqueous solution (4)

Thermodynamic data of reactants

Thermodynamic data of products

References

List of references

Related reactions

Reactions with same reactants

Related categories

Type of reaction

General equation

Reactant

Product

2Cu + Co₃O₄ + 3H₂O 🔥→ Cu₂O + 3Co(OH)₂