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Laboratory experiment 2. Oxidation of ethanol by copper(II) oxide

Lecture



Oxidation of ethanol by copper(II) oxide

Heat a copper wire in the flame of a spirit lamp until it glows red. The surface of the copper becomes coated with a black layer as a result of oxidation to copper(II) oxide, which is black. Then quickly dip the glowing wire into a test tube of ethanol. The black coating disappears and the surface of the copper wire becomes shiny again. If the experiment is repeated several times, an apple-like smell characteristic of acetaldehyde can be detected.

Explain the observed phenomena, and write the equations for the reactions taking place.

Purpose of the experiment:

Demonstrate the oxidation reaction of ethanol by CuO, producing an aldehyde (acetaldehyde) and reducing copper(II) oxide to metallic copper.

Laboratory experiment 2. Oxidation of ethanol by copper(II) oxide

Equipment and reagents:

  • Test tube

  • Spirit lamp

  • Test tube holder

  • Ethanol (C₂H₅OH)

  • Copper(II) oxide (CuO) — black powder

  • Water

  • Pipette

Procedure:

  1. Pour a small amount of copper(II) oxide (black powder) into a test tube.

  2. Add a few drops of ethanol.

  3. Carefully heat the test tube over the spirit lamp, holding it tilted.

  4. Observe the changes:

    • the color of the copper oxide changes from black to red (metallic copper is formed),

    • a characteristic smell of acetaldehyde (a sharp, irritating odor) can be detected.

Chemical equation of the reaction:

C2H5OH+CuO→t∘CH3CHO+Cu+H2O u+H2​O

Conclusion:

During the experiment, ethanol was oxidized to acetaldehyde, and CuO was reduced to copper. The reaction confirms that ethanol has reducing properties.

created: 2025-04-14
updated: 2026-03-10
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Lectures and tutorial on "organic-chemistry"

Terms: organic-chemistry

1. Structure of the Atom. State of the Electron in the Atom. Atomic Orbital
1.2. Structure of the Electron Shells of Atoms
3. Types of Chemical Bonds - Metallic, Covalent, and Ionic
1.4. Covalent bond
1.5. The Subject of Organic Chemistry. The Theory of Structure of Organic Compounds
2.6. Structural Formulas of the Simplest Hydrocarbons. Alkanes. Isomerism of Alkanes
2.7. Spatial Structure of Alkane Molecules. sp3-Hybridization
Laboratory Experiment 1. Making Ball-and-Stick Models of Hydrocarbon Molecules
2.8. The Homologous Series and Physical Properties of Alkanes
8-1. Avogadro's Law. Relative Density of Gases. Volume Fraction of Gas in a Mixture
9. Nomenclature of Alkanes
10. Chemical properties, preparation, and applications of alkanes
11. Determining the Formula of an Organic Substance
11-1. Cycloalkanes
12. Alkenes. Structure of Molecules
13. Alkenes. Structural Isomerism and Nomenclature
14. Spatial Isomerism of Alkenes
15. Physical and Chemical Properties of Alkenes
15-1. Addition of Hydrogen Halides and Water to Alkenes. Markovnikov's Rule
16. Preparation and Uses of Alkenes
Practical Work 1. Preparation of Ethylene and Study of Its Properties
17. Alkadienes
18. Alkynes
19. Aromatic hydrocarbons. Benzene, structure of the molecule
20. Chemical properties, production, and uses of benzene
21. Natural sources of hydrocarbons and their use
22. Saturated monohydric alcohols. Isomerism, nomenclature, classification
23. Physical properties of alcohols. Hydrogen bonding and its effect on the properties of alcohols
24. Chemical properties, preparation, and uses of alcohols
Laboratory experiment 2. Oxidation of ethanol by copper(II) oxide
25. Polyhydric alcohols
Laboratory experiment 3. Reaction of glycerol with copper(II) hydroxide
26. Relationship Between Hydrocarbons and Alcohols
27. Phenols
28. Chemical Properties, Preparation, and Uses of Phenol
29. Aldehydes. Nomenclature. Isomerism. Physical Properties
30. Chemical Properties, Preparation, and Uses of Aldehydes
Laboratory Experiment 4. Oxidation of an Aldehyde with Copper(II) Hydroxide
31. Carboxylic Acids. Classification
32. Saturated Monobasic Carboxylic Acids. Nomenclature. Isomerism. Physical Properties
33. Chemical Properties of Saturated Monobasic Carboxylic Acids
Practical Work 2. Comparison of the Properties of Carboxylic and Inorganic Acids
34. Preparation and Uses of Saturated Monobasic Carboxylic Acids
35. Unsaturated Monobasic Carboxylic Acids
36. Calculations Based on Equations of Reactions Occurring in Solutions
37. Interrelationship Between Hydrocarbons, Alcohols, Aldehydes, and Carboxylic Acids
38. Esters
39. Fats. Structure. Physical and Chemical Properties
Laboratory Experiment 5. Investigation of the Properties of Fats
*Laboratory Experiment 5. Comparison of the Properties of Soap and Synthetic Detergents
40. Carbohydrates. Glucose
41. Chemical Properties of Glucose
Laboratory Experiment 6. Reaction of Glucose with Copper(II) Hydroxide
42. Fructose. Sucrose
42-1. Ribose. Deoxyribose
3.43 Starch: Composition and Structure, Chemical Properties of Starch, Uses and Production
*Practical Work 3. Hydrolysis of Starch
Laboratory Experiment 7. Study of the Physical Properties of Starch.
3.44. Cellulose: Structure, Physical and Chemical Properties, Applications
Practical Work 3. Solving Experimental Problems
CHAPTER 4. NITROGEN-CONTAINING ORGANIC COMPOUNDS § 45. Structure and Physical Properties of Amines
4.46 Chemical properties, preparation, and uses of amines
4.47. Amino Acids. Nomenclature, Physical and Chemical Properties, Preparation and Uses
4.48 Proteins. Properties of Proteins
Laboratory Experiment 8. Properties of Proteins: Denaturation, Color Reactions
Practical Work 4. Solving Experimental Problems
Polymers and Copolymers as Substances: Their Properties and Applications
*Practical Work 4. Properties of High-Molecular-Weight Compounds
Conclusion