What is Ethane Definition Molecular Formula Structure and Chemical Reactions
Ethane is essential in chemistry and helps students understand various practical and theoretical applications related to this topic. This simple hydrocarbon is the foundation for learning about alkanes, bonding, and how natural gas fuels modern life. Let's explore everything about ethane below!
What is Ethane in Chemistry?
A hydrocarbon, ethane is an alkane with the formula C2H6. It consists of two carbon atoms and six hydrogen atoms joined by single bonds. This concept appears in chapters related to alkane structure, hydrocarbons, and organic compounds, making it a foundational part of your chemistry syllabus.
Molecular Formula and Composition
The molecular formula of ethane is C2H6. It consists of a single carbon–carbon bond, with three hydrogen atoms attached to each carbon. Ethane belongs to the alkane family, which are all saturated hydrocarbons containing only single bonds.
Preparation and Synthesis Methods
Industrially, ethane is separated from natural gas using a process called cryogenic distillation. In the laboratory, ethane can be prepared by the Wurtz reaction, where ethyl halides are reacted with sodium metal in dry ether:
C2H5Br + 2Na + BrC2H5 → C2H6 + 2NaBr
Another method involves the hydrogenation of ethylene (ethene) using a catalyst.
Physical Properties of Ethane
Ethane is a colorless, odorless, and flammable gas at room temperature. Here is a compact summary of its main physical properties:
| Property | Value |
|---|---|
| Chemical Formula | C2H6 |
| Molar Mass | 30.07 g/mol |
| Boiling Point | -88.5 °C |
| Melting Point | -182.8 °C |
| Solubility | Very slightly soluble in water |
| State at Room Temperature | Gas |
Chemical Properties and Reactions
Ethane is a stable alkane, so it is not very reactive. However, it undergoes certain important reactions:
1. Combustion: Burns in oxygen to form carbon dioxide and water.
C2H6 + 3.5 O2 → 2CO2 + 3H2O
2. Halogenation: Reacts with chlorine or bromine under UV light to produce haloalkanes.
3. Cracking: Can be thermally cracked to form ethylene (ethylene is vital for manufacturing plastics).
Frequent Related Errors
- Confusing ethane with ethene (C2H4), which is an alkene with a double bond.
- Assuming ethane is an unsaturated hydrocarbon (it is saturated and contains only single bonds).
- Mistaking ethane for being toxic or poisonous (at normal exposure levels, it is not toxic).
- Incorrectly drawing the Lewis structure (forgetting the complete eight electrons on both carbons).
Uses of Ethane in Real Life
Ethane is widely used in the petrochemical industry. Key uses include:
- As a feedstock for producing ethylene (used to make plastics like polyethylene).
- Limited use as a fuel, mostly where natural gas is processed.
- Used in laboratories and refrigeration systems in liquid form.
- Helps make acetic acid, ethanol, and other chemicals via chemical conversion.
Relation with Other Chemistry Concepts
Ethane connects with several important chemistry topics. For example, its simple bonding and structure are the basis for learning about alkanes and organic compounds.
The way ethane burns links to combustion reactions and energy cycles. Compared to methane and ethene, it helps students see differences between saturated and unsaturated hydrocarbons.
Step-by-Step Reaction Example
1. Combustion of ethane:C2H6 + O2 → CO2 + H2O
2. Balance carbon first:
C2H6 + O2 → 2CO2 + H2O
3. Balance hydrogen next (6 H = 3 H2O):
C2H6 + O2 → 2CO2 + 3H2O
4. Balance oxygen (2x2 = 4, 3x1 = 3; total 7 O on right):
Use 3.5 O2 on left.
5. Final Balanced Equation:
C2H6 + 3.5 O2 → 2CO2 + 3H2O
Lab or Experimental Tips
Remember ethane as the "two-carbon, single-bond" alkane! A simple way to draw ethane is to write two “CH3” groups connected by a single line (CH3–CH3). Vedantu educators often use this tip in live sessions to help students quickly visualize ethane's structure for exam diagrams.
Try This Yourself
- Write the IUPAC name of C2H6.
- Draw the full Lewis structure for ethane with all bonds shown.
- Compare ethane and ethene—what is the main difference in bonding?
- List two uses of ethane in the petrochemical industry.
Final Wrap-Up
We explored ethane—its structure, properties, reactions, and real-life importance. Understanding ethane forms the base for concepts like alkanes, hydrocarbons, and chemical reactions. For more in-depth explanations and exam-prep tips, explore live classes and notes on Vedantu.
Related Reading: Alkanes, Hydrocarbons, Organic Compounds, Methane
FAQs on Ethane in Organic Chemistry Structure Properties and Reactions
1. What is ethane in chemistry?
Ethane is a saturated hydrocarbon with the molecular formula C2H6 and is the second member of the alkane series. It consists of two carbon atoms joined by a single covalent bond, each carbon bonded to three hydrogen atoms.
- Belongs to the alkanes (general formula: CnH2n+2).
- Contains only single C–C and C–H bonds.
- Is a colorless, odorless gas at room temperature.
2. What is the structural formula of ethane?
The structural formula of ethane is CH3–CH3, showing two carbon atoms joined by a single bond. Each carbon atom forms four single covalent bonds:
- One C–C bond between the two carbons.
- Three C–H bonds on each carbon.
3. What is the molecular formula of ethane?
The molecular formula of ethane is C2H6. It follows the general alkane formula CnH2n+2, where n = 2.
- Number of carbon atoms (n) = 2
- Hydrogen atoms = 2(2) + 2 = 6
4. How is ethane prepared in the laboratory?
Ethane can be prepared in the laboratory by the Wurtz reaction using methyl halide and sodium in dry ether. The balanced reaction is:
2CH3Cl + 2Na → C2H6 + 2NaCl
- Methyl chloride reacts with sodium metal.
- Dry ether is used as a solvent.
- Two methyl groups combine to form ethane.
5. What happens when ethane undergoes combustion?
When ethane undergoes complete combustion, it reacts with oxygen to form carbon dioxide and water. The balanced equation is:
2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l)
- This is an exothermic reaction.
- It releases a large amount of heat energy.
- Incomplete combustion can produce carbon monoxide (CO).
6. What type of hybridization is present in ethane?
Each carbon atom in ethane exhibits sp3 hybridization. In ethane:
- One sp3 orbital forms the C–C sigma bond.
- Three sp3 orbitals form C–H sigma bonds.
- The bond angle is approximately 109.5°.
7. What are the physical properties of ethane?
Ethane is a colorless, odorless, and highly flammable gas at room temperature. Its key physical properties include:
- Molecular formula: C2H6
- Boiling point: approximately −88.6°C
- Slightly soluble in water
- Non-polar molecule
8. What is the difference between ethane and ethene?
The main difference between ethane and ethene is that ethane is a saturated alkane while ethene is an unsaturated alkene.
- Ethane: C2H6, single C–C bond, sp3 hybridization.
- Ethene: C2H4, double C=C bond, sp2 hybridization.
- Ethene undergoes addition reactions, while ethane mainly undergoes substitution reactions.
9. What are the main uses of ethane?
Ethane is primarily used as a raw material in the production of ethene (ethylene) in the petrochemical industry. Its major uses include:
- Cracking to produce ethene (C2H4)
- Fuel source in some industrial processes
- Component of natural gas
10. What type of reactions does ethane undergo?
Ethane mainly undergoes substitution reactions and combustion reactions because it is a saturated alkane. A common example is halogenation:
C2H6 + Cl2 → C2H5Cl + HCl (in the presence of UV light).
- Occurs via a free radical mechanism.
- One hydrogen atom is replaced by a halogen.
- Also undergoes complete combustion with oxygen.
