Ethane is a hydrocarbon with the chemical formula C2H6. It is commonly used as a fuel and is a component of natural gas. Ethane has two carbon atoms and six hydrogen atoms.
| IUPAC Name | Ethane |
| Molecular Formula | C2H6 |
| CAS Number | 74-84-0 |
| Synonyms | Diethyl, Dimethyl, Ethylhydride, Methylmethane |
| InChI | InChI=1S/C2H6/c1-2/h1-2H3 |
Ethane Properties
Ethane Formula
The chemical formula of ethane is C2H6. It indicates that each molecule of ethane consists of two carbon atoms and six hydrogen atoms. The formula helps us understand the composition of ethane and its structural arrangement.
Ethane Molar Mass
The molar mass of ethyl hydride is calculated by adding the atomic masses of its constituent elements. Carbon has an atomic mass of 12.01 g/mol, and hydrogen has an atomic mass of 1.008 g/mol. Multiplying the atomic masses by their respective counts and summing them gives the molar mass of ethyl hydride, which is approximately 30.07 g/mol.
Ethane Boiling Point
Ethyl hydride has a boiling point of -88.6 degrees Celsius. This means that at standard atmospheric pressure, ethyl hydride will transition from a liquid to a gaseous state when heated to this temperature. The boiling point is an important property as it determines the conditions under which ethyl hydride can be vaporized.
Ethane Melting Point
The melting point of ethyl hydride is -182.8 degrees Celsius. At temperatures below this point, ethyl hydride exists as a solid. When heated to or above this temperature, ethyl hydride undergoes a phase change from a solid to a liquid state. The melting point is crucial in understanding the physical behavior of ethyl hydride during cooling or heating processes.
Ethane Density g/mL
The density of ethyl hydride is around 0.55 g/mL at standard temperature and pressure. Density is a measure of how much mass is present in a given volume. In the case of ethyl hydride, it tells us how tightly packed its molecules are and provides insights into its physical properties.
Ethane Molecular Weight
The molecular weight of ethyl hydride is 30.07 g/mol. It is the sum of the atomic masses of all the atoms in a single molecule of ethyl hydride. The molecular weight helps us determine the amount of ethyl hydride present in a given mass or volume.
Ethane Structure
The structure of ethyl hydride consists of two carbon atoms bonded together by a single covalent bond. Each carbon atom is surrounded by three hydrogen atoms. The structural arrangement is linear, with the hydrogen atoms positioned symmetrically around the carbon-carbon bond.
Ethane Solubility
Ethyl hydride is not very soluble in water. It is a nonpolar molecule, while water is a polar solvent. Nonpolar molecules like ethyl hydride have weak intermolecular forces and do not readily dissolve in polar solvents. However, ethyl hydride can dissolve in other nonpolar solvents, such as hexane or benzene.
| Appearance | Colorless gas |
| Specific Gravity | 1.038 g/L |
| Color | N/A |
| Odor | Odorless |
| Molar Mass | 30.07 g/mol |
| Density | 0.55 g/mL |
| Melting Point | -182.8 °C |
| Boiling Point | -88.6 °C |
| Flash Point | -135 °C |
| Water Solubility | Insoluble |
| Solubility | Soluble in nonpolar solvents |
| Vapour Pressure | 46.9 psi (at 21 °C) |
| Vapour Density | 1.52 (air = 1) |
| pKa | ~50 |
| pH | N/A |
Ethane Safety and Hazards
Ethyl hydride poses several safety considerations and hazards. It is highly flammable and can form explosive mixtures with air. When exposed to a flame or heat source, ethyl hydride can ignite, causing fire or explosions. It is important to handle and store ethyl hydride in well-ventilated areas away from ignition sources. Ethyl hydride is also an asphyxiation hazard, as it displaces oxygen in enclosed spaces. Inhalation of high concentrations of ethyl hydride can cause dizziness, nausea, and even loss of consciousness. It is essential to use proper personal protective equipment and follow safety protocols when working with or around ethyl hydride to mitigate these risks.
| Hazard Symbols | Flammable Gas |
| Safety Description | Keep away from heat, sparks, and open flames. Use in well-ventilated areas. Handle with proper precautions to avoid fire or explosion hazards. |
| UN IDs | UN1035 |
| HS Code | 29011000 |
| Hazard Class | 2.1 (Flammable gas) |
| Packing Group | Not Applicable |
| Toxicity | Ethane is not considered to be highly toxic. However, inhalation of high concentrations can cause asphyxiation. Use with proper ventilation and avoid prolonged exposure. |
Ethane Synthesis Methods
Various methods synthesize ethyl hydride.
One common method is the steam cracking process, where high temperatures (around 750-900 °C) heat hydrocarbons, typically ethyl hydride or heavier hydrocarbons, in the presence of steam. This process initiates reactions, including thermal decomposition and rearrangement, producing ethyl hydride, ethylene, and propylene.
Another method involves the catalytic hydrogenation of acetylene, where acetylene gas reacts with hydrogen over suitable catalysts like palladium or nickel, yielding ethyl hydride. This method selectively converts highly reactive and potentially hazardous acetylene into a more stable and less reactive ethyl hydride.
Ethane can also be obtained from natural gas through cryogenic extraction. Natural gas, primarily methyl hydride, undergoes low temperatures and high pressures to separate and recover ethyl hydride. Natural gas processing plants commonly employ this process to extract valuable ethyl hydride for various industrial applications.
Furthermore, petroleum refining and certain petrochemical processes generate ethyl hydride as a byproduct. Techniques like distillation or absorption separate ethyl hydride from other hydrocarbon streams.
Overall, these synthesis methods enable the production of ethyl hydride, a crucial feedstock for manufacturing a wide range of chemicals, plastics, and fuels, contributing to numerous industries worldwide.
Ethane Uses
Ethyl hydride finds application in various industries due to its versatile properties. Here are some key uses of ethyl hydride:
- Petrochemical Industry: Ethyl hydride is a vital feedstock for the production of ethylene, which serves as a building block for plastics, resins, and synthetic fibers. It is a key component in the manufacturing of polyethylene, one of the most widely used plastics globally.
- Fuel and Energy: Ethyl hydride plays a role in fueling and energizing specific industrial processes and is a constituent of natural gas. Industries burn ethyl hydride to generate heat or electricity, thereby serving as an energy source for residential, commercial, and industrial applications.
- Refrigeration: In certain applications, such as low-temperature systems, ethyl hydride serves as a refrigerant, offering efficient cooling capabilities. It offers efficient cooling capabilities and is an alternative to other refrigerants with higher environmental impact.
- Solvent: Ethyl hydride serves as a nonpolar solvent, particularly in laboratory settings. Ethyl hydride facilitates processes like extraction, purification, and analysis.
- Calibration Gas: Ethyl hydride serves as a component in the calibration of gas mixtures for gas detectors and analyzers, enabling the calibration and verification of gas detection equipment.
- Aerosol Propellant: Ethyl hydride functions as an aerosol propellant in various products, expelling their contents from the container upon release of pressure. It imparts the required force to spray substances such as cosmetics, paints, and household products.
- Chemical Synthesis: Ethyl hydride serves as a raw material for the synthesis of a variety of organic chemicals, including ethanol, ethylene oxide, and vinyl chloride. These chemicals find applications in the production of solvents, plastics, detergents, and PVC pipes, among others.
These diverse applications highlight the significance of ethyl hydride across multiple industries, making it a crucial component in modern manufacturing and everyday life.
Questions:
Q: Is C2H6 polar or nonpolar?
A: C2H6 (ethyl hydride) is a nonpolar molecule because the electronegativity difference between carbon and hydrogen is small, resulting in an even distribution of electron density.
Q: How many moles of carbon atoms are there in 0.500 moles of C2H6?
A: In 0.500 mole of C2H6, there is 1.00 mole of carbon atoms since each molecule of C2H6 contains 2 carbon atoms.
Q: What is the empirical formula for C2H6?
A: The empirical formula for C2H6 is CH3, representing the simplest ratio of atoms present in the molecule.
Q: What is C2H6?
A: C2H6 is the chemical formula for ethyl hydride, a hydrocarbon gas commonly used as fuel and a component of natural gas.
Q: Why doesn’t ethane (C2H6) have any structural isomers?
A: Ethyl hydride (C2H6) doesn’t have structural isomers because its carbon atoms are connected by a single bond, resulting in a linear structure with no other possible arrangements.
Q: Does C2H6 have hydrogen bonding?
A: C2H6 (ethyl hydride) does not have hydrogen bonding because it lacks hydrogen atoms bonded to highly electronegative elements like nitrogen, oxygen, or fluorine.
Q: Is C2H6 ionic or covalent?
A: C2H6 is a covalent compound as it is formed by sharing of electrons between carbon and hydrogen atoms.
Q: Is C2H6 soluble in water?
A: C2H6 is insoluble in water as it is a nonpolar molecule and does not readily dissolve in the polar solvent.
Q: Does a gaseous mixture contain CH4 and C2H6 in equimolar proportion?
A: Yes, if the gaseous mixture contains CH4 and C2H6 in equimolar proportion, it means that the number of moles of CH4 is equal to the number of moles of C2H6 in the mixture.