Methane is the simplest hydrocarbon and chemical compound. Methane is gas that’s found in small quantities in Earth’s atmosphere. It is a group-14 hydride and also the simplest alkane and is that the main constituent of gas. Discovery and isolation of methane were between 1776 and 1778 when Alessandro Volta studying marsh gas from Lake Maggiore Alessandro Volta. It is the main component of gas, about 87% by volume. In this short article, we will learn about methane formula, its properties, chemical reactions, and uses.
Chemical Methane Formula is CH4. Four hydrogen atoms bonded to a single carbon atom in methane. It is a group-14 hydride and the simplest alkane and is the main constituent of natural gas. Methane is a colourless, odourless, highly flammable gas at room temperature and can be found in a wide variety of sources on Earth. Although, methane can be found in the universe anywhere. Methane is present in interstellar space as well as solar systems beyond our own.
The abundance of methane on Earth makes it a beautiful fuel. Although capturing and storing it poses challenges to its gaseous state under normal conditions for temperature and pressure. Marsh gas, fossil fuel, carbon tetrahydride, hydrogen carbide are other names of methane. The molar mass of methane is 16.043 g·mol−1.
Properties of Methane
At temperature and standard atmosphere, methane may be a colourless, odourless gas. Methane contains a boiling point of −164 °C (−257.8 °F) at a pressure of 1 atmosphere. As a gas, it’s flammable over a variety of concentrations (5.4–17%) within the air at standard atmosphere. Solid methane exists in several modifications.
Cooling methane at normal pressure leads to the formation of methane I. This substance crystallizes within the cubic system & space group Fm3m. The positions of the hydrogen atoms aren’t fixed in methane I, i.e. methane molecules may rotate freely. Therefore, it’s a plastic crystal.
Preparation of Methane
- By the catalytic reduction of methyl iodide.
CH3-I + H2 → CH4 +HI
- By the hydrolysis of aluminum carbide. In the laboratory, methane is often prepared by boiling aluminum carbide with water.
Al4C3 + 12H2O → 3CH4 +Al (OH)3
Combustion Reaction: Methane’s heat of combustion is 55.5 MJ/kg. Combustion of methane may be a multiple-step reaction summarized as follows:
- CH4 + 2O2 → CO2 + 2H2O
Methane radical reactions where X may be a halogen: fluorine (F), chlorine (Cl), bromine (Br), or iodine (I).
- X• + CH4 → HX + CH3•
- CH3• + X2 → CH3X + X•
- CH4 + Cl2 → CH3Cl + HCl (dichloromethane)
- CH3Cl + Cl2 → CH2Cl2 +HCl (dichloromethane)
- CH2Cl2 + Cl2 → CHCl3 + HCl (chloroform)
- CHCl3 + Cl2 → CCl4 +HCl (carbon tetrachloride)
Methane is essentially utilized in domestic and industrial fuel. Moreover, it’s utilized in blacking and printer’s ink. Tire manufacturing and manufacture of methanol are other uses of methane. However, gas pipelines distribute large amounts of gas. Methane is the principal component in gas pipelines. Refined liquid methane is employed as a rocket propellant.
Solved Examples for Methane Formula
Q] How methane prepared within the laboratory?
Solution- Laboratory preparation of methane includes heating a mix of sodium acetate with the mixture . Powdered sodium acetate is mixed with fourfold the quantity of mixture. The mixture is taken during a hard glass tube. it’s fitted with the delivery tube.