Categories: Lesson Notes

SS2 Chemistry Lesson Note on Methane

The website has the complete lesson note for all the subjects in secondary school but this piece showcases the SS2 Chemistry Lesson Note on Methane. You can use the website search button to filter out the subject of interest to you.

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METHANE

Occurrence: Methane is the major constituent of natural gas, petroleum gas and, is usually known as Marsh gas. It is also found in poorly ventilated coal mines as fire dump.

LABORATORY PREPARATION

Procedure: A finely powdered mixture of equal amount of anhydrous sodium ethanoate and soda lime is heated in a hard glass test tube. The methane evolved is collected over water.

Equation of reaction is shown below:

CH3COONa(s)   +   NaOH(s)    →   Na2CO3(s) +   CH4 (g)

To prepared other members, the same method is applied. For example, the preparation of ethane required heating sodium propanoate according to the equation below:

CH3CH2COONa  →   Na2CO3  +  C2H6                                          

PROPERTIES OF ALKANES

PHYSICAL PROPERTIES

  1. The first members (i.e. C1 –C4) are colourless gases. From (C5 –C17) are colourless liquids. Higher members greater than C17 are colourless, wax like solids.
  2. They are insoluble in water
  3. Branched alkanes have lower boiling and melting points than their corresponding straight chain alkanes. Branching makes the molecules spherical and therefore reduces the intermolecular forces between the molecules. For example, the boiling point of 2-methylpropane is lower than that of the straight chain isomer butane.

 CHEMICAL PROPERTIES

Alkanes are generally inert but they can undergo two types of reactions: combustion and substitution reactions

  1. Combustion reaction. Alkanes burn in air (or oxygen) to form CO2 and H2O (steam). The reaction is exothermic e.g

Combustion of Methane, CH4

CH4(g) + 2O2(g)  →  2H2O(g) +CO2(g)

  1. Substitution reaction.: Alkanes undergo substitution reaction with halogens. The reaction of methane with chlorine takes place in the presence of ultra-violet light which serves as catalyst. The continues until all hydrogen atoms in methane are replaced with chlorine

CH4(g) + Cl2(g)  →  CH3Cl(g) + HCl(g)

CH3Cl + Cl2    CH2Cl2 + HCl

CH2Cl2  + Cl2  → CHCl3  + HCl

CHCl3 + Cl2 → CCl4 + HCl

Uses of methane

  1. It is mainly used fuel
  2. It is used to make carbon black, carbon (iv) sulphide, trichloromethane or tetrachloromethane.

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