Final answer:
The question deals with the chemical reactions between chlorine gas and alkanes to produce haloalkanes, commonly occurring through a free radical substitution mechanism. Such reactions are utilized in industrial settings to create more reactive organic compounds that can participate in various polar reactions. The concentration and conditions are carefully managed for these reactions to ensure the desired haloalkanes are the major products.
Step-by-step explanation:
The question concerns the chemical reaction between chlorine gas (Cl₂) and various alkanes to produce haloalkanes. The halogenation of methane with chlorine gas, for example, can produce a range of products such as chloromethane (CH₃Cl), dichloromethane (CH₂Cl₂), trichloromethane (CHCl₃), and carbon tetrachloride (CCl₄). To generate the major product, multiple chlorine molecules are required as the reaction proceeds through a free radical substitution mechanism. This reaction is exothermic, where heat and light can catalyze the reaction to start the chain process.
In an industrial setting, the concentration of the initial alkane is kept high to minimize the formation of side products. This promotes the generation of haloalkanes, which are more reactive due to the polar C-Cl bond. These haloalkanes are valuable in organic synthesis because they undergo various polar reactions. Additionally, factors like increasing pressure or adding more chlorine can shift the equilibrium to favor the production of haloalkanes, as per Le Chatelier's principle.
Chemical equilibrium reactions such as PC₁₅(g) ⇒ PC₁₃(g) + Cl₂(g) and their corresponding ICE (Initial, Change, Equilibrium) tables are also relevant to understand the dynamics of these reactions and predict the concentration of products and reactants over time.