Consider the exothermic reaction: C₂H₄(g) + Cl₂(g) ⇌ C₂H₄Cl₂(g) If you were trying to maximize the amount of C₂H₄Cl₂ produced, which tactic might you try? Assume that the reaction mixture reaches equilibrium. a. increasing the reaction volume b. removing C₂H₄Cl₂ from the reaction mixture as it forms c. lowering the reaction temperature d. adding Cl₂

Verified step by step guidance

1. Identify the nature of the reaction: The given reaction is exothermic, meaning it releases heat. Therefore, changes in temperature can affect the equilibrium position.
2. Apply Le Chatelier's Principle: This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. In the context of an exothermic reaction, lowering the temperature shifts the equilibrium towards the products.
3. Consider the effect of lowering the temperature: Since the reaction is exothermic, reducing the temperature favors the formation of more products (C2H4Cl2) because the system seeks to produce more heat to counterbalance the temperature decrease.
4. Evaluate other options: Increasing the reaction volume generally shifts the equilibrium towards the side with more moles of gas. In this case, the number of moles of reactants and products are the same, so this change would not be effective. Removing C2H4Cl2 as it forms would indeed shift the equilibrium towards more product formation to replace what is removed. Adding more Cl2 would also shift the equilibrium towards more product formation by increasing the concentration of one of the reactants.
5. Choose the best tactic: Based on Le Chatelier's Principle and the nature of the reaction, lowering the reaction temperature (option c) is a strategic way to maximize the production of C2H4Cl2 in an exothermic reaction.

Key Concepts

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. This principle helps predict how a system at equilibrium will respond to changes in concentration, temperature, or pressure, allowing for strategies to maximize product formation.

Exothermic Reactions

Exothermic reactions release heat as they proceed, resulting in a decrease in the system's internal energy. For exothermic reactions, lowering the temperature generally favors the formation of products, as the system shifts to produce more heat to counteract the temperature change, thus increasing the yield of products like C2H4Cl2.

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. Changes in concentration or pressure can shift the equilibrium position, affecting the amounts of reactants and products present, which is crucial for determining the best tactic to maximize C2H4Cl2 production.