Consider the endothermic reaction: C₂H₄(g) + I₂(g) ⇌ C₂H₄I₂(g) If you were trying to maximize the amount of C₂H₄I₂ produced, which tactic might you try? Assume that the reaction mixture reaches equilibrium. a. decreasing the reaction volume b. removing I₂ from the reaction mixture c. raising the reaction temperature d. adding C₂H₄ to the reaction mixture

Verified step by step guidance

1. Identify the nature of the reaction: The given reaction is endothermic, which means it absorbs heat. According to Le Chatelier's Principle, increasing the temperature will favor the endothermic reaction, shifting the equilibrium towards the products.
2. Analyze the effect of changing reaction volume: Decreasing the volume of a gaseous system increases the pressure, affecting the side of the reaction with more moles of gas. In this case, both sides of the equilibrium have the same number of moles of gas (1 mole of C2H4 and 1 mole of I2 on the reactant side, and 1 mole of C2H4I2 on the product side), so changing the volume would not significantly shift the equilibrium.
3. Consider the effect of removing a reactant: Removing I2 from the reaction mixture would shift the equilibrium to the left, according to Le Chatelier's Principle, as the system tries to counteract the change by producing more I2. This would decrease the amount of C2H4I2 produced.
4. Evaluate the impact of adding a reactant: Adding more C2H4 would increase the concentration of one of the reactants, shifting the equilibrium towards the right to produce more C2H4I2, according to Le Chatelier's Principle.
5. Choose the best tactic: Based on the analysis, the most effective tactic to maximize the amount of C2H4I2 produced would be to raise the reaction temperature, as this would favor the formation of the product in an endothermic 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 us to determine the best tactics to maximize product formation.

Endothermic Reactions

An endothermic reaction is one that absorbs heat from its surroundings. In the context of the given reaction, increasing the temperature will favor the formation of products, as the system will shift to absorb the added heat, thus promoting the production of C2H4I2.

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 temperature can affect the value of K, guiding decisions on how to manipulate the reaction conditions to favor product formation.