Consider the hypothetical reaction A(π) β 2 B(π). A flask is charged with 0.75 atm of pure A, after which it is allowed to reach equilibrium at 0Β°C. At equilibrium, the partial pressure of A is 0.36 atm. (c) To maximize the yield of product B, would you make the reaction flask larger or smaller?
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insert step 1> Identify the reaction: A(g) β 2 B(g). This is a gaseous equilibrium reaction where A is converted to B.
insert step 2> Understand the concept of Le Chatelier's Principle: It states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
insert step 3> Consider the effect of volume change on equilibrium: Increasing the volume of the container decreases the pressure, favoring the side with more moles of gas. Conversely, decreasing the volume increases the pressure, favoring the side with fewer moles of gas.
insert step 4> Analyze the reaction: The reaction A(g) β 2 B(g) has 1 mole of A converting to 2 moles of B. Increasing the volume will favor the formation of more moles of gas, thus shifting the equilibrium towards the products (B).
insert step 5> Conclusion: To maximize the yield of product B, you should make the reaction flask larger, as this will shift the equilibrium towards the side with more moles of gas (2 B).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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. In the context of the reaction A(g) β 2B(g), if the volume of the flask is altered, it affects the partial pressures of the gases, thereby influencing the equilibrium position and the yield of products.
The equilibrium constant (Kp) for a gaseous reaction is defined in terms of the partial pressures of the reactants and products at equilibrium. For the reaction A(g) β 2B(g), Kp can be expressed as Kp = (P_B^2) / (P_A). Understanding Kp helps predict how changes in pressure or volume will affect the concentrations of A and B at equilibrium.
Changing the volume of a reaction flask affects the partial pressures of gases involved in the reaction. Reducing the volume increases the pressure, favoring the side of the reaction with fewer moles of gas. In this case, since there are 2 moles of B produced for every mole of A consumed, decreasing the volume would shift the equilibrium towards producing more B, thus maximizing its yield.
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