Methanol (CH₃OH) can be made by the reaction of CO with H₂: CO(𝑔) + 2 H₂(𝑔) ⇌ CH₃OH(𝑔) (c) To maximize the equilibrium yield of methanol, would you use a high or low pressure?

검증된 단계별 안내

Understand the concept of Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

Identify the number of moles of gas on both sides of the reaction: 1 mole of CO and 2 moles of H₂ on the left (total 3 moles) and 1 mole of CH₃OH on the right.

Recognize that increasing the pressure of a system in equilibrium favors the side of the reaction with fewer moles of gas. In this reaction, the right side with CH₃OH has fewer moles of gas compared to the left side.

Conclude that to maximize the equilibrium yield of methanol, a high pressure should be used because it will shift the equilibrium towards the formation of methanol, which has fewer moles of gas.

Consider other factors that might affect the yield, such as temperature and catalysts, but for pressure specifically, a high pressure is favorable for increasing the yield of methanol in this reaction.

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주요 개념

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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 gas reactions, increasing pressure favors the side of the reaction with fewer moles of gas, while decreasing pressure favors the side with more moles.

Mole Ratio in Reactions

In the given reaction, the mole ratio of reactants to products is crucial for understanding how pressure affects equilibrium. The reaction CO(g) + 2 H2(g) ⇌ CH3OH(g) has three moles of gas on the reactant side and one mole on the product side, indicating that increasing pressure will favor the formation of methanol.

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of concentrations of products to reactants at equilibrium. Changes in pressure can influence the concentrations of gaseous reactants and products, thereby affecting the position of equilibrium and the yield of methanol. A higher pressure shifts the equilibrium towards the side with fewer gas moles, potentially increasing K for the product.

Methanol (CH3OH) can be made by the reaction of CO with H2: CO(𝑔) + 2 H2(𝑔) ⇌ CH3OH(𝑔) (c) To maximize the equilibrium yield of methanol, would you use a high or low pressure?