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Ch.15 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 4th EditionCh.15 - Chemical Equilibrium문제 80
15장, 문제 80

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

검증된 단계별 안내
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.
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.
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.
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.
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.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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.
추천 영상:
가이드 코스
07:32
Le Chatelier's Principle

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.
추천 영상:
가이드 코스
02:30
Endothermic & Exothermic Reactions

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.
추천 영상:
가이드 코스
01:14
Equilibrium Constant K
관련 실천
교과서 질문

At 650 K, the reaction MgCO3(s) ⇌ MgO(s) + CO2(g) has Kp = 0.026. A 10.0-L container at 650 K has 1.0 g of MgO(s) and CO2 at P = 0.0260 atm. The container is then compressed to a volume of 0.100 L. Find the mass of MgCO3 that is formed.

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교과서 질문

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

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교과서 질문

Consider the reaction: H2(g) + I2(g) ⇌ 2 HI(g) A reaction mixture at equilibrium at 175 K contains PH2 = 0.958 atm, PI2 = 0.877 atm, and PHI = 0.020 atm. A second reaction mixture, also at 175 K, contains PH2 = PI2 = 0.621 atm and PHI = 0.101 atm. Is the second reaction at equilibrium? If not, what will be the partial pressure of HI when the reaction reaches equilibrium at 175 K?

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