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Ch.15 - Chemical Equilibrium
McMurry - Chemistry 8th Edition
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모든 교과서McMurry 8th EditionCh.15 - Chemical Equilibrium문제 12
15장, 문제 12

Suppose that the following endothermic reaction is at equilibrium: 2 CO(g) + O2(g) ⇌ 2 CO2(g). Which of the following changes would cause the reaction to shift toward products? (LO 15.12 – 15.15) (a) Remove CO(g). (b) Increase the temperature. (c) Add a catalyst. (d) Increase the volume of the container.

검증된 단계별 안내
1
Step 1: Understand Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change and re-establish equilibrium.
Step 2: Analyze the effect of removing CO(g). According to Le Chatelier's Principle, removing a reactant will shift the equilibrium towards the reactants to replace the removed substance, not towards the products.
Step 3: Consider the effect of increasing the temperature. Since the reaction is endothermic, increasing the temperature will shift the equilibrium towards the products to absorb the added heat.
Step 4: Evaluate the impact of adding a catalyst. A catalyst speeds up the rate of both the forward and reverse reactions equally, so it does not shift the position of equilibrium.
Step 5: Assess the effect of increasing the volume of the container. Increasing the volume decreases the pressure, and the equilibrium will shift towards the side with more moles of gas. In this reaction, the reactants have more moles of gas (3 moles) compared to the products (2 moles), so the equilibrium will shift towards the reactants.

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 direction in which the reaction will shift.
추천 영상:
가이드 코스
07:32
Le Chatelier's Principle

Endothermic Reactions

Endothermic reactions absorb heat from their surroundings, resulting in a decrease in temperature of the environment. In the context of equilibrium, increasing the temperature of an endothermic reaction will favor the formation of products, as the system shifts to absorb the added heat, thus promoting the forward reaction.
추천 영상:
가이드 코스
02:30
Endothermic & Exothermic Reactions

Effect of Volume on Gaseous Equilibria

Changing the volume of a container affects the pressure of gaseous reactants and products. According to the ideal gas law, decreasing the volume increases pressure, which shifts the equilibrium toward the side with fewer moles of gas. Conversely, increasing the volume decreases pressure and shifts the equilibrium toward the side with more moles of gas, influencing the direction of the reaction.
추천 영상:
가이드 코스
02:31
Photoelectric Effect
관련 실천
교과서 질문

Calculate the value of the equilibrium constant at 427 °C for the reaction

Na O1s2 + 1>2 O 1g2 ∆ Na O 1s2

given the following equilibrium constants at 427 °C.

Na2O1s2 ∆ 2 Na1l2 + 1>2 O21g2 Kc = 2 * 10-25 Na O 1s2 ∆ 2 Na1l2 + O 1g2 K = 5 * 10-29

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교과서 질문

Calculate the value of the equilibrium constant for the reaction 4 NH31g2 + 3 O21g2 ∆ 2 N21g2 + 6 H2O1g2

given the following equilibrium constants at a certain temperature.

2 H21g2 + O21g2 ∆ 2 H2O1g2 Kc = 3.2 * 1081

N21g2 + 3 H21g2 ∆ 2 NH31g2 Kc = 3.5 * 108

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교과서 질문
For the general, single-step reaction A1g2 + B1g2 ∆ AB1g2, Kc = 4.5 * 10-6, which of the following statements is true? (LO 15.16) (a) Ea 1forward2 6 Ea 1reverse2 (b) The equilibrium mixture contains mostly products. (c) kr 7 kf (d) The reaction is exothermic.
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