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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 81
15장, 문제 81

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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1
Identify the equilibrium constant expression for the reaction: \( K_p = \frac{{(P_{\text{HI}})^2}}{{P_{\text{H}_2} \cdot P_{\text{I}_2}}} \).
Calculate the equilibrium constant \( K_p \) using the first reaction mixture: substitute \( P_{\text{H}_2} = 0.958 \) atm, \( P_{\text{I}_2} = 0.877 \) atm, and \( P_{\text{HI}} = 0.020 \) atm into the expression.
Determine the reaction quotient \( Q_p \) for the second reaction mixture using the same expression: substitute \( P_{\text{H}_2} = 0.621 \) atm, \( P_{\text{I}_2} = 0.621 \) atm, and \( P_{\text{HI}} = 0.101 \) atm.
Compare \( Q_p \) with \( K_p \): if \( Q_p = K_p \), the system is at equilibrium; if \( Q_p \neq K_p \), the system is not at equilibrium.
If the system is not at equilibrium, determine the direction of the shift: if \( Q_p < K_p \), the reaction will shift to the right (towards products), and calculate the change in \( P_{\text{HI}} \) needed to reach equilibrium.

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주요 개념

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Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In this state, the system appears static, but molecular activity continues. The equilibrium constant (K) quantifies the ratio of product concentrations to reactant concentrations at equilibrium, providing insight into the position of equilibrium.
추천 영상:
가이드 코스
04:21
Chemical Equilibrium Concepts

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. This principle helps predict how changes in concentration, pressure, or temperature will affect the position of equilibrium in a chemical reaction.
추천 영상:
가이드 코스
07:32
Le Chatelier's Principle

Partial Pressure and the Ideal Gas Law

Partial pressure refers to the pressure exerted by an individual gas in a mixture, which can be calculated using Dalton's Law of Partial Pressures. The Ideal Gas Law (PV=nRT) relates the pressure, volume, and temperature of a gas, allowing for the determination of the behavior of gases under various conditions. Understanding these concepts is crucial for calculating equilibrium concentrations in gas-phase reactions.
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가이드 코스
00:44
Law of Partial Pressures
관련 실천
교과서 질문

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

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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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