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1. Which of the following is true for a system whose equilibrium constant is relatively small? a) It will take a short time to reach equilibrium. b) It will take a long time to reach equilibrium. c) The equilibrium lies to the left (favors reactants). d) The equilibrium lies to the right (favors products). e) Two of these are true.

1. Which of the following is true for a system whose equilibrium constant is relatively small? a) It will take a short time to reach equilibrium. b) It will take a long time to reach equilibrium. c) The equilibrium lies to the left (favors reactants). d) The equilibrium lies to the right (favors products). e) Two of these are true.

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter16: Acids And Bases
Section: Chapter Questions
Problem 65AP: . The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in...
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is esc You may use your notes and textbook, but no other resources. Show all your work and circle the final answer. Use your acid/base resource sheet for any K values that are not provided here. (2 JEGYZ bubb 1. Which of the following is true for a system whose equilibrium constant is relatively small? a) It will take a short time to reach equilibrium. b) It will take a long time to reach equilibrium. c) The equilibrium lies to the left (favors reactants). d) The equilibrium lies to the right (favors products). e) Two of these are true. 2. sample of ammonia gas was allowed to come to equilibrium at 400 K. The decomposition is endothermic. 2NH3(g) → N₂(g) + 3H₂(g) At equilibrium, it was found that the concentration of H₂ was 0.0584 M, the concentration of N₂ was 0.0195 M, and the concentration of NH3 was 0.430 M. What was the initial concentration of ammonia? b. What is the equilibrium constant at this temperature (K.)? C. A reaction mixture that is not at equilibrium contains 0.15 M H2, 0.25 M N2, and 3 M NH3. In order to reach equilibrium, will this reaction shift in the direction of reactants or products? Explain why. g of a nagy d. How would the system respond if the volume of the reaction vessel is increased? e. If the temperature of the reaction mixture is increased, how will this affect the amount of ammonia present at equilibrium?
Transcribed Image Text:is esc You may use your notes and textbook, but no other resources. Show all your work and circle the final answer. Use your acid/base resource sheet for any K values that are not provided here. (2 JEGYZ bubb 1. Which of the following is true for a system whose equilibrium constant is relatively small? a) It will take a short time to reach equilibrium. b) It will take a long time to reach equilibrium. c) The equilibrium lies to the left (favors reactants). d) The equilibrium lies to the right (favors products). e) Two of these are true. 2. sample of ammonia gas was allowed to come to equilibrium at 400 K. The decomposition is endothermic. 2NH3(g) → N₂(g) + 3H₂(g) At equilibrium, it was found that the concentration of H₂ was 0.0584 M, the concentration of N₂ was 0.0195 M, and the concentration of NH3 was 0.430 M. What was the initial concentration of ammonia? b. What is the equilibrium constant at this temperature (K.)? C. A reaction mixture that is not at equilibrium contains 0.15 M H2, 0.25 M N2, and 3 M NH3. In order to reach equilibrium, will this reaction shift in the direction of reactants or products? Explain why. g of a nagy d. How would the system respond if the volume of the reaction vessel is increased? e. If the temperature of the reaction mixture is increased, how will this affect the amount of ammonia present at equilibrium?
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