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2. A 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. a. 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. WIF 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 ammoni. present at equilibrium?

2. A 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. a. 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. WIF 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 ammoni. present at equilibrium?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Can you help w/ #2 from a-e

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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