- Use Le Chatelier's Principle to answer the questions about the following reversible reaction: 204 (g) = 2NO2 (g) a. If the concentration of N204 is increased, what will happen to the equilibrium of the reaction? Will it shift in the reverse direction to favor the formation of N204, will it shift forward to favor the formation of NO2, or will it stay the same? b. You are observing this reaction in a closed container. What will happen to the equilibrium if you increase the pressure inside the container? Will it shift in the reverse direction to favor the formation of N204, will it shift forward to favor the formation of NO2, or will it stay the same?
- Use Le Chatelier's Principle to answer the questions about the following reversible reaction: 204 (g) = 2NO2 (g) a. If the concentration of N204 is increased, what will happen to the equilibrium of the reaction? Will it shift in the reverse direction to favor the formation of N204, will it shift forward to favor the formation of NO2, or will it stay the same? b. You are observing this reaction in a closed container. What will happen to the equilibrium if you increase the pressure inside the container? Will it shift in the reverse direction to favor the formation of N204, will it shift forward to favor the formation of NO2, or will it stay the same?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 92QRT
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