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How is the equilibrium affected by an increase in volume? It shifts to the left. O It shifts to the right. It has no effect. O It cannot be determined.

How is the equilibrium affected by an increase in volume? It shifts to the left. O It shifts to the right. It has no effect. O It cannot be determined.

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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3H2(g) + N2(g) ⟷⟷ 2NH3(g) + Heat

--- ### Understanding Equilibrium Shifts **Question: How is the equilibrium affected by an increase in volume?** **Options:** 1. ○ It shifts to the left. 2. ○ It shifts to the right. 3. ○ It has no effect. 4. ○ It cannot be determined. --- ### Explanation: When the volume of a reaction system is increased, it typically leads to a decrease in pressure (assuming temperature is constant). According to Le Chatelier's Principle, the equilibrium will shift in the direction that counteracts this change—in this case, to the side with the greater number of gas molecules. - **Option 1: It shifts to the left.** This would be correct if the reaction produces fewer gas molecules on the left side. - **Option 2: It shifts to the right.** This would be correct if the reaction produces more gas molecules on the right side. - **Option 3: It has no effect.** This might be the case if the number of gas molecules is the same on both sides of the reaction. - **Option 4: It cannot be determined.** This might be chosen if there is insufficient information about the number of gas molecules involved in the reaction. Understanding the direction of the shift requires knowing the specific balanced equation for the reaction and the respective quantities of gas molecules on each side. For more detailed study on equilibrium and Le Chatelier's Principle, explore our comprehensive guides and interactive modules on chemical reactions and equilibrium shifts. ---
Transcribed Image Text:--- ### Understanding Equilibrium Shifts **Question: How is the equilibrium affected by an increase in volume?** **Options:** 1. ○ It shifts to the left. 2. ○ It shifts to the right. 3. ○ It has no effect. 4. ○ It cannot be determined. --- ### Explanation: When the volume of a reaction system is increased, it typically leads to a decrease in pressure (assuming temperature is constant). According to Le Chatelier's Principle, the equilibrium will shift in the direction that counteracts this change—in this case, to the side with the greater number of gas molecules. - **Option 1: It shifts to the left.** This would be correct if the reaction produces fewer gas molecules on the left side. - **Option 2: It shifts to the right.** This would be correct if the reaction produces more gas molecules on the right side. - **Option 3: It has no effect.** This might be the case if the number of gas molecules is the same on both sides of the reaction. - **Option 4: It cannot be determined.** This might be chosen if there is insufficient information about the number of gas molecules involved in the reaction. Understanding the direction of the shift requires knowing the specific balanced equation for the reaction and the respective quantities of gas molecules on each side. For more detailed study on equilibrium and Le Chatelier's Principle, explore our comprehensive guides and interactive modules on chemical reactions and equilibrium shifts. ---
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