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How is the equilibrium affected by an increase in pressure? It shifts to the right. It has no effect. O It shifts to the left.

How is the equilibrium affected by an increase in pressure? It shifts to the right. It has no effect. O It shifts to the left.

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

**Question: How is the equilibrium affected by an increase in pressure?** - ○ It shifts to the right. - ○ It has no effect. - ○ It shifts to the left. - ○ Cannot be determined. *Explanation:* This question is designed to test your understanding of Le Chatelier’s Principle in the context of chemical equilibrium. When the pressure of a system is increased, the system will react to counterbalance this change. Typically, the equilibrium will shift towards the side with fewer gas molecules. This minimizes the change in pressure. For example, consider the following reaction: \[ \text{N}_2(g) + 3\text{H}_2(g) \leftrightharpoons 2\text{NH}_3(g) \] In this case, increasing the pressure will shift the equilibrium towards the right, where there are fewer moles of gas (since 4 moles on the left become 2 moles on the right). Your ability to answer this question accurately requires knowledge of the specific reaction in question.
Transcribed Image Text:**Question: How is the equilibrium affected by an increase in pressure?** - ○ It shifts to the right. - ○ It has no effect. - ○ It shifts to the left. - ○ Cannot be determined. *Explanation:* This question is designed to test your understanding of Le Chatelier’s Principle in the context of chemical equilibrium. When the pressure of a system is increased, the system will react to counterbalance this change. Typically, the equilibrium will shift towards the side with fewer gas molecules. This minimizes the change in pressure. For example, consider the following reaction: \[ \text{N}_2(g) + 3\text{H}_2(g) \leftrightharpoons 2\text{NH}_3(g) \] In this case, increasing the pressure will shift the equilibrium towards the right, where there are fewer moles of gas (since 4 moles on the left become 2 moles on the right). Your ability to answer this question accurately requires knowledge of the specific reaction in question.
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