**Consider the system at equilibrium.** \[ 2 \text{H}_2 (g) + \text{S}_2 (g) \rightleftharpoons 2 \text{H}_2\text{S} (g) \] **How will increasing the concentration of H₂ shift the equilibrium?** - ○ to the right - ○ no effect - ○ to the left **Explanation:** This is a typical equilibrium scenario involving Le Chatelier’s principle. When the concentration of a reactant is increased, the system will adjust to minimize this change by shifting the equilibrium position. In this case, increasing the concentration of \( \text{H}_2 \) will cause the equilibrium to shift to the right, favoring the formation of more \( \text{H}_2\text{S} \). **Equilibrium Shifts in Chemical Reactions** *Question 1:* How will increasing the concentration of H₂S shift the equilibrium? - ⦿ to the right - ○ to the left - ○ no effect *Question 2:* How will adding a catalyst shift the equilibrium? - ○ no effect - ○ to the left - ○ to the right **Explanation:** 1. **Increasing the Concentration of H₂S:** - Selecting "to the right" indicates that increasing the concentration of hydrogen sulfide (H₂S) will cause the equilibrium to shift in the forward direction, favoring the production of the products. 2. **Adding a Catalyst:** - The option for "no effect" suggests that adding a catalyst will not change the position of the equilibrium, although it will speed up the rate at which equilibrium is reached. There are no graphs or diagrams present in this content.
**Consider the system at equilibrium.** \[ 2 \text{H}_2 (g) + \text{S}_2 (g) \rightleftharpoons 2 \text{H}_2\text{S} (g) \] **How will increasing the concentration of H₂ shift the equilibrium?** - ○ to the right - ○ no effect - ○ to the left **Explanation:** This is a typical equilibrium scenario involving Le Chatelier’s principle. When the concentration of a reactant is increased, the system will adjust to minimize this change by shifting the equilibrium position. In this case, increasing the concentration of \( \text{H}_2 \) will cause the equilibrium to shift to the right, favoring the formation of more \( \text{H}_2\text{S} \). **Equilibrium Shifts in Chemical Reactions** *Question 1:* How will increasing the concentration of H₂S shift the equilibrium? - ⦿ to the right - ○ to the left - ○ no effect *Question 2:* How will adding a catalyst shift the equilibrium? - ○ no effect - ○ to the left - ○ to the right **Explanation:** 1. **Increasing the Concentration of H₂S:** - Selecting "to the right" indicates that increasing the concentration of hydrogen sulfide (H₂S) will cause the equilibrium to shift in the forward direction, favoring the production of the products. 2. **Adding a Catalyst:** - The option for "no effect" suggests that adding a catalyst will not change the position of the equilibrium, although it will speed up the rate at which equilibrium is reached. There are no graphs or diagrams present in this content.
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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![**Consider the system at equilibrium.**
\[ 2 \text{H}_2 (g) + \text{S}_2 (g) \rightleftharpoons 2 \text{H}_2\text{S} (g) \]
**How will increasing the concentration of H₂ shift the equilibrium?**
- ○ to the right
- ○ no effect
- ○ to the left
**Explanation:**
This is a typical equilibrium scenario involving Le Chatelier’s principle. When the concentration of a reactant is increased, the system will adjust to minimize this change by shifting the equilibrium position. In this case, increasing the concentration of \( \text{H}_2 \) will cause the equilibrium to shift to the right, favoring the formation of more \( \text{H}_2\text{S} \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc14feaa7-f26c-4630-9d28-afce0e4a19e9%2F05397f02-af83-44ff-b7d6-521dfeff67da%2Fgc907kt_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Consider the system at equilibrium.**
\[ 2 \text{H}_2 (g) + \text{S}_2 (g) \rightleftharpoons 2 \text{H}_2\text{S} (g) \]
**How will increasing the concentration of H₂ shift the equilibrium?**
- ○ to the right
- ○ no effect
- ○ to the left
**Explanation:**
This is a typical equilibrium scenario involving Le Chatelier’s principle. When the concentration of a reactant is increased, the system will adjust to minimize this change by shifting the equilibrium position. In this case, increasing the concentration of \( \text{H}_2 \) will cause the equilibrium to shift to the right, favoring the formation of more \( \text{H}_2\text{S} \).
Transcribed Image Text:**Equilibrium Shifts in Chemical Reactions**
*Question 1:*
How will increasing the concentration of H₂S shift the equilibrium?
- ⦿ to the right
- ○ to the left
- ○ no effect
*Question 2:*
How will adding a catalyst shift the equilibrium?
- ○ no effect
- ○ to the left
- ○ to the right
**Explanation:**
1. **Increasing the Concentration of H₂S:**
- Selecting "to the right" indicates that increasing the concentration of hydrogen sulfide (H₂S) will cause the equilibrium to shift in the forward direction, favoring the production of the products.
2. **Adding a Catalyst:**
- The option for "no effect" suggests that adding a catalyst will not change the position of the equilibrium, although it will speed up the rate at which equilibrium is reached.
There are no graphs or diagrams present in this content.
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