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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Question
![**Kinetics and Equilibrium: Writing the Concentration Equilibrium Expression**
**Task:**
Write the concentration equilibrium constant expression for this reaction:
\[ \text{CN}^-(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{HCN}(\text{aq}) + \text{OH}^-(\text{aq}) \]
**Diagram Explanation:**
The image includes a text box for inputting the equilibrium constant expression, and basic formatting tools are displayed next to it. These tools likely offer options for exponents or subscripts commonly used in chemical equations. There is a progress bar at the top right, indicating the current position in a sequence of tasks, labeled "1/5," with the first segment highlighted in green.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F868a7cc3-2ad7-4fe7-9a39-259d78c013d4%2Fe803b454-78fe-4a18-a7c9-958c3dd61a0d%2Fmzjrlzu_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Kinetics and Equilibrium: Writing the Concentration Equilibrium Expression**
**Task:**
Write the concentration equilibrium constant expression for this reaction:
\[ \text{CN}^-(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{HCN}(\text{aq}) + \text{OH}^-(\text{aq}) \]
**Diagram Explanation:**
The image includes a text box for inputting the equilibrium constant expression, and basic formatting tools are displayed next to it. These tools likely offer options for exponents or subscripts commonly used in chemical equations. There is a progress bar at the top right, indicating the current position in a sequence of tasks, labeled "1/5," with the first segment highlighted in green.
![### Predicting Relative Forward and Reverse Rates of Reaction
**Kinetics and Equilibrium**
**Reaction Description:**
Nitrogen and hydrogen react to form ammonia as described by the chemical equation:
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \]
Imagine 180 mmol of \(\text{NH}_3\) are added to an empty flask, and then answer the following questions.
**Questions:**
1. **What is the rate of the reverse reaction before any \(\text{NH}_3\) has been added to the flask?**
- Zero.
- Greater than zero, but less than the rate of the forward reaction.
- Greater than zero, and equal to the rate of the forward reaction.
- Greater than zero, and greater than the rate of the forward reaction.
2. **What is the rate of the reverse reaction just after the \(\text{NH}_3\) has been added to the flask?**
- Zero.
- Greater than zero, but less than the rate of the forward reaction.
- Greater than zero, and equal to the rate of the forward reaction.
- Greater than zero, and greater than the rate of the forward reaction.
3. **What is the rate of the reverse reaction at equilibrium?**
- Zero.
- Greater than zero, but less than the rate of the forward reaction.
- Greater than zero, and equal to the rate of the forward reaction.
- Greater than zero, and greater than the rate of the forward reaction.
4. **How much \(\text{NH}_3\) is in the flask at equilibrium?**
- None.
- Some, but less than 180 mmol.
- 180 mmol.
- More than 180 mmol.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F868a7cc3-2ad7-4fe7-9a39-259d78c013d4%2Fe803b454-78fe-4a18-a7c9-958c3dd61a0d%2Fchpb66u_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Predicting Relative Forward and Reverse Rates of Reaction
**Kinetics and Equilibrium**
**Reaction Description:**
Nitrogen and hydrogen react to form ammonia as described by the chemical equation:
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \]
Imagine 180 mmol of \(\text{NH}_3\) are added to an empty flask, and then answer the following questions.
**Questions:**
1. **What is the rate of the reverse reaction before any \(\text{NH}_3\) has been added to the flask?**
- Zero.
- Greater than zero, but less than the rate of the forward reaction.
- Greater than zero, and equal to the rate of the forward reaction.
- Greater than zero, and greater than the rate of the forward reaction.
2. **What is the rate of the reverse reaction just after the \(\text{NH}_3\) has been added to the flask?**
- Zero.
- Greater than zero, but less than the rate of the forward reaction.
- Greater than zero, and equal to the rate of the forward reaction.
- Greater than zero, and greater than the rate of the forward reaction.
3. **What is the rate of the reverse reaction at equilibrium?**
- Zero.
- Greater than zero, but less than the rate of the forward reaction.
- Greater than zero, and equal to the rate of the forward reaction.
- Greater than zero, and greater than the rate of the forward reaction.
4. **How much \(\text{NH}_3\) is in the flask at equilibrium?**
- None.
- Some, but less than 180 mmol.
- 180 mmol.
- More than 180 mmol.
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