Part A The rate constant for a certain reaction is k = 3.70x10-3 s Express your answer with the appropriate units. View Available Hint(s) [A] = 0.061 μA Submit Previous Answers Request Answer Part B X Incorrect; Try Again; 5 attempts remaining [A]o = M μA A zero-order reaction has a constant rate of 3.10x10-4 M/s. If after 65.0 seconds the concentration has dropped to 8.50x10-2 M, what was the initial concentration? Express your answer with the appropriate units. View Available Hint(s) Value ? Units If the initial reactant concentration was 0.150 M, what will the concentration be after 4.00 minutes? ?
Part A The rate constant for a certain reaction is k = 3.70x10-3 s Express your answer with the appropriate units. View Available Hint(s) [A] = 0.061 μA Submit Previous Answers Request Answer Part B X Incorrect; Try Again; 5 attempts remaining [A]o = M μA A zero-order reaction has a constant rate of 3.10x10-4 M/s. If after 65.0 seconds the concentration has dropped to 8.50x10-2 M, what was the initial concentration? Express your answer with the appropriate units. View Available Hint(s) Value ? Units If the initial reactant concentration was 0.150 M, what will the concentration be after 4.00 minutes? ?
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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I’m not sure where I went wrong. Please help with a and b.
![**Part A**
The rate constant for a certain reaction is \( k = 3.70 \times 10^{-3} \, \text{s}^{-1} \). If the initial reactant concentration was \( 0.150 \, \text{M} \), what will the concentration be after 4.00 minutes?
Express your answer with the appropriate units.
- **Input Box with Unit Selector:**
- \([A]_t =\) [Input: 0.061] [Unit Selector: M]
- **Submit Button**
- Feedback: Incorrect; Try Again; 5 attempts remaining
**Part B**
A zero-order reaction has a constant rate of \( 3.10 \times 10^{-4} \, \text{M/s} \). If after 65.0 seconds the concentration has dropped to \( 8.50 \times 10^{-2} \, \text{M} \), what was the initial concentration?
Express your answer with the appropriate units.
- **Input Box with Unit Selector:**
- \([A]_0 =\) [Input: Value] [Unit Selector: Units]
- **Submit Button**
**Hint and Feedback Options:**
- View Available Hint(s)
- Request Answer
- Provide Feedback
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Transcribed Image Text:**Part A**
The rate constant for a certain reaction is \( k = 3.70 \times 10^{-3} \, \text{s}^{-1} \). If the initial reactant concentration was \( 0.150 \, \text{M} \), what will the concentration be after 4.00 minutes?
Express your answer with the appropriate units.
- **Input Box with Unit Selector:**
- \([A]_t =\) [Input: 0.061] [Unit Selector: M]
- **Submit Button**
- Feedback: Incorrect; Try Again; 5 attempts remaining
**Part B**
A zero-order reaction has a constant rate of \( 3.10 \times 10^{-4} \, \text{M/s} \). If after 65.0 seconds the concentration has dropped to \( 8.50 \times 10^{-2} \, \text{M} \), what was the initial concentration?
Express your answer with the appropriate units.
- **Input Box with Unit Selector:**
- \([A]_0 =\) [Input: Value] [Unit Selector: Units]
- **Submit Button**
**Hint and Feedback Options:**
- View Available Hint(s)
- Request Answer
- Provide Feedback
No graphs or diagrams are present in this content.
Expert Solution
Step 1
We need to use the correct integrated rate law equation as per order of reaction to calculate the required value.
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