5. The above reaction was conducted at different initial concentrations of A and B and each time the initial rates of the reaction were determined (table 1) Table 1 Trial# 12 ● 3 [A] (M) 0.01 0.01 0.02 [B] (M) 181 (M) 0.02 0.04 0.01 The overall rate of the reaction = k [A]m [B]" Using the information on the table above explain: eta from which traits did you use and why? a) Is the reaction rate dependent on the concentration of A? the reaction By what factor the concentration of A changed? Overall rate (mol/sec) 0.001 0.004 0.002 0.002 . By what factor the overall reaction rate changed? • Is the reaction O-order with respect to A/is m =0? If not explain why? ils did you use? b) Is the reaction rate dependent on the concentration of B? down rate of the reaction= . By what factor the concentration of B changed? ● what factor the overall reaction rate changed? • Is the reaction 0-order with respect to B/is n = 0? If not explain why?
5. The above reaction was conducted at different initial concentrations of A and B and each time the initial rates of the reaction were determined (table 1) Table 1 Trial# 12 ● 3 [A] (M) 0.01 0.01 0.02 [B] (M) 181 (M) 0.02 0.04 0.01 The overall rate of the reaction = k [A]m [B]" Using the information on the table above explain: eta from which traits did you use and why? a) Is the reaction rate dependent on the concentration of A? the reaction By what factor the concentration of A changed? Overall rate (mol/sec) 0.001 0.004 0.002 0.002 . By what factor the overall reaction rate changed? • Is the reaction O-order with respect to A/is m =0? If not explain why? ils did you use? b) Is the reaction rate dependent on the concentration of B? down rate of the reaction= . By what factor the concentration of B changed? ● what factor the overall reaction rate changed? • Is the reaction 0-order with respect to B/is n = 0? If not explain why?
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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![### Determining Reaction Order Based on Experimental Data
The experiment described investigated the effect of varying initial concentrations of reactants A and B on the initial rate of a reaction. The data is summarized in the table below:
#### Table 1 - Experimental Data
| Trial # | [A] (M) | [B] (M) | Overall Rate (mol/sec) |
| ------- | ------- | ------- | --------------------- |
| 1 | 0.01 | 0.02 | 0.001 |
| 2 | 0.01 | 0.04 | 0.004 |
| 3 | 0.02 | 0.01 | 0.002 |
The overall rate of the reaction can be described by the rate equation:
\[ \text{Rate} = k [A]^m [B]^n \]
Using the information from Table 1, we can answer the following questions:
#### a) Dependency of the Reaction Rate on the Concentration of A
1. **Is the reaction rate dependent on the concentration of A?**
- **Explanation:** To determine if the reaction rate depends on the concentration of A, we compare Trials 1 and 3, where the concentration of B is kept constant at 0.01 M.
2. **By what factor the concentration of A changed?**
- In comparing Trials 1 and 3:
\[ \text{[A]} \text{ (trial 3)} = 0.02 \; \text{M}, \; \text{[A]} \text{ (trial 1)} = 0.01 \; \text{M} \rightarrow \text{Factor change} = \frac{0.02}{0.01} = 2 \]
3. **By what factor the overall reaction rate changed?**
- The reaction rate changes from 0.001 mol/sec (Trial 1) to 0.002 mol/sec (Trial 3):
\[ \text{Rate} \text{ (trial 3)} = 0.002 \; \text{mol/sec}, \; \text{Rate} \text{ (trial 1)} = 0.001 \; \text{mol/sec} \rightarrow \text{Factor change} = \frac{0.002}{0](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa3b13a71-cd62-4da6-9e1d-f686bcc45db9%2Fed0f9d7f-c275-45d4-ab47-15679542c7d5%2Ff8ta5ul_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Determining Reaction Order Based on Experimental Data
The experiment described investigated the effect of varying initial concentrations of reactants A and B on the initial rate of a reaction. The data is summarized in the table below:
#### Table 1 - Experimental Data
| Trial # | [A] (M) | [B] (M) | Overall Rate (mol/sec) |
| ------- | ------- | ------- | --------------------- |
| 1 | 0.01 | 0.02 | 0.001 |
| 2 | 0.01 | 0.04 | 0.004 |
| 3 | 0.02 | 0.01 | 0.002 |
The overall rate of the reaction can be described by the rate equation:
\[ \text{Rate} = k [A]^m [B]^n \]
Using the information from Table 1, we can answer the following questions:
#### a) Dependency of the Reaction Rate on the Concentration of A
1. **Is the reaction rate dependent on the concentration of A?**
- **Explanation:** To determine if the reaction rate depends on the concentration of A, we compare Trials 1 and 3, where the concentration of B is kept constant at 0.01 M.
2. **By what factor the concentration of A changed?**
- In comparing Trials 1 and 3:
\[ \text{[A]} \text{ (trial 3)} = 0.02 \; \text{M}, \; \text{[A]} \text{ (trial 1)} = 0.01 \; \text{M} \rightarrow \text{Factor change} = \frac{0.02}{0.01} = 2 \]
3. **By what factor the overall reaction rate changed?**
- The reaction rate changes from 0.001 mol/sec (Trial 1) to 0.002 mol/sec (Trial 3):
\[ \text{Rate} \text{ (trial 3)} = 0.002 \; \text{mol/sec}, \; \text{Rate} \text{ (trial 1)} = 0.001 \; \text{mol/sec} \rightarrow \text{Factor change} = \frac{0.002}{0
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