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Using the plots from Figure 2 again, plot (i) graphs In[AJ versus time. The value of k for this reaction can be determined as In[A] - [A]o 1 [A], Time Time Time i ii i Figure 2. Plots for three different reaction rates. k = -slope k = In(slope) k = 1/slope k = slope '[v] "[v] In[A];

Using the plots from Figure 2 again, plot (i) graphs In[AJ versus time. The value of k for this reaction can be determined as In[A] - [A]o 1 [A], Time Time Time i ii i Figure 2. Plots for three different reaction rates. k = -slope k = In(slope) k = 1/slope k = slope '[v] "[v] In[A];

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Using the plots from Figure 2 again, plot (i) graphs ln[A] versus time. The value of k for this reaction can be determined as __.** ### Graph Descriptions: - **Plot i (ln[A] vs. Time):** - **Axes**: The vertical axis is labeled as ln[A] with the initial concentration ln[A]_0 at the top. The horizontal axis is labeled as Time. - **Line**: A red line with a negative slope indicates a linear relationship, suggesting a first-order reaction where the rate constant can be determined from the slope. - **Plot ii (1/[A] vs. Time):** - **Axes**: The vertical axis is labeled as 1/[A] with the initial value 1/[A]_0 at the bottom. The horizontal axis is labeled as Time. - **Line**: A red line with a positive slope displays a linear relationship, typically associated with a second-order reaction. - **Plot iii ([A] vs. Time):** - **Axes**: The vertical axis is labeled as [A] with the initial concentration [A]_0 at the top. The horizontal axis is labeled as Time. - **Line**: A red line with a negative slope, indicating a zero-order reaction where the concentration decreases linearly over time. ### Figure 2: **Plots for three different reaction rates.** - ○ k = –slope - ○ k = ln(slope) - ○ k = 1/slope - ○ k = slope
Transcribed Image Text:**Using the plots from Figure 2 again, plot (i) graphs ln[A] versus time. The value of k for this reaction can be determined as __.** ### Graph Descriptions: - **Plot i (ln[A] vs. Time):** - **Axes**: The vertical axis is labeled as ln[A] with the initial concentration ln[A]_0 at the top. The horizontal axis is labeled as Time. - **Line**: A red line with a negative slope indicates a linear relationship, suggesting a first-order reaction where the rate constant can be determined from the slope. - **Plot ii (1/[A] vs. Time):** - **Axes**: The vertical axis is labeled as 1/[A] with the initial value 1/[A]_0 at the bottom. The horizontal axis is labeled as Time. - **Line**: A red line with a positive slope displays a linear relationship, typically associated with a second-order reaction. - **Plot iii ([A] vs. Time):** - **Axes**: The vertical axis is labeled as [A] with the initial concentration [A]_0 at the top. The horizontal axis is labeled as Time. - **Line**: A red line with a negative slope, indicating a zero-order reaction where the concentration decreases linearly over time. ### Figure 2: **Plots for three different reaction rates.** - ○ k = –slope - ○ k = ln(slope) - ○ k = 1/slope - ○ k = slope
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