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I need help with this question it is very confusing What is the relationship between concentration of solution #1 and the reaction rate?

I need help with this question it is very confusing What is the relationship between concentration of solution #1 and the reaction rate?

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
Section: Chapter Questions
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I need help with this question it is very confusing What is the relationship between concentration of solution #1 and the reaction rate?
**Procedure A: Effect of Concentration** 1. Fill each buret on the stand with the solution that it is marked for. 2. Deliver exactly 10 ml of solution #1 into a clean, dry test tube from the buret. 3. Deliver exactly 10 ml of solution #2 into a separate clean, dry test tube. 4. Get the stopwatch ready, then mix solutions 1 and 2 by pouring back and forth between the test tubes three times. You should begin timing the reaction as soon as you begin mixing. Stop timing as soon as the color change occurs. You may need to practice this a few times before proceeding. 5. Repeat the above procedure using successive dilutions of solution #1 as per the data chart on the report sheet. 6. Calculate the reaction rate by using 100/(time in seconds). 7. On graph paper, plot a graph of your reaction rates vs. concentration by using a vertical scale or Y-axis representing reaction rate and a horizontal scale or X-axis representing ml of solution #1 (KIO₃).
Transcribed Image Text:**Procedure A: Effect of Concentration** 1. Fill each buret on the stand with the solution that it is marked for. 2. Deliver exactly 10 ml of solution #1 into a clean, dry test tube from the buret. 3. Deliver exactly 10 ml of solution #2 into a separate clean, dry test tube. 4. Get the stopwatch ready, then mix solutions 1 and 2 by pouring back and forth between the test tubes three times. You should begin timing the reaction as soon as you begin mixing. Stop timing as soon as the color change occurs. You may need to practice this a few times before proceeding. 5. Repeat the above procedure using successive dilutions of solution #1 as per the data chart on the report sheet. 6. Calculate the reaction rate by using 100/(time in seconds). 7. On graph paper, plot a graph of your reaction rates vs. concentration by using a vertical scale or Y-axis representing reaction rate and a horizontal scale or X-axis representing ml of solution #1 (KIO₃).
### Experimental Data Table This table presents experimental data for a series of chemical trials. Below is the information arranged in a structured format: | **Trial** | **KIO<sub>3</sub> + H<sub>2</sub>O** | **Test Tube 1** | **Test Tube 2** | **Starch** | **Time (sec)** | **Rate (100/t)** | |-----------|-------------------------------------|-----------------|-----------------|------------|----------------|------------------| | | **4** | 2 ml | 10 ml | 10 ml | 68 | 100/68 = 1.5 s<sup>-1</sup> | | | **3** | 5 ml | 10 ml | 10 ml | 32 | 100/32 = 3.1 s<sup>-1</sup> | | | **2** | 7 ml | 10 ml | 10 ml | 27 | 100/27 = 3.7 s<sup>-1</sup> | | | **1** | 10 ml | 10 ml | 10 ml | 18 | 100/18 = 5.5 s<sup>-1</sup> | ### Explanation: - **Trials:** There are four trials, labeled from 1 to 4. - **KIO<sub>3</sub> + H<sub>2</sub>O / Test Tube 1:** Indicates the volume of potassium iodate and water solution used. - **Test Tube 2:** Constant volume of 10 ml used in all trials. - **Starch:** Constant volume of 10 ml used in all trials. - **Time (sec):** The time taken for a reaction or event to occur during each trial. - **Rate (100/t):** The reaction rate calculated using the formula 100 divided by time (in seconds), expressing the rate in s<sup>-1</sup>. This table can be used to analyze the effect of varying the concentration of KIO<sub>3</sub> + H<sub>2</sub>O on the reaction time and rate.
Transcribed Image Text:### Experimental Data Table This table presents experimental data for a series of chemical trials. Below is the information arranged in a structured format: | **Trial** | **KIO<sub>3</sub> + H<sub>2</sub>O** | **Test Tube 1** | **Test Tube 2** | **Starch** | **Time (sec)** | **Rate (100/t)** | |-----------|-------------------------------------|-----------------|-----------------|------------|----------------|------------------| | | **4** | 2 ml | 10 ml | 10 ml | 68 | 100/68 = 1.5 s<sup>-1</sup> | | | **3** | 5 ml | 10 ml | 10 ml | 32 | 100/32 = 3.1 s<sup>-1</sup> | | | **2** | 7 ml | 10 ml | 10 ml | 27 | 100/27 = 3.7 s<sup>-1</sup> | | | **1** | 10 ml | 10 ml | 10 ml | 18 | 100/18 = 5.5 s<sup>-1</sup> | ### Explanation: - **Trials:** There are four trials, labeled from 1 to 4. - **KIO<sub>3</sub> + H<sub>2</sub>O / Test Tube 1:** Indicates the volume of potassium iodate and water solution used. - **Test Tube 2:** Constant volume of 10 ml used in all trials. - **Starch:** Constant volume of 10 ml used in all trials. - **Time (sec):** The time taken for a reaction or event to occur during each trial. - **Rate (100/t):** The reaction rate calculated using the formula 100 divided by time (in seconds), expressing the rate in s<sup>-1</sup>. This table can be used to analyze the effect of varying the concentration of KIO<sub>3</sub> + H<sub>2</sub>O on the reaction time and rate.
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