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6. What are the units for the rate constant, k, in this reaction? Are rate constant units always the same for every different reaction? Explain. 7. It was mentioned in the handout that what we measure in this experiment is the (average) initial rate of the reaction. We measure the time it takes for the first 6.0 x 104 M of I3 to form, and get the rate by dividing the change in concentration (=6.0x104 M) by that time. After this, the reaction then continues. What happens to the rate? Explain your answer. 8. Why do you think we say that you should stop timing at "the first appearance of blue color"? (Think about the consequences if some people stopped at the first appearance, and others waited until the flask was totally blue.)

6. What are the units for the rate constant, k, in this reaction? Are rate constant units always the same for every different reaction? Explain. 7. It was mentioned in the handout that what we measure in this experiment is the (average) initial rate of the reaction. We measure the time it takes for the first 6.0 x 104 M of I3 to form, and get the rate by dividing the change in concentration (=6.0x104 M) by that time. After this, the reaction then continues. What happens to the rate? Explain your answer. 8. Why do you think we say that you should stop timing at "the first appearance of blue color"? (Think about the consequences if some people stopped at the first appearance, and others waited until the flask was totally blue.)

Chemistry
Chemistry
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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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Answer questions 6,7 and 8 please Answer ASAP PLEASE
[S2Og1 Times (sec) M Ru Avera Rate Constant (list times to Rate () ge Time M nearest tenth of a Units %3D second) (sec) 32 1 0.080 0.040 30. 6.0e4/32-2.0e5 6.25e3 Mls 33. & 31. 0.040 0.040 56. 59 6.0e4/59 1.02e 6.375e M-s 60. & 60. 3 0.020 0.040 120. 120. 3.13e M's1 240 6.0e4/240-2.5e 4 0.010 0.040 229. 220 6.0e4/220-2.72e6 6.8e M's 210. 5 0.040 0.080 33. 30 6.0e4/30= 2.0e- 6.25e-3 M-ls-l 25. 0.040 0.040 59. 60 6.0e4/60- 1.0e-5 6.25 e-3M-1 s-1 60. 7. 0.040 0.020 137. 135 6.0e /135= 4.4e-6 5.5 e Ms1 132. 0.040 0.010 240. 240 6.0e /240= 2.5e6 6.25 eM-s-!
Transcribed Image Text:[S2Og1 Times (sec) M Ru Avera Rate Constant (list times to Rate () ge Time M nearest tenth of a Units %3D second) (sec) 32 1 0.080 0.040 30. 6.0e4/32-2.0e5 6.25e3 Mls 33. & 31. 0.040 0.040 56. 59 6.0e4/59 1.02e 6.375e M-s 60. & 60. 3 0.020 0.040 120. 120. 3.13e M's1 240 6.0e4/240-2.5e 4 0.010 0.040 229. 220 6.0e4/220-2.72e6 6.8e M's 210. 5 0.040 0.080 33. 30 6.0e4/30= 2.0e- 6.25e-3 M-ls-l 25. 0.040 0.040 59. 60 6.0e4/60- 1.0e-5 6.25 e-3M-1 s-1 60. 7. 0.040 0.020 137. 135 6.0e /135= 4.4e-6 5.5 e Ms1 132. 0.040 0.010 240. 240 6.0e /240= 2.5e6 6.25 eM-s-!
3. Why is it more instructive in detemining reaction order, to compare the rate of Expt 4 to Expt 3 rather than comparing Expt 3 to Expt 5? 4. Which experiment(s) had the greatest rate? Why was this the greatest rate? Which had the smallest rate? Why was this the smallest rate? Can you make a general statement about what rate depends on from the answers to this question? 5. Compare the value of k (the rate constant) for each of the experiments. Is it similar, the same, differet? It that what you expected? Why is it called a constant? 6. What are the units for the rate constant, k, in this reaction? Are rate constant units always the same for every different reaction? Explain. 7. It was mentioned in the handout that what we measure in this experiment is the (average) initial rate of the reaction. We measure the time it takes for the first 6.0 x 104 M of I3 to form, and get the rate by dividing the change in concentration (=6.0x104 M) by that time. After this, the reaction then continues. What happens to the rate? Explain your answer. 8. Why do you think we say that you should stop timing at "the first appearance of blue color"? (Think about the consequences if some people stopped at the first appearance, and others waited until the flask was totally blue.) 9. Look at Table 1, where you recorded the data for times of each experiment. Take experiment 1. Look at the times for that experiment. What are the typical fluctuations in the times? In other words, are the different time measurements for this experiment within 2 seconds of each other? 5? 10? More? Less? How many seconds? Do this for experiment 2 as well. Think of this range of seconds as the "error" in the time measurement for each experiment. Now answer this question... do you think that if you added or subtracted this "error" in the times from the average times for each experiment that it would alter your conclusion about the reaction order? Please give this some thought. What does this tell you about the reliability of your reaction order choices?
Transcribed Image Text:3. Why is it more instructive in detemining reaction order, to compare the rate of Expt 4 to Expt 3 rather than comparing Expt 3 to Expt 5? 4. Which experiment(s) had the greatest rate? Why was this the greatest rate? Which had the smallest rate? Why was this the smallest rate? Can you make a general statement about what rate depends on from the answers to this question? 5. Compare the value of k (the rate constant) for each of the experiments. Is it similar, the same, differet? It that what you expected? Why is it called a constant? 6. What are the units for the rate constant, k, in this reaction? Are rate constant units always the same for every different reaction? Explain. 7. It was mentioned in the handout that what we measure in this experiment is the (average) initial rate of the reaction. We measure the time it takes for the first 6.0 x 104 M of I3 to form, and get the rate by dividing the change in concentration (=6.0x104 M) by that time. After this, the reaction then continues. What happens to the rate? Explain your answer. 8. Why do you think we say that you should stop timing at "the first appearance of blue color"? (Think about the consequences if some people stopped at the first appearance, and others waited until the flask was totally blue.) 9. Look at Table 1, where you recorded the data for times of each experiment. Take experiment 1. Look at the times for that experiment. What are the typical fluctuations in the times? In other words, are the different time measurements for this experiment within 2 seconds of each other? 5? 10? More? Less? How many seconds? Do this for experiment 2 as well. Think of this range of seconds as the "error" in the time measurement for each experiment. Now answer this question... do you think that if you added or subtracted this "error" in the times from the average times for each experiment that it would alter your conclusion about the reaction order? Please give this some thought. What does this tell you about the reliability of your reaction order choices?
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