Answer questions 6,7 and 8 pleaseAnswer ASAP PLEASE [S2Og1 Times (sec)MRuAveraRate Constant(list times toRate ()geTimeMnearest tenth of aUnits%3Dsecond)(sec)3210.080 0.04030.6.0e4/32-2.0e56.25e3 Mls33. & 31.0.040 0.04056.596.0e4/59 1.02e6.375e M-s60. & 60.30.020 0.040120.120.3.13e M's12406.0e4/240-2.5e40.0100.040229.2206.0e4/220-2.72e66.8e M's210.50.040 0.08033.306.0e4/30= 2.0e-6.25e-3 M-ls-l25.0.040 0.04059.606.0e4/60- 1.0e-56.25 e-3M-1 s-160.7.0.040 0.020137.1356.0e /135= 4.4e-65.5 e Ms1132.0.040 0.010240.2406.0e /240= 2.5e66.25 eM-s-! 3. Why is it more instructive in detemining reaction order, to compare the rate of Expt 4 to Expt 3 rather thancomparing 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 theanswers 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 thereaction. We measure the time it takes for the first 6.0 x 104 M of I3 to form, and get the rate by dividingthe change in concentration (=6.0x104 M) by that time. After this, the reaction then continues. Whathappens 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 aboutthe consequences if some people stopped at the first appearance, and others waited until the flask was totallyblue.)9. Look at Table 1, where you recorded the data for times of each experiment. Take experiment 1. Look at thetimes for that experiment. What are the typical fluctuations in the times? In other words, are the differenttime measurements for this experiment within 2 seconds of each other? 5? 10? More? Less? How manyseconds? Do this for experiment 2 as well. Think of this range of seconds as the "error" in the timemeasurement for each experiment. Now answer this question... do you think that if you added or subtractedthis "error" in the times from the average times for each experiment that it would alter your conclusion aboutthe reaction order? Please give this some thought. What does this tell you about the reliability of yourreaction order choices?

Question

Answer questions 6,7 and 8 pleaseAnswer ASAP PLEASE [S2Og1 Times (sec)MRuAveraRate Constant(list times toRate ()geTimeMnearest tenth of aUnits%3Dsecond)(sec)3210.080 0.04030.6.0e4/32-2.0e56.25e3 Mls33. & 31.0.040 0.04056.596.0e4/59 1.02e6.375e M-s60. & 60.30.020 0.040120.120.3.13e M's12406.0e4/240-2.5e40.0100.040229.2206.0e4/220-2.72e66.8e M's210.50.040 0.08033.306.0e4/30= 2.0e-6.25e-3 M-ls-l25.0.040 0.04059.606.0e4/60- 1.0e-56.25 e-3M-1 s-160.7.0.040 0.020137.1356.0e /135= 4.4e-65.5 e Ms1132.0.040 0.010240.2406.0e /240= 2.5e66.25 eM-s-! 3. Why is it more instructive in detemining reaction order, to compare the rate of Expt 4 to Expt 3 rather thancomparing 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 theanswers 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 thereaction. We measure the time it takes for the first 6.0 x 104 M of I3 to form, and get the rate by dividingthe change in concentration (=6.0x104 M) by that time. After this, the reaction then continues. Whathappens to the rate? Explain your answer.8. Why do you think we say that you should stop timing at &#34;the first appearance of blue color&#34;? (Think aboutthe consequences if some people stopped at the first appearance, and others waited until the flask was totallyblue.)9. Look at Table 1, where you recorded the data for times of each experiment. Take experiment 1. Look at thetimes for that experiment. What are the typical fluctuations in the times? In other words, are the differenttime measurements for this experiment within 2 seconds of each other? 5? 10? More? Less? How manyseconds? Do this for experiment 2 as well. Think of this range of seconds as the &#34;error&#34; in the timemeasurement for each experiment. Now answer this question... do you think that if you added or subtractedthis &#34;error&#34; in the times from the average times for each experiment that it would alter your conclusion aboutthe reaction order? Please give this some thought. What does this tell you about the reliability of yourreaction order choices?

Accepted Answer

The rate of the reaction is given as follows:
aA→bB
Rate=-1ad[A]dt=1bd[B]dt
rate of disappearance of…