Chem 162-2011 exam I review from 2008 exam I student copy

Chem 162-2011 exam I review from 2008 exam I student copy -...

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2011 REVIEW Chemistry 162 Exam I February 20, 2008 C162s08e1v1
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12 CHEM 162-2008 EXAM I CHAPTER 13 - KINETICS 10RATES, RATE CONSTANTS, REACTION ORDERS, HALF-LIVES CONCEPTS Which units of k are consistent with a fifth order rate law? A. M -5 s -1 B. M 4 s -1 C. M -4 s -4 D. M s -1 E . M -4 s -1 We can solve this in two ways: Reaction k Order units 0 M 1 s -1 1 M o s -1 2 M -1 s -1 By continuing the pattern: 3 M -2 s -1 4 M -3 s -1 5 M -4 s -1 or Rate = k[A] 5 Rate = (Y 2 -Y 1 )/(X 2 -X 1 ) = (M 2 -M 1 )/(s 2 -s 1 ) = M/s M/s = k[M] 5 k = (M/s)/M 5 = M -4 s -1 C162s08e1v1
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20 CHEM 162-2008 EXAM I CHAPTER 13 - KINETICS 10RATES, RATE CONSTANTS, REACTION ORDERS, HALF-LIVES CONCEPTS What is the rate of appearance of C when the rate of disappearance of A is 2.75×10 -4 M/s in the reaction below? 2A + B → 3C + D A . 4.13×10 -4 M/s B. 1.83×10 -4 M/s C. 8.25×10 -4 M/s D. 1.38×10 -4 M/s E. 5.50×10 -4 M/s Rate of appearance of C = 3/2 the rate of disappearance of A. 2.75 x 10 -4 M/s x 3/2 = 4.125 x 10 -4 C162s08e1v1
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2 CHEM 162-2008 EXAM I CHAPTER 13 - KINETICS 10RATES, RATE CONSTANTS, REACTION ORDERS, HALF-LIVES CONCEPTS Which of following will result in a straight line plot? A . A plot of 1/[A] vs. t for a second order reaction B. A plot of 1/[A] vs. t for a first order reaction. C. A plot of [A] vs. t for a second order reaction. D. A plot of ln [A] vs. t for a zero order reaction. E. A plot of [A] 2 vs. t for a second order reaction. A. True. For a second order reaction the integrated rate law is: 1/[C] t = kt + 1/[C] o Therefore, plotting 1/[C] t on the y-axis vs t on the x-axis will provide a straight line. B. False. For a first order reaction the integrated rate law is: ln[C] t = -kt + ln[C] o Therefore, plotting ln[C] t on the y-axis vs t on the x-axis will provide a straight line. C. False. For a second order reaction the integrated rate law is: 1/[C] t = kt + 1/[C] o Therefore, plotting 1/[C] t on the y-axis vs t on the x-axis will provide a straight line. D. False. For a zero order reaction the integrated rate law is: [C] t = -kt + [C] o Therefore, plotting [C] t on the y-axis vs t on the x-axis will provide a straight line. E. False. For a second order reaction the integrated rate law is: 1/[C] t = kt + 1/[C] o Therefore, plotting 1/[C] t on the y-axis vs t on the x-axis will provide a straight line. C162s08e1v1
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CHEM 162-2008 EXAM I CHAPTER 13 - KINETICS 11RATES,RATE CONSTANTS, REACTION ORDERS, HALF-LIVES CALCULATIONS Given the following data, what is the best estimate of the instantaneous rate at 5s? Time (s) [A] 0 5.00 5 3.03 10 1.84 15 1.12 20 0.68 A. 0.18 M/s B . 0.32 M/s C. 0.39 M/s D. 0.22 M/s E. 0.61 M/s Calculate an average rate centered around 5 seconds. Hence, calculate the rate between 0 and 10 seconds. Rate of disappearance of A = -(A
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This document was uploaded on 11/02/2011 for the course GEN CHEM 162 at Rutgers.

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Chem 162-2011 exam I review from 2008 exam I student copy -...

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