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Unformatted text preview: Worksheet 4 Solutions. Data Set 1 Solution: First, determine the order of reaction; since a linear relationship is seen for ln[C], the reaction is first order. Therefore, the rate is k[C]. Data at 300K Data at 310 K Time(s) [C] 1/[C] ln[C] [C] Time (s) [C] ln[C] 1/[C] [C] 1 0.12 8.3333332.1202 0.12 1 0.0742.6036 13.51351 0.074 2 0.074 13.513512.603 0.074 2 0.0273.6119 37.03704 0.027 3 0.044 22.727273.123 0.044 3 0.0094.7105 111.1111 0.009 4 0.027 37.037043.611 0.027 4 0.00365.6268 277.7778 0.0036 5 0.016 62.54.135 0.016 5 0.00136.6453 769.2308 0.0013 6 0.009 111.11114.710 0.009 6 0.00057.6009 2000 0.0005 8 0.0036 277.77785.6268 0.0036 7 6.7E059.610 14925.37 6.7E05 10 0.0013 769.23086.6453 0.0013 10 9E0611.607 109890.1 9.1E06 Solve for rate constant, k , and initial concentration, C , directly knowing the order, using integrated rate law: ln [C] = kt + ln [C ] so slope = k and y intercept = ln[C ]. At 300K curve fit yields y = 0.5x1.6; k = 0.5 sec1 and [C o ] = 0.2M At 310 K curve fit yields y = 1.0x1.6; k = 1.0 sec1 and [C o ] = 0.2M Solve for half life, t1/2, for second order reaction: t 1/2 = 0.693/k At 300 K , t 1/2 = 0.639/0.5sec1 = 1.39 sec. At 310K, t 1/2 = 0.693/1 sec1 = 0.693 sec Solve for activation energy,...
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This homework help was uploaded on 04/12/2008 for the course CH 302 taught by Professor Holcombe during the Spring '07 term at University of Texas at Austin.
 Spring '07
 Holcombe
 Chemistry, Reaction

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