Lecture 6 - Integrated Rate Law The differential rate law...

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Integrated Rate Law Integrated Rate Law W The differential rate law relates the rate of reaction to the concentration of reactants W The integrated rate law relates concentration and time W Below is first order [] [] A k dt A d = [ ] [] = kdt A A d [ ] [] kt A A = 0 ln
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More Integrated Rate Laws More Integrated Rate Laws W Only going to deal with integral orders W First order aA Products ln [A] = -kt + ln[A] 0 Tells us concentration as a function of time A plot of ln[A] vs t yields a straight line with slope -k
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Example Example W 2N 2 O 5 (g) 4NO 2 (g) + O 2 (g) obeys the rate law r=6.93×10 -3 s -1 [N 2 O 5 ] W If we start with 0.100M N 2 O 5 , how much N 2 O 5 after 150s? ln[A] = -6.93×10 -3 s -1 150s + ln(0.100) [A] = 0.0353M W We could ask about amount of product, or predict what initial concentration was.
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Half life W Because [A]/[A] 0 = e -kt , the amount of time it takes for any given fraction to disappear is constant W For historical reasons, we care about the time it takes for ½ to disappear. ln( ½ ) = -kt
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Lecture 6 - Integrated Rate Law The differential rate law...

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