ReactionOrder - kt 1[A vs t k Note k terms are negative...

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Reaction Order r = -k C n Rate Expression Units 0 (where n = 0) r A = -k / independent of [A] (conc)(time) -1 e.g., kg/sec 1 (where n = 1) r A = -k[A] /dependent on [A] (time) -1 e.g., sec -1 , hr -1, day -1 2 (where n = 2) r A = -k[A] 2 (conc) -1 (time) -1 Plotting procedure to determine order of reaction: Order Rate Equation Integrated Equation Linear Plot Slope 0 d([A]/dt = -k [A] - [A] o = -kt [A] vs. t -k 1 d[A]/dt = -k[A] ln[A]/[A] o = -kt ln[A] vs. t -k 2 d[A]/dt = -k[A] 2 1/[A]–1/[A]
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Unformatted text preview: kt 1/[A] vs. t k Note: k terms are negative because A is a reactant and is disappearing (e.g., aA + bB → cC) Rate Law: r = -k C n where r = rate, k = reaction rate constant, C = concentration To solve problems: where [A] = conc @ t and [A] o = initial conc of A For zero-order reactions: use [A]-[A] o = -kt For first-order reactions: use ln[A]/[A] o = -kt or [A] = [A] o e-kt CE 3400/Reactions...
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