Chemical Kinetics

Chemical Kinetics - Chemical Kinetics Rate Laws r =...

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Chemical Kinetics – Rate Laws r = k[A]^m[B]^n[C]^p overall order = m + n + p + … First order reactions: R = k[A] exponential decay of reactant concentration [A] t = [A] o e -kt where k is rate constant ln[A] t vs. t straight line of slope –k Half-life t 1/2 = 0.693/k Second order: A P Rate = -∆[A]/ ∆t = k[A] 2 – differential rate [A] t = [A] o / (1+k[A] o t) 1/[A] t = kt + 1/[A] o Half-life: [A] t /[A] o = 1 / (1+k[A] o t) k[A] o t 1/2 = 1 t 1/2 = 1/k[A] o Half-life now depends on concentration! Zeroth-order kinetics: A Product Rate = k[A] o Rate = k, no concentration dependence, rate is constant [A] t = [A] o – kt (straight line) Half-life (0 th order): gets shorter as reaction proceeds Reaction mechanisms – the sequence of reaction steps that form the pathway from reactants to products Each step is an elementary reaction describing the reactive event of a molecule or group of 2 or 3 molecules. Stoichiometry of a balanced reaction predicts the rate law only for elementary (single-step) reactions.
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This note was uploaded on 06/12/2011 for the course HUMA 111 taught by Professor -- during the Spring '11 term at Rice.

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Chemical Kinetics - Chemical Kinetics Rate Laws r =...

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