Kinetics+Part+3 - 1 Integrated Rate Laws Changes in...

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Integrated Rate Laws – Changes in concentration over time – Calculus applied to kinetics Consider the general reaction: A → B Rate = −∆[A] / ∆ t Rate = k [A] −∆[A] / ∆ t = k [A] Using calculus, the expression is integrated over time to obtain the integrated rate law for first order reaction : ln ([A] 0 / [A] t ) = kt or ln [A] 0 ln [A] t = kt second order reaction: Rate = [A] / −∆ t = k [A] 2 Integrating over time: (1 / [A] t ) (1 / [A] 0 ) = kt zero order reaction: Rate = [A] / −∆ t = k [A] 0 Integrating over time: [A] t [A] 0 = kt Problem: At 25 o C, HI breaks down slowly to hydrogen and iodide: rate = k [HI] 2 . The rate constant at 25 o C is 2.4 x 10 21 L/mol s. If 0.0100 mol of HI( g ) is placed in a 1.0-L container, how long will it take for the concentration of HI to reach 0.00900 mol/L? 1
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Determine reaction order from integrated rate law For a first order reaction: ln [A] 0 ln [A] t = kt ln [A] t = kt + ln [A] 0 y = mx + b second order:
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Kinetics+Part+3 - 1 Integrated Rate Laws Changes in...

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