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This 2 page Class Notes was uploaded by Audrey Notetaker on Friday February 19, 2016. The Class Notes belongs to 111001 at Boston College taught by Neil Wolfman in Fall 2016. Since its upload, it has received 28 views. For similar materials see General Chemistry II in Chemistry at Boston College.
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Date Created: 02/19/16
Chapter 13: Intro to Kinetics 2/15/16 What affects rate: Concentration of reactants Presence of a catalyst Temperature – most reactions go faster at higher temperatures Surface area (if working with a solid) Rate of Reaction: depends on the amount of product formed per unit time and the amount of reactant used per unit time *always positive *Can titrate the acetic acid to see how fast the reaction is going and watch it over time *If changing the number of moles of gas in a sealed vessel you can measure change in pressure (greater change = faster rate) *can also use a spectrophotometer to measure the concentration by watching the change in color concentration over time Beer’s Law: A=c*l*e A= absorbance l = cuvet path length (cm) C= concentration (M) e= a constant Rate = K[A][B] K= rate constant independent of temperature but dependent on temperature Reaction order: dependent on the exponents in the rate equation Can be integers, negative values, fractions, or 0 (if the concentration does not impact rate) 2x concentration – 2x rate m=1 2x concentration – 4x rate m=2 2x concentration – 8x rate m=3 2x concentration – no change m=0 2x concentration – ½x rate m= 1 4x concentration – 2x rate m=1/2 Chapter 13: The Rate Law 2/19/16 1st Order: ln([A]t/[A]t=0) = kt Order: (1/[A]t) = kt + (1/[A]t=0) 0 Order: [A]t = kt + [A]t=0 Halflife: how long does it take for 50% of reactants to react If half life doesn’t change by concentration then the reaction is first order
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