22 Integration & Review

22 Integration & Review - Integration & Review Ch...

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1 Integration & Review Ch 13 Kinetics Ch 14 Equilibrium Ch 16 Acids & Bases 2 22 1[ ] 1[ ] [ ] Rate NO NO O tt t   The reaction rate can be determined by measuring the rate at which the concentration of any reactant or any product changes with time. Any such measurement needs to give the same positive value for the reaction rate, so normalization by a minus sign for reactants and the stoichiometric coefficient is necessary. 2 NO 2 2 NO + O 2 Rate of a Chemical Reaction
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3 Rate Law The rate law for a reaction gives the dependence of the rate on the concentrations of the reactants. Example Rate = k [CH 3 COOCH 3 ] x [OH - ] y The exponents x and y are called the orders of the reaction with respect to each respective reactant. The overall order is x + y. k is the rate constant for the reaction. The rate law is determined experimentally (method of initial rates) and then compared with predictions based on proposed mechanisms. 4 For a single substance, A, reacting Zero order [A] t = - k t + [A] 0 First order ln [A] t = - k t + ln [A] 0 Second order ___ 0 11 [] t kt A A  k t [A] Rate k[A] t [A] Rate 2 k[A] t [A] Rate Rate Laws Integrated Rate Laws What are the units of the rate constant, k, for each?
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5 Given a rate constant, k, identify the order of the reaction from its units. Zero order [A] t = - k t + [A] 0 First order ln [A] t = - k t + ln [A] 0 Second order Are the units in the following correct? A) YES B) NO C) How should I know? 0 order k has units M/time 1 st order k has units of 1/time 2 nd order k has units of 1/(M x time) 0 11 [] t kt A A  6 For each, what data should be plotted to obtain a straight line and determine k from the slope?
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This note was uploaded on 03/29/2010 for the course CHE 132 taught by Professor Hanson during the Spring '08 term at SUNY Stony Brook.

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22 Integration & Review - Integration & Review Ch...

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