chem107f07wk12s

chem107f07wk12s - A B Kinetics: Reaction Rates Chp. 11 k CF...

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Unformatted text preview: A B Kinetics: Reaction Rates Chp. 11 k CF 2 Cl 2 ( g ) + h CF 2 Cl( g ) + Cl( g ) Cl( g ) + O 3 ( g ) ClO( g ) + O 2 ( g ) 2ClO( g ) O 2 ( g ) + 2Cl( g ) ____________________________________________________ 2O 3 ( g ) 3O 2 ( g ) 1995 Crutzen, Molina and Rowland Nobel Prize in Chemistry Kinetics Ozone in the Upper Atmosphere t B t A time in change ion concentrat in change = = ] [ ] [ _ _ _ _ time concentration A B Reaction Rates Chp. 11.2 C 4 H 9 Cl( aq ) + H 2 O( l ) C 4 H 9 OH( aq ) + HCl( aq ) Reaction Rates Chp. 11.2 C 4 H 9 Cl( aq ) + H 2 O( l ) C 4 H 9 OH( aq ) + HCl( aq ) Reaction Rates Chp. 11.2 aA + bB cC + dD t D d t C c t B b t A a = = = 1 1 1 1 In general t O t O = ] [ ] [ 2 1 2 O 2 (g) + h 2 O(g) Reaction Rates Chp. 11.2 If the rate of appearance of oxygen is 6.0 x 10-5 M/s at a particular instant, what is the value of the rate of disappearance of ozone? 2O 3 (g) 3O 2 (g) Effect of concentration on reaction rate. aA + bB cC + dD Rate = k[A] n [B] m Rate constant, k, is large for high reaction rates and is dependent on temperature. Units of k vary with reaction order. Reaction orders, n and m, may be independent of stoichiometric coefficients, a and b. Overall reaction order is n + m. Rate Laws Chp. 11.3 1 st Order Reactions Rate = k[A] 1 n x [A] o n 1 x rate o 2 nd Order Reactions Rate = k[A] 2 n x [A] o n 2 x rate o i th Order Reactions Rate = k[A] i n x [A] o n i x rate o th Order Reactions Rate = k n x [A] o rate o Rate Laws Chp. 11.3 ouston Sources of NOx Industry 50% raffic 30%...
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chem107f07wk12s - A B Kinetics: Reaction Rates Chp. 11 k CF...

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