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Chem_215_Lect_30_Color

Chem_215_Lect_30_Color - Prelim 2 Thurs Nov 8 7:00 8:30 PM...

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1 Prelim 2: Thurs. Nov. 8, 7:00- 8:30 PM Covers: Ch. 10 (except 10.12 - 10.14) Ch. 11 (except 11.8), Ch 4.10 - 4.11 Ch. 15.1 - 15.5 Problem Sets 6 - 9
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2 Reaction Mechanism Notes : Exponents in rate law are the stoichiometric coefficients. Elementary processes are reversible, may reach eq’m with equal rates of forward and reverse reactions. Reaction intermediates may be formed and consumed in elementary steps. They cannot appear in the overall chemical equation or in the overall rate law expression. The “rate determining step” occurs much more slowly than the others. Common Mechanisms : 1. Slow step followed by a fast step. 2. Fast reversible step followed by a slow step. 3. If not clear which step is slow, apply steady state approx . NO 2 (g) + CO (g) NO (g) + CO 2 (g) 2NO (g) + O 2 (g) 2NO 2 (g) 2NO (g) + O 2 (g) 2NO 2 (g)
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3 We have seen two methods for determining rate laws and k: - Method of Initial Rates. - Graphical analysis of [A] vs. time (good for A prods.) For complex systems, it is often convenient to carry out experiments under pseudo first order conditions.
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