Chem_208_10_2007_final

Chem_208_10_2007_final - Prelim 1: Tues. Feb 27, 7:30-...

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Prelim 1: Tues. Feb 27, 7:30- 9:00PM Ch. 7,14 Rev. Session 1: Sun. 2:00 - 3:30 p.m. Baker 200 Rev. Session 2: 7:30 - 9:00 p.m. Mon. Statler Aud.
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Reaction Mechanism otes : 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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• provides a new reaction pathway of lower activation energy • involved in a reaction without undergoing permanent change • is not a reactant or product
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This note was uploaded on 05/18/2008 for the course CHEM 2080 taught by Professor Davis,f during the Spring '07 term at Cornell.

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Chem_208_10_2007_final - Prelim 1: Tues. Feb 27, 7:30-...

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