test_2 - Chem 112 Review for Test 2 Spring 2008 We are now...

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Chem 112 – Review for Test 2 Spring 2008 We are now in the position of being able to extract from experimental data the relationship between rate and concentration of reactant(s) at any temperature by finding values for the constants A, E a , m, and n. [ ] [ ] n m RT E B A Ae Rate a - = Once this relationship has been discovered, chemists use it to make educated guesses about reaction mechanisms. Collision theory is the link that allows these guesses to be made. Please be able to explain how collision theory is consistent with the observed temperature dependence of rate and how collision theory is consistent with the observed dependence of rate on the concentration of reactant. In particular, first and second order reactions happen in distinctly different ways. First order reactions are consistent with a slow step involving only a single molecule of reactant. Second order reactions are consistent with a slow step involving two molecules of reactant. Now if the mechanism is just a list of all the elementary steps which occur, and if the rate equation describes the kinetics of the slow step, then from the experimentally obtained rate equation we can deduce the molecularity of the slow step. Explain the concept of a catalyst and and intermediate in a reaction mechanism.
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test_2 - Chem 112 Review for Test 2 Spring 2008 We are now...

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