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Practice problems on chemical kinetics for students enrolled in chem 3410 at the richard stockton college of new jersey. The problems involve deriving rate laws for reversible and irreversible reactions, as well as determining the apparent orders of reactions based on rate constants.
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Chemistry Program, School of Natural Sciences and Mathematics PO Box 195, Pomoma, NJ
November 21, 2008
H 2 + I 2 โโฝ 2 HI
However, direct bimolecular reaction between H 2 and I 2 is not observed to occur. A proposed mechanism for the forward reaction is: I 2 โโฝ 2 I (1) H 2 + 2 I โ 2 HI (2)
(a) Derive a rate law assuming that step (1) is reversible, step (2) is irreversible and step (2) is the slowest process. (b) Derive a rate law assuming that step (1) is reversible, step (2) is irreversible and step (2) is the fastest process. You can use the steady-state approximation for the concentration of the intermediate [I].
Hint: For both parts, be sure to pay careful attention to the stoichiometry of the proposed elementary reactions.
Suppose that the mechanism of this reaction is found to consist of the following elementary reac- tions: A + B
k 1 EGGGGGGGGGGCGG kโ 1
k 2 GGGGGGA D
(a) Show that this mechanism is consistent with the overall reaction. (b) Write expressions for d dt[C ]and d[ dtD ]in terms of [A], [B], [C], [D], k 1 , kโ 1 , and k 2. (c) Impose the steady-state approximation and solve for [C]ss. (d) Use the steady-state approximation to derive the rate law for d[ dtD ] in terms of [A], [B], k 1 , kโ 1 , and k 2. (e) If k 2 [A] kโ 1 what are the apparent orders of the reaction with respect to [A] and [B]? (f) If k 2 [A] kโ 1 what are the apparent orders of the reaction with respect to [A] and [B]?