122ch14hmwk_add - t 1/2 = 7.6 min; 0.0015 M, 3.7 min;...

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Chapter 14 - Kinetics Additional Practice Problems 1) A hypothetical reaction A ----> products is second order in A. The half-life of a reaction that was initially 1.66 M in A is 310 min. What is the value of the rate constant, k ? 2) A reaction shows the same half-life regardless of the starting concentration of the reactant. Is it a zero-order, first-order or second-order reaction? 3) In three different experiments the following results were obtained for the reaction A ----> products: [A] 0 = 1.00 M, t 1/2 = 50 min; [A] 0 = 2.00 M, t 1/2 = 25 min; [A] 0 = 0.50 M, t 1/2 = 100 min. Write the rate equation for this reaction and indicate the value of k . 4) Ammonia decomposes on the surface of a hot tungsten wire. Following are the half-lives that were obtained at 1100 °C for different initial concentrations of NH 3 : [NH 3 ] 0 = 0.0031 M,

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Unformatted text preview: t 1/2 = 7.6 min; 0.0015 M, 3.7 min; 0.00068 M, 1.7 min. For this decomposition reaction, what is (a) the order of the reaction; (b) the rate constant k ? 5) The gas-phase reaction of chlorine with carbon monoxide to form phosgene, Cl 2 (g) + CO (g) ----> COCl 2 (g), obeys the following rate law: ) [COCl 2 ] Rate = -------------- = k [Cl 2 ] 3/2 [CO] (exp. rate law) ) t A mechanism involving the following series of steps is consistent with the rate law: Cl 2 º 2C1 Cl + CO º COCl COCl + Cl 2 º COCl 2 + Cl Assuming that this mechanism is correct, which of the steps above is the slow, or rate-determining, step? Explain. Hint: try making each step the slowest step (rate-det. step) and see what rate law you get and if it agrees with the experimental rate law given....
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This note was uploaded on 06/11/2011 for the course CHEM 122 taught by Professor Zellmer during the Spring '07 term at Ohio State.

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122ch14hmwk_add - t 1/2 = 7.6 min; 0.0015 M, 3.7 min;...

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