1442test2 - 1442 Test 2 Chapters 16 & 17 Kinetics and...

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1442 Test 2 Chapters 16 & 17 Kinetics and Equilibrium (Silberberg) website: http://dipowell1.home.mindspring.com Useful Information: ln [A] o / [A t ] = kt 1 st order 1 / [A] t – 1 / [A] o = kt 2 nd order t 1 2 = ln 2 k t 1 2 = 1 k[A] o ln k 2 / k 1 = - E a /R (1 / T 2 – 1 / T 1 ) R = 8.314 J/mol.K Chemical Kinetics Chapter 16 Deriving the Rate Law 1. The following rate data were measured for the reaction: A + B C + D. What is the rate law? Initial [ A ] Initial [ B ] Initial Rate (M/s) 0.1 0.2 0.004 0.1 0.3 0.0135 0.3 0.4 0.288 2. What is the rate equation for the elementary reaction: 2 NO 2 O 2 + N 2 O 2 ? (a)Rate = k [ O 2 ] (b) Rate = k [ N 2 O 2 ] (c) Rate = k [ NO 2 ] (d) Rate = k [ NO 2 ] 2 Using the integrated rate law equations for first and second order reactions 3. SO 2 Cl 2 (g) decomposes in a first order reaction to produce SO 2 (g) and Cl 2 (g). From the date below relating the partial pressure of SO 2 Cl 2 (g) to time, determine the rate constant for the reaction. SO 2 Cl 2 (atm) Time, Sec 1.000 0 0.803 10,000
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(a) 2.2 X 10 -5 /s (b) 9.5 X 10 -6 /s (c) 8.0 X 10 -5 /s (d) 1.0 X 10 -4 /s (e) 2.0 X 10 -5 /s 4. The decomposition of nitrosyl chloride is a bimolecular reaction involving two nitrosyl chloride molecules and therefore is second order. If the rate constant for the reaction at room temperature is 0.020 liter mol -1 s -1 , what will be the concentration of NOCl be after 2 minutes if the initial concentration was .200 M? (a) .14 M (b) .07 M (c) .09 M (d) .12 M (e) .16 M 5. The decomposition of nitrogen dioxide to produce nitric oxide and oxygen is a second-order reaction. For this reaction, a plot of which variables should produce a
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This note was uploaded on 10/13/2009 for the course CHEM 1442 taught by Professor Rogers during the Fall '08 term at UT Arlington.

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1442test2 - 1442 Test 2 Chapters 16 & 17 Kinetics and...

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