Exam 1 (Early) - 2010

Exam 1 (Early) - 2010 - CHEM 188 Spring, 2010 Hour Exam 1...

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CHEM 188 – Spring, 2010 Hour Exam 1 (Early) February 10, 2010 Instructions: Your scantron answer sheet must show your NAME , 7-DIGIT KU ID NUMBER , and LAB SECTION . (Begin these entries at the LEFT end of the space provided.) In answering the questions, be careful to fill in the corresponding circles on the answer sheet according to the number of the question on the exam. USE A SOFT (No. 2) PENCIL .  Useful information: Gas constant, R = 8.314 J/K mol = 0.08206 L atm/K mol Integrated Rate Laws: kt [A] 1 [A] 1 : order Second e [A] [A] : order - First kt - [A] [A] : order - Zero 0 kt 0 0 + = - = = - Arrhenius equation: /RT -E a Ae k =  - = 2 1 2 1 a 2 1 T T T T R E k k ln Relation of K P to K C : K P = K C (0.0821 T) n Quadratic formula: a ac b b x 2 4 2 - ± - = 1
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1. Consider the reaction 2 NO( g ) + O 2 ( g ) 2 NO 2 ( g ) Suppose that at a particular moment during the reaction nitric oxide (NO) is reacting at the rate of 0.025 M /s. At what rate is NO 2 being formed? A. –0.050 M/s B. –0.025 M/s C. +0.025 M/s D. +0.050 M/s E. +0.10 M/s 2. The rate law for the reaction shown below is given by rate = k [NH 4 + ][NO 2 - ]. NH 4 + ( aq ) + NO 2 - ( aq ) N 2 ( g ) + 2 H 2 O( l ) At 25°C, the rate constant is 3.0 10 -4 / M s. Calculate the rate of the reaction at this temperature if [NH 4 + ] = 0.50 M and [NO 2 - ] = 0.080 M . A. 2.4 × 10 - 7 M/s B. 1.2 × 10 - 6 M/s C. 2.4 × 10 - 6 M/s D. 1.2 × 10 - 5 M/s E. none of the above 3. Consider the reaction given below. A + B products The following data are obtained at a certain temperature. [A] [B] rate ( M /s) 1.50 1.50 1.20 10 -1 1.50 2.50 1.20 10 -1 3.00 1.50 4.80 10 -1 Determine the rate law for this reaction. A. rate = k[A] B. rate = k[A] 2 C. rate = k[A][B] D. rate = k[A] 2 [B] E. rate = k[A][B] 2 4. If concentration is expressed in units of moles per liter (mol/L) and time in units of seconds (s), the units of a second-order rate constant are A. mol L - 1 s - 1 B. L 2 mol - 2 s - 1 C. s - 1 D. s - 2 E. L mol - 1 s - 1 2
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5. For what reaction-order does the half-life independent of the initial concentration?
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Exam 1 (Early) - 2010 - CHEM 188 Spring, 2010 Hour Exam 1...

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