2004 - Chem 2 Key #1 1. Exam #2 February 27, 2004 The...

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Chem 2 Exam #2 February 27, 2004 Key #1 1. The following reaction was observed for nitrous oxide (N 2 O): 2 N 2 O (g) ÷ 2 N 2(g) + O 2(g) The concentration of N 2 was measured as a function of time. The rate of the reaction is equal to: a) b) c) rate N t =− [] 2 rate N t = 2 rate N t = 2 2 d) e) rate N t = 2 2 rate N t 2 2 2. For the following reaction: 2 N 2 O 5(g) ÷ 4 NO 2(g) + O 2(g) the empirical rate law was: rate = k [N 2 O 5 ] What are the units of k if the concentration of N 2 O 5 is measured in atm? a) s -1 b) atm/s c) atm -1 s -1 d) atm-s e) atm -2 s -1 3. Using the reaction and empirical rate law in Question #2, the initial rate for the reaction was found to be 6.08 x 10 -6 atm/s when the initial pressure of N 2 O 5 was 0.010 atm. What will be the rate when the pressure of N 2 O 5 is 0.0020 atm? a) 6.08 x 10 -6 atm/s b) 1.21 x 10 -8 atm/s c) 3.04 x 10 -3 atm/s d) 1.22 x 10 -6 atm/s e) 3.04 x 10 -5 atm/s
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4. For the following reaction: NO 2(g) + CO (g) 6 NO (g) + CO 2(g) the data below were obtained: [NO 2 ], atm [CO], atm rate, atm/s 2.0 0.50 6.0 x 10 -3 2.8 0.50 1.2 x 10 -2 2.0 1.5 6.0 x 10 -3 What is the order of the reaction with respect to NO 2 ? a) zero order b) first order c) second order d) half-order e) third order 5. Using the data and reaction in Question #4, what is the order of the reaction with respect to CO? a) zero order b) first order c) second order d) half-order e) third order 6. For the following reaction: 2 NO 2(g) + F 2(g) ÷ 2 NO 2 F (g) the empirical rate law was: rate = k [NO 2 ] [F 2 ] What is the value of k if the initial rate 4.9 x 10 -3 atm/s when the pressure of NO 2 is 0.024 atm and the pressure of F 2 is 0.12 atm? a) 1.7 atm -1 s -1 b) 4.9 x 10 -3 atm/s c) 1.4 x 10 -5 atm -1 s -1 d) 0.58 atm-s e) 2.9 x 10-3 atm -1 s -1
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7. In Question #6, what will happen to the initial rate of the reaction if the pressure of NO 2 is doubled to 0.048 atm, and the pressure F 2 remains constant at 0.12 atm? a) the initial rate will double b) the initial rate will be unchanged c) the initial rate will decrease by ½ d) the initial rate will quadruple e) the initial rate will decrease by 1/4 8. In Question #6, what will happen to the initial rate of the reaction if the pressure of both NO 2 and F 2 are doubled to 0.048 atm and 0.24 atm, respectively? a) the initial rate will double b) the initial rate will be unchanged c) the initial rate will decrease by ½ d) the initial rate will quadruple e) the initial rate will decrease by 1/4 9. The following reaction has been observed in the gas phase: 2 NO (g) + F 2(g) ÷ 2 NOF (g) The mechanism below can be written for the reaction: Step 1: 2 NO (g) ÷ N 2 O 2(g) Step 2: N 2 O 2(g) + F 2(g) ÷ 2 NOF The empirical rate law is: rate = k [NO] 2 [F 2 ] If this mechanism is correct, which step is the slow step?
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This note was uploaded on 04/07/2008 for the course CHEM 002 taught by Professor Ryan during the Spring '08 term at Marquette.

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2004 - Chem 2 Key #1 1. Exam #2 February 27, 2004 The...

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