ch13probs - Solomons Study Notes General Chemistry CHE 132...

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S olomon’s Study Notes General Chemistry CHE 132 Fall 2009 Midterm 1 Solomon Weiskop PhD Chapter 13 Practice Problems (Kinetics)
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Study Notes & Practice Problems are available to print out by registering at www.solomonlinetutor.com Solomon Weiskop PhD Solomon’s CHE 1 32 Tutoring © Copyright 2009
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1 Problems numbered in blue were written by Prof. Hanson [#1] For the following reaction, which one of the following is not correct? 2I + H 2 O 2 + 2H 3 O + I 2 + 4H 2 O (a) rate = I 2 ± / t (b) rate = −∆ H 3 O + ± / t (c) rate = −∆ H 2 O 2 ± / t (d) the rate decreases with time after the reaction begins (e) rate = 1 2 I ± / t (f) I ± decreases twice as fast as H 2 O 2 ± (g) I 2 ± increases half as fast as the rate at which I ± decreases [#2] Hydrogen iodide HI reacts to form hydrogen H 2 and iodine I 2 . If the concentration of HI is 0.050 M and then 100 s later it is 0.010 M, what is the average reaction rate over this interval? (a) 0.012 M min-1 (b) 4.0 × 10 4 M min 1 (c) 2.0 × 10 4 M min 1 (d) 0.024 M min -1 (e) 0.024 M min -1 [#3] 4NH 3 (g) +5O 2 (g) → 4NO(g) +6H 2 O(g) In an experiment it is found that the amount of NO increases from zero to 9g in 140 s. The reaction vessel is 50 mL. (a) Find the rate of change of the concentration of O 2 (in M/sec) (b) Find the overall rate for this reaction (in M/sec)
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[#4] For the reaction N 2 O 5 → 2NO 2 +1/2O 2 (a) Calculate the average reaction rate during the time interval from 0.5 to 1.0 hours (in M/hr) by using the data below Time (hr) [N 2 O 5 ] (M) 0.00 0.849 0.50 0.733 1.00 0.633 2.00 0.472 (b) Calculate the average rate of production of O 2 (in M/hr) during this same time interval. [#5] A reaction mechanism predicts the following rate law. What does this rate law predict to happen to the initial rate of the reaction if the concentration of each of the reactants is increased by a factor of 4? rate = k CHCl 3 ± Cl 2 ± 1/2 (a) the rate increases by 2 times (b) the rate increases by 8 times (c) the rate increases by 16 times (d) the rate doesn’t change (e) the rate increases by 4 times [#6] 2NO(g) +Br 2 (g) → 2NOBr(g) Experiments show that this reaction is first order in Br 2 and second order in NO. Which are incorrect? (May be more than one.) (a) The rate law is third order overall. (b) If the concentration of Br 2 is tripled, the rate will increase by a factor of 3. (c) If the concentration of NO is tripled, the rate will increase by a factor of 9 (d) If the concentration of NO is decreased by ½ and Br 2 is increased by a factor of two the rate will remain constant. (e) The value of k is independent of temperature. (f) The value of k is independent of concentration.
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This note was uploaded on 06/12/2011 for the course CHE 132 taught by Professor Hanson during the Spring '08 term at SUNY Stony Brook.

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ch13probs - Solomons Study Notes General Chemistry CHE 132...

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