kinetics - Kinetics 1. Consider the following reaction:...

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Kinetics 1. Consider the following reaction: 3 A 2 B How is the average rate of appearance of B related to the average rate of disappearance of A? A. −Δ [A]/ Δ t = Δ [B]/ Δ t B. −Δ [A]/ Δ t = (2/3)( Δ [B]/ Δ t) C. −Δ [A]/ Δ t = (3/2)( Δ [B]/ Δ t) D. −Δ [A]/ Δ t = (1/2)( Δ [B]/ Δ t) E. −Δ [A]/ Δ t = (1/3)( Δ [B]/ Δ t) 2. The combustion of ethylene proceeds by the reaction: C 2 H 4 (g) + 3O 2 (g) Æ 2CO 2 (g) + 2H 2 O(g) When the rate of disappearance of O 2 is 0.23 M s 1 , what is the rate of appearance of CO 2 in M s 1 ? A. 0.15 B. 0.077 C. 0.69 D. 0.35 E. 0.46 3. Given the following kinetic data for the reaction, A + B + C products Experiment [A] (M) [B] (M) [C] (M) − Δ [A]/ Δ t (M/s) 1 0.10 0.10 0.10 7.0 x 10 -5 2 0.20 0.10 0.10 1.4 x 10 -4 3 0.10 0.20 0.10 7.0 x 10 -5 4 0.10 0.10 0.20 2.8 x 10 -4 The rate law for this reaction is: A. Rate = k[A][B][C] B. Rate = k[A] 2 [B] C. Rate = k[A] 2 [C] D. Rate = k[A][B][C] 2 E. None of these is the correct rate law.
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4. The decomposition of ethanol (C 2 H 5 OH) on an alumina (Al 2 O 3 ) surface was studied at 600K. C 2 H 5 OH (g) Æ C 2 H 4 (g) + H 2 O (g) Analysis of the data revealed the adjacent straight- line plot with a slope of 4.00 x 10 5 M 1 s 1 ___1 ___ [ C 2 H 5 OH] If the initial concentration of C 2 H 5 O H w a s , T i m e 1.25 x 10 -2 M, calculate the half-life for this reaction. A. 2.00 x 10 6 s B. 1.73x 10 4 s C. 5.73 x 10 3 s D. 45.7 s E. 106 s 5. Two substances A and B react with each other in such a way that A is 50% consumed in 33 minutes and 75% consumed in 66 minutes. Changing the concentration of B has no effect on the results. This reaction is: A. zero order in both A and B. B.
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kinetics - Kinetics 1. Consider the following reaction:...

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