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C Chegg Study Guided Sc X Lyndon State College x C www.saplinglearning.com/ibiscms/mod/ibis/view.php?id 3173739 Apps HP Connected D estudent hus son O User Dashboard Apple 7 Disney EESPN Yahoo! C Chegg study l Guid D Mobile Ei My Husson 4/17/2017 11:00 PM o/100 Gradebook Attempts Score nt Calculator Periodic Table Question 26 of 33 Map EA Sapling Learning The following is a multi-step reaction. The rate-limiting step is unimolecular, with Aas the sole reactant. A B C+ D If [Al and CBI are both 0.180 M, then the rate of reaction is 0.0040 M/s. (a) What is the rate of the reaction if [A] is doubled? Number (b) Starting with the original concentrations, what is the rate of the reaction if IB]is halved? Number (c) Starting with the original concentrations, what is the rate of the reaction if LA] and [B) are both increased by a factor of five? Number A Previous ® Give Up & View Solution Check Answer Next Exit O Hint c 20 2017 Sapling Learning, Inc. privacy policy terms of use contact us help about us areers partners Other bookmarks o Assignment Information Available From: 3/27/2017 10:0 Due Date: 4/17/2017 11:0 Points Possible 00 Grade Category: Graded Description Policies: You can check your answers. You can view solutions when you up on any question. You can keep trying to answer each you get it right or give up You lose 59% of the points available in your question for each incorrect O eTextbook O Help With This Topic O Web Help & Videos O Technical Support and Bug Repo

Explanation / Answer

The following a multi-step reaction. The rate -limiting step is unimolecular with A as the sole reactant.
               A+B --> C+D
if [A] and [B] are both 0.180 M, then the rate of reaction is 0.0040 M/s.

For unimolecular reaction, the rate

   - d[A]/dt = -k1[A]
   - 0.0040 = -k1 (0.18 M)
   k1 = 0.0222 s-1
  
Since, its unimolecular reaction, the rate depends only on the concentration of A.

a) what is the rate of the reaction if [A] is doubled

       d[A]/dt = -0.0222 s-1(2x0.180 M) = 0.008 M/s
      
Therefore, the rate of the reaction will also double upon doubling the concentration [A]

b) what is the rate of reaction if the [B] is halved.

Since the rate of the reaction doesn't depend on the [B], there is no change in the rate of the reaction.

So, the rate of reaction = d[A]/dt = 0.0040 M/s.

c) What is the rate of the reaction if [A] and [B] are both increased by a factor of five.

Since, there is no dependancy of [B], we just plug the value [A] = 5x [A] in the rate equation.

d[A]/dt = -0.0222 s-1(5x0.180 M) = 0.02 M/s

So, the rate = 0.02 M/s

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