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Find the order of the reaction given initial rates and concentration. ?

** There is a typo on the photo, the third [A] (M) is actually 0.400 , not 0.053***

The answer choices are

n = 0

n = 0.5

n = 1

n = 3

Please explain how to solve. 

Attachment image

2 Answers

  • 1 month ago
    Favourite answer

    The reaction is 0 order. 

    If it were anything else, you would expect to see a much greater change in the rate of the reaction than is seen. 

    The rate law for this reaction would be: Rate = k[A]^n

    Rate 3/Rate 1 = 0.054/0.052 = (0.4/0.2)^n

    1.04 = 2^n

    n = 0

  • Anonymous
    1 month ago

    The answer:  n = 0

    The reaction is zeroth-order because the initial rate is constant when [A] varies.  This means that the initial rate is independent of [A].  The slight variation  in initial rate (0.052, 0.053 and 0.054 M/s) is due to acceptable experimental error.

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