Consider the following reaction: A+B+C→D The rate law for this reaction is as follows: Rate=k[A][C]2[B]1/2 Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.13x10-2 M/s. What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? Rate 2= ? M/s (the answer is not 0.1566 M/s) (I've posted this question before and the answer is not

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Consider the following reaction:
A+B+C→D
The rate law for this reaction is as follows:
Rate=k[A][C]2[B]1/2
Suppose the rate of the reaction at certain
initial concentrations of A, B, and C is
1.13x10-2 M/s.
What is the rate of the reaction if the
concentrations of A and C are doubled and
the concentration of B is tripled?
Rate 2= ? M/s
(the answer is not 0.1566 M/s)
(I've posted this question before and the
answer is not
Transcribed Image Text:Consider the following reaction: A+B+C→D The rate law for this reaction is as follows: Rate=k[A][C]2[B]1/2 Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.13x10-2 M/s. What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? Rate 2= ? M/s (the answer is not 0.1566 M/s) (I've posted this question before and the answer is not
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