The reaction A+B-> C+D rate=k[A][B]^2 has an initial rate of 0.0810 M/s. What will the initial rate be if [A] is halved and [B] is tripled? What will the initial rate be if [A] is tripled and [B] is halved?

Question

Chemistry

Bronson Peck

19 November, 20:49

The reaction A+B-> C+D rate=k[A][B]^2 has an initial rate of 0.0810 M/s. What will the initial rate be if [A] is halved and [B] is tripled? What will the initial rate be if [A] is tripled and [B] is halved?

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Answers (1)

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Vava · Answer 1

The first to do is to isolate the constant, k, to one side. The rate expression would then be:

k = rate / [A][B]^2

This constant, k, will be the same for the given reaction at a certain temperature. Then, we can relate a second rate to this reaction.

rate1 / [A1][B1]^2 = rate2 / [A2][B2]^2

First question:

0.0810 / [A1][B1]^2 = rate2 / [A2/2][3B2]^2

rate2 = (0.0810 [A2/2][3B2]^2) / [A1][B1]^2

rate2 = 0.3645 M/s

Second Equation:

0.0810 / [A1][B1]^2 = rate2 / [A2/2][3B2]^2

rate2 = (0.0810 [3A2][B2/2]^2) / [A1][B1]^2

rate2 = 0.0608 M/s