The reaction A + B ⟶ C + D rate = k [ A ] [ B ] 2 A+B⟶C+Drate=k[A][B]2 has an initial rate of 0.0640 M / s. 0.0640 M/s. What will the initial rate be if [ A ] [A] is halved and [ B ] [B] is tripled?What will the initial rate be if [A] is tripled and [B] is halved? answer M/s

Answer :

(1) The initial rate when [A] is halved and [B] is tripled is, 0.288 M/s

(2) The initial rate when [A] is tripled and [B] is halved is, 0.096 M/s

Explanation:

The given rate law expression is:

Now we have to determine the initial rate when [A] is halved and [B] is tripled.

The new rate law expression will be:

Given:

Initial rate = 0.0640 M/s

As, Initial rate = = 0.0640 M/s

Thus,

Now we have to determine the initial rate when [A] is tripled and [B] is halved.

The new rate law expression will be:

Given:

Initial rate = 0.0640 M/s

As, Initial rate = = 0.0640 M/s

Thus,

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