## THIS USER ASKED 👇

**Consider the rate constants below. which would correspond to the highest order reaction? k = 8.79 x 102 ms–1 k = 4.46 x 10–1 m–1s–1 k = 2.35 x 106 s–1 k = 1.88 x 10–3 m–2s–1**

## THIS IS THE BEST ANSWER 👇

When determining this formula the order n of the reaction rate:

rate = K * [A]^ n

when we have the rate unit MS ^ -1

and unit [A] M.

So:

1- for k = 8.79 x 10 ^ 2 MS ^ -1:

where MS ^ -1 is the unit of K here

by substitution in rate formula:

MS ^ -1 = MS ^ -1 * M ^ n

∴ M ^ n = 1

∴M ^ 0 = 1

∴ zero reaction of this reaction rate

2- when k = 4.46 x 10 ^ -1 with unit M-1 S-1:

by substitution in rate formula:

MS ^ -1 = M-1 S-1 * M ^ n

∴M ^ 2 = M ^ n

∴n = 2 so this is the second reaction

3- where K is 2.35 x 10 ^ 6 and its unit is S-1:

So by substituting in a rate formula:

MS ^ -1 = S ^ -1 * M ^ n

∴ M ^ n = M.

∴ n = 1

So this is the first order reaction

4- when k = 1.88 x 10 ^ -3 and its unit M-2 S-1

by substitution in rate formula:

MS ^ -1 = M ^ -2 S ^ -1 * M ^ n

∴ M ^ n = M ^ 3

∴ n = 3

∴ This is a third-order reaction

from 1 & 2 & 3 & 4

so that we see that (4) is the correct answer, the highest reaction in the order is K = 1.88 x 10 ^ -3 M-2 S-1.

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