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Using the given data, calculate the rate constant of this reaction.?

Using the given data, calculate the rate constant of this reaction.

Trial [A] (M) [B] (M) Rate (M/s)

1 0.350 0.250 0.0222

2 0.350 0.675 0.162

3 0.560 0.250 0.0355

A+B ---> C+D

k= ?

How do you solve this question?

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This is the best answer for Using the given data, calculate the rate constant of this reaction.?

Comparing Trial 1 to Trial 3, [A] was increased by a factor of (0.560 M) / (0.350 M) = 1.600. In response, the initial rate of the reaction increased by a factor of (0.0355 M/s) / (0.0222 M/s) = 1.599. This is close enough to say the the rate law is first order with respect to A.

Comparing Trial 1 to Trial 2, [B] was increased by a factor of (0.675 M) / (0.250 M) = 2.7. In response, the initial rate of the reaction increased by a factor of (0.162 M/s) / (0.0222 M/s) = 7.297. It turns out that 2.7^2 = 7.29; this is close enough to say the the rate law is second order with respect to B.

The overall rate law is then

Rate = k[A][B]^2.

Now substitute all the data from any of the three experiments to find k. I'll choose Trial 1:

0.0222 M/s = k (0.350 M) (0.25 M)^2;

Solving, k = 1.0149 M^-2s^-1.

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