# [SOLVED] Using the given data, calculate the rate constant of this reaction.?

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?

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.