What is the value of k for this reaction?

Question

You have been studying the reaction:

A(g) + 2 B(g) --> C(l)

And have determined that the reaction is 2nd order with respect to A and 0th order with respect to B. As part of your experiment, you performed a trial in which [A]initial= 0.309M and [B]initial= 0.573M in which you found the initial rate to be 0.0255 M/min. What is the value of k for this reaction?

Answer 1

A(g) + 2B(g) ==> C(l)

Since it is 2nd order in A and zero order in B, we can write the rate equation as ...

rate = k[A]²

Substituting values obtained from the experiment, we can solve for the rate constant (k)

0.0255 M/min = [0.309 M]² k

k = 0.0255 M/min / 0.09548 M²

k = 0.267 M^-1min^-1