The reaction 2A = B is the second order reaction in A with a rate constant of 51/M × min at 24°C.
1. Starting with (A) initial= 0.0092 M, how long will it take in seconds for (A)final= 3.7 × 10^-3M?
First, we need to determine the time it takes for the concentration of A to decrease from 0.0092 M to 3.7 x 10^-3 M using the second-order rate equation:
1/[A]t - 1/[A]0 = kt
Solving for t:
1/(3.7 x 10^-3) - 1/(0.0092) = (51/M x min)t
270.27 - 108.7 = 51t
161.57 = 51t
t = 3.17 min
Now we need to convert minutes to seconds:
3.17 min x 60 sec/min = 190.2 sec
Therefore, it will take 190.2 seconds for the concentration of A to decrease from 0.0092 M to 3.7 x 10^-3 M.