2A → B + C
The above reaction is run and found to follow second order kinetics with a rate constant of 1.30 x 10-3 M-1sec-1. If the initial concentration of A is 1.45 M, what is the concentration after 142 seconds?
Since the reaction is second order and we have to find final concentration after 142 second, we can use integrated rate equation for the second order.
1/[A]t = kt + 1/ [A]0
Here subscript t and 0 are shown for concentration at time t and present initially respectively.
k is rate constant and t is time.
Lets plug in the given values in order to get [A]t
1/[A]t = (1.30 E-3 per M per s x 142 s ) + 1/ 1.45 M
We have to calculate value of [A]t
[A]t= 1.14 M
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