The rate constant for a certain reaction is k = 5.30×10−3 s −1 . If the initial reactant concentration was 0.900 M , what will the concentration be after 13.0 minutes?
The rate constant for a certain reaction is k = 5.30×10−3 s −1 . If the initial reactant concentration was 0.900 M , what will the concentration be after 13.0 minutes?
Solution
Unit of rate constant shows that reaction is first order.
First order integrated rate equation
Ln ([A]t/[A]0) = - kt
Here At and A0 are the concentrations at time t and initial concentration respectively.
k is rate constant , t is the time.
Lets plug given values to get the At
ln ( [A]t / 0.900 ) = - 5.30 E-3 x 13.0 x 60 x
take exp of both side
[A]t/0.900 = exp ( -5.30 E-3 x 13.0 x 60 )
[A]t = 0.01442 M
So the concentration at time 13.0 minute = 0.0144 M
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