Question

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^{-1}sec^{-1}. If the initial concentration of A
is 1.45 M, what is the concentration after 142 seconds?

Answer #1

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.

Equation:

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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