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The rate constant for the reaction is 0.130 M–1·s–1 at 200 °C. If the initial concentration...

The rate constant for the reaction is 0.130 M–1·s–1 at 200 °C. If the initial concentration of A is 0.00680M, what will be the concentration after 435s?

Solutions

Expert Solution

The units of the rate constant is M-1 s-1. Therefore it is a second order reaction

For a second order reaction:   2A products   or   A + B products   (when [A] = [B])    ,    rate = k[A]2

The integrated rate law is 1/[A] = kt + 1/[Ao]

Given, k = 0.130 M-1 s-1

  Ao= 0.00680 M

t = 435s

Therefore from the integrated rate law

1/[A] = (0.130 M-1 s-1)(435) + 1/(0.00680 M)

[A] = 0.00491 M

Therefore concentration after 435s is 0.00491M

queen_honey_blossom answered 2 years ago
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