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25 September, 20:33

The rate constant for this second‑order reaction is 0.190 M - 1 ⋅ s - 1 0.190 M-1⋅s-1 at 300 ∘ C. 300 ∘C. A ⟶ products A⟶products How long, in seconds, would it take for the concentration of A A to decrease from 0.820 M 0.820 M to 0.340 M?

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  1. 25 September, 20:58
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    9.1 seconds

    Explanation:

    Given that for a second order reaction

    1/[A]t = kt + 1/[A]o

    Where [A]t = concentration at time = t = 0.340M

    [A]o = initial concentration = 0.820M

    k = rate constant for the reaction=0.190m-1s-1

    t = time taken for the reaction (the unknown)

    Hence;

    (0.340) ^-1 = 0.190*t + (0.820) ^-1

    t = (0.340) ^-1 - (0.820) ^-1/0.190

    t = 9.1 seconds

    Hence the time taken for the concentration to decrease from 0.840M to 0.340M is 9.1 seconds.
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