The reaction ch3nc - > ch3cn is first order. it takes 156 seconds for the concentration of reactant to fall from 0.100 m to 0.0500 m. how much time would it take for the concentration of reactant to fall from 0.0500 m to 0.0400 m?

Answers (1)
  1. Kherington
    Reaction of interest is: CH3NC → CH3CN

    Given: Reaction obeys 1st order kinetics

    Also, it takes 156 s for the concentration of reactant to fall from 0.100 m to 0.0500 m. Hence, half life of reaction (t1/2) is 156 s.

    We know that, for 1st order reaction:

    k = 0.693 / t (1/2)

    = 0.693 / 156

    = 0.0044 s-1

    We also know that, for 1st order reaction

    t = 2.303/k log (initial conc. / final conc.)

    ∴ Time required for the conc. of reactant to fall from 0.05 m to 0.04 m = 2.303/k log (initial conc. / final conc.)

    = 2.303/0.0044 log (0.05/0.04)

    = 50.72 s.
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