The isomerization reaction,CH₃NC → CH₃CN,is first order and the rate constant is equal to 0.46 s^-1 at 600 K.What is the concentration of CH₃NC after 0.20 minutes if the initial concentration is 0.10 M?

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The integrated rate law for a first-order reaction is:ln[A]t=−kt+ln[A]0where [A]t is the concentration of the reactant at time t, k is the rate constant, and [A]0 is the initial concentration of the reactant.Substituting the given values into the integrated rate law, we get:ln[CH3NC]t=−(0.46s−1)(0.20min)(60smin)+ln(0.10M)ln[CH3NC]t=−5.52+ln(0.10M)ln[CH3NC]t=−4.62[CH3NC]t=e−4.62=4.0×10−4M

The Isomerization Reaction,CH3NC → CH3CN,is First Order and the Rate

The Isomerization Reaction,CH₃NC → CH₃CN,is First Order and the Rate