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 0.30 M?

Question

Quizplus · Accepted Answer

The rate law for a first-order reaction is: rate = k[A], where k is the rate constant and [A] is the concentration of the reactant. The integrated rate law for a first-order reaction is: ln[A]t = -kt + ln[A]0, where [A]t is the concentration of the reactant at time t, [A]0 is the initial concentration of the reactant, and k is the rate constant. Substituting the given values into the integrated rate law, we get: ln[CH3NC]t = -(46 s-1)(0.20 min)(60 s/min) + ln(0.30 M) = -5.52. Solving for [CH3NC]t, we get: [CH3NC]t = 0.0027 M = 2.7 × 10-3 M.

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

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