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?

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. We can use this equation to calculate the concentration of CH3NC after 0.20 minutes if the initial concentration is 0.10 M.ln[CH3NC]t = -k*t + ln[CH3NC]0ln[CH3NC]t = -(46 s^-1)*(0.20 min)*(60 s/min) + ln(0.10 M)ln[CH3NC]t = -5.52[CH3NC]t = 0.004 MTherefore, the concentration of CH3NC after 0.20 minutes if the initial concentration is 0.10 M is 0.004 M.

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

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