The reaction CH₃-N≡C → CH₃-C≡N
Is a first-order reaction. At 230.3 °C, k = 6.29 × 10^-⁴s^-1. If [CH₃-NC] is 1.00 × 10^-³ initially, [CH₃-NC] is __________ after 1.000 × 10³ s.

Question

Quizplus · Accepted Answer

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(1.00 × 10^-3) = -(6.29 × 10^-4 s^-1)(1.000 × 10^3 s) + ln[CH3-N≡C]0Solving for [CH3-N≡C]0, we get:[CH3-N≡C]0 = 5.33 × 10^-4

The Reaction CH3-N≡C → CH3-C≡N

The Reaction CH₃-N≡C → CH₃-C≡N