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 mol L^-1?

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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.We can use this equation to calculate the concentration of CH3NC after 0.20 minutes:ln[CH3NC]t = -0.46 s-1 * (0.20 min * 60 s/min) + ln(0.30 mol L-1)ln[CH3NC]t = -5.52[CH3NC]t = 2.7 × 10-3 mol L-1

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

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