The isomerization of methylisonitrile to acetonitrile CH₃NC (g) → CH₃CN (g)
Is first order in CH₃NC. The rate constant for the reaction is 9.45 × 10^-5s^-1 at 478 K. The half-life of the reaction when the initial [CH₃NC] is 0.030 M is __________ s.

Question

Quizplus · Accepted Answer

The half-life of a first-order reaction can be calculated using the equation: 
t1/2 = ln(2) / k

where k is the rate constant.

We are given k = 9.45 × 10^-5s^-1 and an initial concentration of CH3NC of 0.030 M.

Plugging in the values, we get: 
t1/2 = ln(2) / k = ln(2) / 9.45 × 10^-5s^-1 = 7.33 × 10^-13 s

Therefore, the answer is choice D.

The Isomerization of Methylisonitrile to Acetonitrile CH3NC (G)→ CH3CN (G)

The Isomerization of Methylisonitrile to Acetonitrile CH₃NC (G)→ CH₃CN (G)