The isomerization of methylisonitrile to acetonitrile CH₃NC (g) → CH₃CN (g)
Is first order in CH₃NC. The half life of the reaction is 5.20 × 10¹ s at 545 K. The rate constant when the initial [CH₃NC] is 0.030 M is __________ s^-1.

Question

Quizplus · Accepted Answer

The half-life of a first-order reaction is given by the following expression:

t1/2 = ln(2)/k

where k is the rate constant of the reaction.

From the given information, we know that:

t1/2 = 5.20 × 10^11 s 
[CH3NC]0 = 0.030 M

Plugging these values into the expression for t1/2, we can solve for k:

5.20 × 10^11 = ln(2)/k

k = ln(2)/(5.20 × 10^11) = 1.33 × 10^-12 s^-1

Therefore, the rate constant when [CH3NC]0 = 0.030 M is 1.33 × 10^-12 s^-1. The closest answer choice is C, 0.0133 s^-1.

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

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