The rate law for the rearrangement of CH₃NC to CH₃CN at 800 K is rate = (1300 s^-1)[CH₃NC]. What is the half-life for this reaction?

Question

Quizplus · Accepted Answer

The half-life (t1/2) can be calculated using the following equation:

t1/2 = ln(2)/k

where k is the rate constant, which can be determined from the rate law:

rate = k[CHS1U1B13S1U1B0NC]

Plugging in the values given in the problem, we have:

k = rate/[CHS1U1B13S1U1B0NC] = (1300 sS1U1P1-1S1S1P0)/(0.01 M) = 1.3 × 10S1U1P1-4S1S1P0 sS1U1P1-1

Substituting k into the first equation, we get:

t1/2 = ln(2)/k = ln(2)/(1.3 × 10S1U1P1-4S1S1P0 sS1U1P1-1) = 5.3 × 10S1U1P1-4S1S1P0 s

Therefore, the correct answer is B.

The Rate Law for the Rearrangement of CH3NC to CH3CN