When the reaction is run in a buffer solution, however, it is pseudo-first-order in CH3I.

rate = k[CH3]

What is the half-life of this reaction in a pH 10.00 buffer if the pseudo-first-order rate constant for this reaction is 7.3 x10-9 s-1?

To determine the half-life of a pseudo-first-order reaction in a buffer solution, we need to use the rate constant (k) provided and the formula for half-life.

The formula for the half-life (t1/2) in a pseudo-first-order reaction is:

t1/2 = (0.693 / k)

Given that the rate constant (k) for the reaction is 7.3 x 10^(-9) s^(-1), we can substitute it into the formula to find the half-life.

t1/2 = (0.693 / 7.3 x 10^(-9))

To simplify the calculation, let's express 0.693 as a fraction.

t1/2 = (1 / 1.4427 x 10^(-8))

Now, we can divide 1 by the value of 1.4427 x 10^(-8).

t1/2 ≈ 6.9308 x 10^7 seconds

The half-life of the reaction in a pH 10.00 buffer is approximately 6.9308 x 10^7 seconds.