Consider the reaction.
Kinetics studies reveal a first-order rate dependence on the concentration of
the \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{C}-\mathrm{Br}\) and a zero-order
dependence on the concentration of \(\mathrm{H}_{2} \mathrm{O}\).
(a) What happens to the reaction rate as the \(\left(\mathrm{CH}_{3}\right)_{3}
\mathrm{C}-\mathrm{Br}\) concentration is changed? What happens to the reaction
rate as the \(\mathrm{H}_{2} \mathrm{O}\) concentration is changed?
(b) Two mechanisms for this reaction are offered below. Can you rule out
either of them? Is either mechanism plausible, given the overall balanced
equation and kinetic data? Explain your answer fully.