Question

For the following reaction
$(C{H}_3{)}_{3}CCl+H_{2}O\to (C{H}_3{)}_{3}COH+HCl\left(\frac{dx}{dt}\right)=k\left[\right(C{H}_3{)}_{3}CCl]$

the rate determining step is:

• A. $(C{H}_3{)}_{3}CCl\to (C{H}_3{)}_3{C}^{⨁}+C{l}^{-}$
• B. $(C{H}_3{)}_{3}CCl+H_{2}O\to (C{H}_3{)}_{3}COH+HCl$
• C. $(C{H}_3{)}_3{C}^{⨁}+H_{2}O\to (C{H}_3{)}_{3}COH+H^{+}$
• D. $H^{+}+C{l}^{-}\to HCl$

Answer 1

The correct option is A $(C{H}_3{)}_{3}CCl\to (C{H}_3{)}_3{C}^{⨁}+C{l}^{-}$

$\frac{dx}{dt}=k\left[\right(C{H}_3{)}_{3}CCl]$

So formation of carbocation from $C{H}_3{)}_{3}CCl$ is rate determining step, since rate of reaction depends on concentration of ($C{H}_3{)}_{3}CCl$