For the reaction CC(C)(C)COCC(C)(C)O the rate law is Identify each mechanism th

step 1 For this question, we have a chemical reaction of CH3CBR with hydroxide, forming CH3 COH, and BR

For the reaction <smiles>CC(C)(C)COCC(C)(C)O</smiles> the...

For the reaction <smiles>CC(C)(C)COCC(C)(C)O</smiles> the rate law is Identify each mechanism that is compatible with the rate law. (a) $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr} \longrightarrow\left(\mathrm{CH}_{3}\right)_{3} \mathrm{C}^{+}+\mathrm{Br}^{-}$ slow $$ \left(\mathrm{CH}_{3}\right)_{3} \mathrm{C}^{+}+\mathrm{OH}^{-} \longrightarrow\left(\mathrm{CH}_{3}\right)_{3} \mathrm{COH} $$ fast (b) $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}+\mathrm{OH}^{-} \longrightarrow\left(\mathrm{CH}_{3}\right)_{3} \mathrm{COH}+\mathrm{Br}^{-}$ (c) $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}+\mathrm{OH}^{-} \longrightarrow\left(\mathrm{CH}_{3}\right)_{2}\left(\mathrm{CH}_{2}\right) \mathrm{CBr}^{-}+\mathrm{H}_{2} \mathrm{O}$ fast $\left(\mathrm{CH}_{3}\right)_{2}\left(\mathrm{CH}_{2}\right) \mathrm{CBr}^{-} \longrightarrow\left(\mathrm{CH}_{3}\right)_{2}\left(\mathrm{CH}_{2}\right) \mathrm{C}+\mathrm{Br}^{-}$ slow $$ \left(\mathrm{CH}_{3}\right)_{2}\left(\mathrm{CH}_{2}\right) \mathrm{C}+\mathrm{H}_{2} \mathrm{O} \longrightarrow\left(\mathrm{CH}_{3}\right)_{3} \mathrm{COH} $$ fast

For the reaction
<smiles>CC(C)(C)COCC(C)(C)O</smiles>
the rate law is
Identify each mechanism that is compatible with the rate law.
(a) $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr} \longrightarrow\left(\mathrm{CH}_{3}\right)_{3} \mathrm{C}^{+}+\mathrm{Br}^{-}$
slow
$$
\left(\mathrm{CH}_{3}\right)_{3} \mathrm{C}^{+}+\mathrm{OH}^{-} \longrightarrow\left(\mathrm{CH}_{3}\right)_{3} \mathrm{COH}
$$
fast
(b) $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}+\mathrm{OH}^{-} \longrightarrow\left(\mathrm{CH}_{3}\right)_{3} \mathrm{COH}+\mathrm{Br}^{-}$
(c) $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}+\mathrm{OH}^{-} \longrightarrow\left(\mathrm{CH}_{3}\right)_{2}\left(\mathrm{CH}_{2}\right) \mathrm{CBr}^{-}+\mathrm{H}_{2} \mathrm{O}$ fast
$\left(\mathrm{CH}_{3}\right)_{2}\left(\mathrm{CH}_{2}\right) \mathrm{CBr}^{-} \longrightarrow\left(\mathrm{CH}_{3}\right)_{2}\left(\mathrm{CH}_{2}\right) \mathrm{C}+\mathrm{Br}^{-}$
slow
$$
\left(\mathrm{CH}_{3}\right)_{2}\left(\mathrm{CH}_{2}\right) \mathrm{C}+\mathrm{H}_{2} \mathrm{O} \longrightarrow\left(\mathrm{CH}_{3}\right)_{3} \mathrm{COH}
$$
fast

Key Concepts

SN1 Mechanism

An SN1 mechanism is a unimolecular nucleophilic substitution process where the first step involves dissociation of the substrate to form a carbocation intermediate. This formation of the carbocation, being the slow, rate?determining step, leads to a rate law that depends solely on the concentration of the substrate.

Rate?Determining Step

The rate?determining step (RDS) is the slowest step in a reaction mechanism, and it controls the overall rate of the reaction. The rate law is directly related to the molecularity and kinetics of this step, so identifying the RDS is crucial in understanding and predicting the reaction’s behavior.

SN2 Mechanism

An SN2 mechanism is a bimolecular nucleophilic substitution process that takes place in one concerted step, where bond formation and bond breaking occur simultaneously. The rate of an SN2 reaction depends on both the substrate and the nucleophile concentrations, and it is characterized by a highly sensitive steric environment affecting the reaction rate.

Rate Law

The rate law is an expression that defines how the rate of a chemical reaction depends on the concentrations of its reactants. Its form, determined experimentally, can provide insights into the reaction mechanism by indicating which species’ concentrations affect the reaction rate.

Reaction Mechanism

A reaction mechanism is a detailed sequence of elementary steps that describes the pathway from reactants to products. Analyzing the mechanism helps correlate individual steps to the overall rate law, revealing which step limits the speed of the reaction.

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