The following data were obtained for the reaction of (CH3)3 CBr with hydroxide ion at 55^∘ C. (C

Name: Problem 65, Chapter 14: Chemistry The Molecular Nature of Matter
Uploaded: 2022-01-10T21:12:44-08:00
Duration: 1 min 37 s
Channel: Crystal Wang
Description: The following data were obtained for the reaction of (CH3)3 CBr with hydroxide ion at 55^∘ C. (CH3)3 CBr+OH^- ⟶(CH3)3 COH+Br^- What is the rate law for the reaction? What is the value of the rate constant (with correct units) at this temperature?

step 1 So in this problem, we're given the data for the reaction and we want to find the rate loss. So

Question

The following data were obtained for the reaction of $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}$ with hydroxide ion at $55^{\circ} \mathrm{C}$. $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}+\mathrm{OH}^{-} \longrightarrow\left(\mathrm{CH}_{3}\right)_{3} \mathrm{COH}+\mathrm{Br}^{-}$ What is the rate law for the reaction? What is the value of the rate constant (with correct units) at this temperature?

   The following data were obtained for the reaction of $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}$ with hydroxide ion at $55^{\circ} \mathrm{C}$.
$\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}+\mathrm{OH}^{-} \longrightarrow\left(\mathrm{CH}_{3}\right)_{3} \mathrm{COH}+\mathrm{Br}^{-}$
What is the rate law for the reaction? What is the value of the rate constant (with correct units) at this temperature?

Chemistry The Molecular Nature of Matter

Neil D. Jespersen,… 6th Edition

Chapter 14, Problem 65

Instant Answer

Solved by Expert Crystal Wang

01/10/2022

Step 1

The concentration of $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}$ changes from 0.19 M to 0.46 M, which is a factor of $\frac{0.46}{0.19} = 2.42105$. The rate of reaction changes from $1.0 \times 10^{-3}$ M/s to $2.4 \times 10^{-3}$ M/s, which is a factor of Show more…

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The following data were obtained for the reaction of $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}$ with hydroxide ion at $55^{\circ} \mathrm{C}$. $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}+\mathrm{OH}^{-} \longrightarrow\left(\mathrm{CH}_{3}\right)_{3} \mathrm{COH}+\mathrm{Br}^{-}$ What is the rate law for the reaction? What is the value of the rate constant (with correct units) at this temperature?

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Key Concepts

SN1 Reaction Mechanism

Many tertiary alkyl halides react with nucleophiles via an SN1 mechanism. In this pathway, the slow, rate-determining step is the ionization of the substrate to form a carbocation intermediate after the leaving group departs. As a result, the reaction rate is independent of the concentration of the nucleophile.

Unimolecular Rate Law

In reactions that proceed via the SN1 mechanism, the rate law depends solely on the concentration of the substrate because the formation of the carbocation is the rate?determining step. Thus, the rate law is expressed as rate = k[substrate], where only the concentration of the tertiary alkyl halide appears.

Rate Constant and Its Units

For a first-order (unimolecular) reaction such as an SN1 reaction, the rate constant (k) has units of inverse seconds (s?¹). The actual numerical value of k is determined experimentally by measuring reaction rates under various conditions and applying the rate law.

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