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Chapter 7: Problem 68

A three-step mechanism has been suggested for the formation of carbonyl chloride: Step I: \(\mathrm{Cl}_{2} \rightarrow 2 \mathrm{Cl}\) Step II: \(\mathrm{Cl}+\mathrm{CO} \rightarrow \mathrm{COCl}\) Step III: \(\mathrm{COCl}+\mathrm{Cl}_{2} \rightarrow \mathrm{COCl}_{2}+\mathrm{Cl}\) Which species is an intermediate in the mechanism? a. \(\mathrm{COCl}_{2}\) b. \(\mathrm{COCl}\) c. \(\mathrm{Cl}\) d

Short Answer

Expert verified
\(\mathrm{COCl}\) is the intermediate in the mechanism.

Step by step solution

01

Identify the Definition

An intermediate is a species that is generated in one step of a reaction mechanism and consumed in a subsequent step. It does not appear in the overall balanced equation for the reaction.
02

Analyze Each Step

Examine each step to identify which species fits the definition of an intermediate. In Step I, \(\mathrm{Cl}_{2} \rightarrow 2 \mathrm{Cl}\), chlorine radicals (\(\mathrm{Cl}\)) are produced. In Step II, \(\mathrm{Cl}+\mathrm{CO} \rightarrow \mathrm{COCl}\), chlorine is used, and \(\mathrm{COCl}\) is produced. In Step III, \(\mathrm{COCl}\) reacts with \(\mathrm{Cl}_{2}\) to form \(\mathrm{COCl}_{2}\) and releases \(\mathrm{Cl}\).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Carbonyl Chloride Formation
Carbonyl chloride, also known as phosgene, is represented by the chemical formula \( \text{COCl}_2 \). It is an essential compound, especially in the chemical industry, and is formed through a multistep reaction mechanism. Let's break down the general idea of this formation process for better understanding.

The formation of carbonyl chloride from chlorine (\( \text{Cl}_2 \)) and carbon monoxide (\( \text{CO} \)) involves three major steps:
  • Step I: The dissociation of chlorine molecules into chlorine radicals, represented as \( \text{Cl}_2 \rightarrow 2 \text{Cl} \). This step requires energy to break the bond and produce reactive chlorine atoms.
  • Step II: The chlorine radicals then react with carbon monoxide to form carbonyl chloride radicals, \( \text{Cl} + \text{CO} \rightarrow \text{COCl} \). This step showcases the reactivity of radical species.
  • Step III: The carbonyl chloride radicals further react with chlorine molecules to yield the complete carbonyl chloride, \( \text{COCl} + \text{Cl}_2 \rightarrow \text{COCl}_2 + \text{Cl} \), and chlorine radicals are regenerated, continuing the cycle.
Understanding these steps is crucial since they provide insights into the reaction dynamics and conditions necessary for synthesizing \( \text{COCl}_2 \).
Intermediate Species in Reactions
In chemical reactions, intermediate species play a pivotal role in the mechanism without appearing in the final balanced equation. Identifying these intermediates can deepen your understanding of reaction pathways.

An intermediate is a transient species, often short-lived, appearing in the middle of the reaction but disappearing by the end. In the carbonyl chloride formation:
  • Chlorine Radicals \( (\text{Cl}) \): These are produced in the first step and consumed in subsequent steps, but not an intermediate since they reappear in the final step, playing indirect roles.
  • Carbonyl Chloride Radicals \( (\text{COCl}) \): These species are produced in the second step and react in the third, not appearing in the final product. Hence, \( \text{COCl} \) is the true intermediate here, as it fulfills the criteria of being produced in one step and consumed in the next, with no presence in the final reaction result.
Identifying intermediates helps chemists to manipulate and optimize reaction conditions, improving yields and efficiency in industrial applications.
Stepwise Reaction Process
Understanding stepwise reaction processes is crucial as it helps in deciphering each reaction stage. Each step showcases the transformation of reactants into products through different intermediates or transient species.

A stepwise reaction means that the transformation from reactants to products does not occur in a single jump but involves a sequence of individual stages:
  • Stepwise Dynamics: Each step is characterized by its distinct pathway and species transitions. It allows scientists to monitor how each component contributes to the eventual goal.
  • Energy Consideration: Steps may require varying energy inputs or releases, affecting the conditions such as temperature or catalysts needed for reactions.
  • Mechanism Analysis: By breaking down into steps, chemists can pinpoint reaction bottlenecks or slow stages which may need acceleration for an effective overall process.
The carbonyl chloride formation is a perfect example, where each step strategically navigates through radicals and intermediates to reach stability with the final product, ensuring a deeper comprehension of such step-by-step processes helps in effortlessly understanding complex chemical reactions.

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Most popular questions from this chapter

Which of the following statements are correct? (1) Order of a reaction can be known from experimental results and not from the stoichiometry of reaction. (2) Molecularity a reaction refers to (i) each of the elementary steps in (an overall mechanism of) a complex reaction or (ii) a single step reaction (3) Overall molecularity of a reaction may be determined in a manner similar to overall order of reaction(4) Overall order of a reaction \(\mathrm{A}^{\mathrm{m}}+\mathrm{B}^{\mathrm{n}} \rightarrow \mathrm{AB}_{\mathrm{x}}\) is \(\mathrm{m}+\mathrm{n} .\) Select the correct answer using the following codes: a. 2 and 3 b. 1,3 and 4 c. 2,3 and 4 d. 1,2 and 3

(A): For the hydrogen halogen photochemical reaction, the quantum yield for the formation of \(\mathrm{HBr}\), is lower than that of \(\mathrm{HCl}\). (R): \(\mathrm{Br}+\mathrm{H}_{2} \rightarrow \mathrm{HBr}+\mathrm{H}\) has higher activation energy than \(\mathrm{Cl}+\mathrm{H}_{2} \rightarrow \mathrm{HCl}+\mathrm{H}\)

Consider a reaction \(\mathrm{aG}+\mathrm{bH} \rightarrow\) Products. When concentration of both the reactants \(\mathrm{G}\) and \(\mathrm{H}\) is doubled, the rate increases by eight times. However when concentration of \(\mathrm{G}\) is doubled keeping the concentration of \(\mathrm{H}\) fixed, the rate is doubled. The overall order of the reaction is a. 0 b. 1 c. 2 d. 3

The basic theory behind Arrhenius's equation is that a. The activation energy and pre-exponential factor are always temperature- independent b. The rate constant is a function of temperature c. The number of effective collisions is proportional to the number of molecules above a certain threshold energy d. As the temperature increases, so does the number of molecules with energies exceeding the threshold energy.

A mechanism for a naturally occurring reaction that destroys ozone is: Step I: \(\mathrm{O}_{3}(\mathrm{~g})+\mathrm{HO}(\mathrm{g}) \rightarrow \mathrm{HO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g})\) Step II: \(\mathrm{HO}_{2}(\mathrm{~g})+\mathrm{O}(\mathrm{g}) \rightarrow \mathrm{HO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g})\) Which species is a catalyst? a. \(\mathrm{O}\) b. \(\mathrm{O}_{3}\) c. \(\mathrm{HO}_{2}\) d. HO
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