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Chapter 14: Problem 46

Which of these species cannot be isolated in a reaction: activated complex, product, intermediate?

Short Answer

Expert verified
The species that cannot be isolated in a reaction is the activated complex.

Step by step solution

01

Understanding Activated Complex

An activated complex, also known as the transition state, represents the highest potential energy along the reaction path. It is the state corresponding to the highest energy along the reaction coordinate and is not stable. It cannot be isolated because it is so highly reactive and exists for a very brief moment during a reaction. So, the activated complex cannot be isolated.
02

Understanding Product of a Reaction

Product(s) are the substance(s) which are formed after the completion of a chemical reaction. They exist at the end of a reaction and as they are stable, they can be isolated.
03

Understanding Intermediate

An intermediate is a molecular entity that forms as a reaction progresses, and its concentration will go to a maximum and then decrease. While they are more stable than an activated complex, they are usually still highly reactive and exist only for a brief period during a reaction. However, under very specific conditions, some intermediates may be isolated.

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Most popular questions from this chapter

When methyl phosphate is heated in acid solution, it reacts with water: $$ \mathrm{CH}_{3} \mathrm{OPO}_{3} \mathrm{H}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{CH}_{3} \mathrm{OH}+\mathrm{H}_{3} \mathrm{PO}_{4} $$ If the reaction is carried out in water enriched with \({ }^{18} \mathrm{O}\), the oxygen- 18 isotope is found in the phosphoric acid product but not in the methanol. What does this tell us about the bond-breaking scheme in the reaction?

A certain first-order reaction is 35.5 percent complete in 4.90 min at \(25^{\circ} \mathrm{C}\). What is its rate constant?

Distinguish between homogeneous catalysis and heterogeneous catalysis. Describe some important industrial processes that utilize heterogeneous catalysis.

The rate law for the reaction $$ 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NOCl}(g) $$ is given by rate \(=k[\mathrm{NO}]\left[\mathrm{Cl}_{2}\right]\). (a) What is the order of the reaction? (b) A mechanism involving these steps has been proposed for the reaction $$ \begin{aligned} \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) & \longrightarrow \mathrm{NOCl}_{2}(g) \\ \mathrm{NOCl}_{2}(g)+\mathrm{NO}(g) \longrightarrow & 2 \mathrm{NOCl}(g) \end{aligned} $$ If this mechanism is correct, what does it imply about the relative rates of these two steps?

Given the same concentrations, the reaction $$ \mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{COCl}_{2}(g) $$ at \(250^{\circ} \mathrm{C}\) is \(1.50 \times 10^{3}\) times as fast as the same reaction at \(150^{\circ} \mathrm{C}\). Calculate the energy of activation for this reaction. Assume that the frequency factor is constant.
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