Consider this two-step mechanism for a reaction: NO 2 (g) + Cl 2 (g) → k1 ClNO 2 (g) + Cl g) Slow NO 2 (g) + Cl(g) →k2 ClNO 2 (g) Fast b. Identify the intermediates in the mechanism.

Hi everyone here we have a question asking us to identify the intermediates in the mechanism A. Two forms A Fast A plus C. B forms C plus B. A. Slow and A plus B. A. Forms B A. Too fast. So let's see what we can cancel out here. We can cancel out A. We can cancel out B. A. So this gives us a two plus C. B Forms C Plus B. A. two. The intermediates are the species that are generated by one step and consumed by other steps. So in this case it is A N. B. A. And that is our final answer. Thank you for watching. Bye.

Ch.14 - Chemical Kinetics

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Ch.14 - Chemical Kinetics

Problem 78b

Chapter 14, Problem 78b

Consider this two-step mechanism for a reaction: NO₂(g) + Cl₂(g) → k1 ClNO₂(g) + Cl g) Slow NO₂(g) + Cl(g) →k2 ClNO₂(g) Fast b. Identify the intermediates in the mechanism.

Verified step by step guidance

Identify the overall reaction by adding the two elementary steps together.

Determine which species are produced in one step and consumed in another.

Recognize that intermediates are not present in the overall reaction but are formed and used up during the reaction mechanism.

Look at the first step: NO2(g) + Cl2(g) → ClNO2(g) + Cl(g). Notice that Cl(g) is produced.

Look at the second step: NO2(g) + Cl(g) → ClNO2(g). Notice that Cl(g) is consumed. Therefore, Cl(g) is an intermediate.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Reaction Mechanism

A reaction mechanism is a step-by-step description of the pathway taken by reactants to form products in a chemical reaction. It outlines the individual elementary steps, including the sequence of bond breaking and forming, and helps in understanding the overall reaction kinetics and dynamics.

Intermediates

Intermediates are species that are formed during the reaction mechanism but are not present in the final products. They are typically unstable and exist only transiently, playing a crucial role in the progression of the reaction from reactants to products.

Rate-Determining Step

The rate-determining step is the slowest step in a reaction mechanism, which limits the overall reaction rate. Understanding which step is rate-determining helps in predicting how changes in concentration or conditions will affect the speed of the reaction.

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Related Practice

Textbook Question

Consider this three-step mechanism for a reaction:

Cl₂ (g) k₁⇌k₂ 2 Cl (g) Fast

Cl (g) + CHCl₃ (g) →k₃ HCl (g) + CCl₃ (g) Slow

Cl (g) + CCl₃ (g) →k₄ CCl₄ (g) Fast

b. Identify the intermediates in the mechanism.

Textbook Question

Consider this three-step mechanism for a reaction:

Cl₂ (g) k₁⇌k₂ 2 Cl (g) Fast

Cl (g) + CHCl₃ (g) →k₃ HCl (g) + CCl₃ (g) Slow

Cl (g) + CCl₃ (g) →k₄ CCl₄ (g) Fast

c. What is the predicted rate law?

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Textbook Question

Many heterogeneous catalysts are deposited on high-surfacearea supports. Why?

Textbook Question

Suppose that the reaction A¡products is exothermic and has an activation barrier of 75 kJ/mol. Sketch an energy diagram showing the energy of the reaction as a function of the progress of the reaction. Draw a second energy curve showing the effect of a catalyst.

Consider this two-step mechanism for a reaction: NO2(g) + Cl2(g) → k1 ClNO2(g) + Cl g) Slow NO2(g) + Cl(g) →k2 ClNO2(g) Fast b. Identify the intermediates in the mechanism.

Verified video answer for a similar problem:

Key Concepts

Reaction Mechanism

Intermediates

Rate-Determining Step

Consider this two-step mechanism for a reaction: NO₂(g) + Cl₂(g) → k1 ClNO₂(g) + Cl g) Slow NO₂(g) + Cl(g) →k2 ClNO₂(g) Fast b. Identify the intermediates in the mechanism.