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

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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.

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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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Rate Law Determination

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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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Open Question

Consider this two-step mechanism for a reaction: Step 1: NO2(g) + Cl2(g) → ClNO2(g) + Cl(g) Slow Step 2: NO2(g) + Cl(g) → ClNO2(g) Fast c. What is the predicted rate law? a. What is the overall reaction?

Textbook Question

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

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.

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Open Question

Suppose that a catalyst lowers the activation barrier of a reaction from 125 kJ/mol to 55 kJ/mol. By what factor would you expect the reaction rate to increase at 25 °C? (Assume that the frequency factors for the catalyzed and uncatalyzed reactions are identical.)

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 Solution

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.