Consider this three-step mechanism for a reaction: Cl 2 (g) k 1 ⇌k 2 2 Cl (g) Fast Cl (g) + CHCl 3 (g) →k 3 HCl (g) + CCl 3 (g) Slow Cl (g) + CCl 3 (g) →k 4 CCl 4 (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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Tro 4th Edition

Ch.14 - Chemical Kinetics

Problem 77b

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Chapter 14, Problem 77b

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.

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Intermediates are species that are produced in one step of a reaction mechanism and consumed in a subsequent step.

Examine each step of the mechanism to identify species that are not present in the overall balanced equation.

In the first step, Cl2 dissociates into 2 Cl atoms.

In the second step, Cl reacts with CHCl3 to form HCl and CCl3.

In the third step, Cl reacts with CCl3 to form CCl4.

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Textbook Question

Consider this overall reaction, which is experimentally observed to be second order in AB and zero order in C: AB + C → A + BC Is the following mechanism valid for this reaction? AB + AB →k1 AB₂ + A Slow AB₂ + C → k2 AB + BC Fast

Consider this overall reaction, which is experimentally observed to be second order in X and first order in Y: X + Y → XY. a. Does the reaction occur in a single step in which X and Y collide? b. Is this two-step mechanism valid? 2X →k1/k2 X2 (Fast) X2 + Y →k3 XY + X (Slow)

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

a. What is the overall reaction?

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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

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

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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Consider this three-step mechanism for a reaction: Cl2 (g) k1⇌k2 2 Cl (g) FastCl (g) + CHCl3 (g) →k3 HCl (g) + CCl3 (g) SlowCl (g) + CCl3 (g) →k4 CCl4 (g) Fastb. Identify the intermediates in the mechanism.

Verified Solution

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.