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Ch.15 - Chemical Kinetics
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.15 - Chemical KineticsProblema 81
Capitolo 15, Problema 81

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

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Identify the overall reaction: AB + C \(\rightarrow\) A + BC.
Determine the rate law from the given information: The reaction is second order in AB and zero order in C, so the rate law is rate = k[AB]^2.
Examine the proposed mechanism: Step 1: AB + AB \(\xrightarrow{k_1}\) AB_2 + A (Slow), Step 2: AB_2 + C \(\xrightarrow{k_2}\) AB + BC (Fast).
Identify the rate-determining step: The slow step (Step 1) is the rate-determining step, so the rate law should be based on this step.
Check if the rate law from the mechanism matches the experimental rate law: The rate of the slow step is rate = k_1[AB]^2, which matches the experimental rate law, confirming the mechanism is valid.

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Reaction Order

Reaction order refers to the power to which the concentration of a reactant is raised in the rate law of a chemical reaction. In this case, the reaction is second order in AB, meaning that the rate of reaction is proportional to the square of the concentration of AB. Understanding reaction order is crucial for analyzing how changes in concentration affect the rate of the reaction.
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Average Bond Order

Rate Law

The rate law expresses the relationship between the rate of a chemical reaction and the concentration of its reactants. For the given reaction, the rate law can be written as rate = k[AB]^2[C]^0, indicating that the rate depends only on the concentration of AB. This concept is essential for determining whether a proposed mechanism is consistent with the observed reaction order.
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Rate Law Fundamentals

Elementary Steps in Reaction Mechanisms

Elementary steps are the individual steps that make up a reaction mechanism, each representing a single molecular event. The validity of a proposed mechanism can be assessed by ensuring that the slowest step (rate-determining step) aligns with the overall reaction order. In this case, the first step is slow and should reflect the second-order dependence on AB, while the second step must not affect the overall order with respect to C.
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Reaction Mechanism Overview
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Which of these two reactions would you expect to have the smaller orientation factor? Explain. a. O(g) + N2(g) → NO( g) + N(g) b. NO(g) + Cl2(g) → NOCl( g) + Cl(g)

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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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Consider these two gas-phase reactions: a. AA(g) + BB(g) → 2 AB(g) b. AB(g) + CD(g) → AC(g) + BD(g) If the reactions have identical activation barriers and are carried out under the same conditions, which one would you expect to have the faster rate?

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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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