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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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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.

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.

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.

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