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.

검증된 단계별 안내

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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주요 개념

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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.

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.