Write the overall reaction for the mechanism proposed below and identify any reaction intermediates. $$ \begin{aligned} &\text { Step } 1 \mathrm{AC}+\mathrm{B} \longrightarrow \mathrm{AB}+\mathrm{C} \\ &\text { Step } 2 \mathrm{AC}+\mathrm{AB} \longrightarrow \mathrm{A}_{2} \mathrm{~B}+\mathrm{C} \end{aligned} $$

In chemical reactions, some species are created and consumed within the process without appearing in the final overall equation. These species are known as reaction intermediates. Identifying these intermediates is key to understanding the reaction mechanism and simplifying complex reactions into more understandable steps.

Let's consider a simplified example where two steps are involved in a reaction mechanism. In the first step, compound AC reacts with B to form AB and C. In the second step, compound AC reacts with the newly formed AB to yield A₂B and another molecule of C.

When we break down this mechanism, we see that both AC and AB are created and then consumed—they don't appear in the final products or reactants. Consequently, AC and AB are reaction intermediates. By recognizing these, we can focus on the substances that are truly altered from reactants to products, which is crucial for understanding the overall chemical change that has occurred.

The study of the rate at which chemical reactions occur and the factors that affect these rates is known as chemical kinetics. In kinetics, we are not only concerned with the end result of a reaction but also the 'path' taken to arrive there and how fast the reaction progresses.

In our example, the formation of AB from AC and B (Step 1), and then the reaction of AC with AB to form A₂B (Step 2) will each have their own rate, determined by the reaction conditions such as temperature, pressure, and the presence of a catalyst. The intermediates play a vital role in kinetics since they can significantly influence the rate of the overall reaction. Understanding the role of intermediates can help chemists design reactions to proceed faster or slower, as needed for industrial or laboratory applications. Therefore, it is not just about whether the reactions occur, but how efficiently they do so, which is integral to the study and application of chemical kinetics.

The overall reaction is the simplified form of a reaction mechanism that shows only the starting reactants and the final products, excluding all the intermediates. In our given exercise, the overall reaction is found by adding together the steps of the mechanism and canceling out intermediates and any other species that appear on both sides.

By canceling out the intermediates AC and AB which are formed and used up within the reaction sequence, and acknowledging that C is a product in both steps and thus cancels itself out, the remaining reactants and products can be combined. The result is the overall reaction that provides a macroscopic perspective of the chemical change taking place.

This simplified reaction is what would be typically written in a chemical equation representing the process and is fundamental to understanding how a set of reactants is transformed into a set of products without needing to consider the more complex pathway of steps and intermediates.