Suppose a postulated mechanism does generate the experimental rate law, but the elementary steps, when added together, do not generate the balanced equation for the overall reaction. What can you say about the postulated mechanism?

Understanding the intricacies of chemical reactions is fundamental for students of chemistry, and the concept of elementary steps is a cornerstone in this knowledge collection. An elementary step in a reaction mechanism is, in essence, like a single stride taken by a runner in a marathon. Each step represents a distinct event on a molecular level, where reactants are directly transformed into products without any intermediate compounds.

Imagine watching a detailed slow-motion video of a chemical reaction. Each frame of that video that captures a single, indivisible chemical event would correspond to what chemists call an elementary step. These are the smallest divisions of a reaction mechanism and are vital because they provide insights into the actual reactants involved and the order of molecular events. If a proposed mechanism's elementary steps do not sum up to the overall balanced equation, this signals to us that we might be missing part of the action – perhaps an overlooked step or a misinterpretation of the process.

The experimental rate law is akin to a recipe that tells you how changing the amount of each ingredient affects the speed of your cooking – except here, the 'cooking' is a chemical reaction. Rate laws are determined through meticulous experiments, which measure how the rate of the reaction changes with varying concentrations of reactants.

In the realm of chemistry, correctly predicting the speed at which reactions occur is crucial, and this is where the experimental rate law shines. It contains powers (orders) of reactant concentrations, summarizing a wealth of experimental data into a mathematical relationship. Therefore, if a proposed mechanism predicts the experimental rate law accurately, it means one aspect of the mechanism is spot-on – it correctly captures how particles collide and react. However, it's also about matching the end result – the final balanced equation – which is why a mechanism's job isn't done until it accounts for both the journey (rate law) and destination (balanced equation).

A balanced chemical equation acts as both a scoreboard and a blueprint for a chemical reaction. It meticulously accounts for all the atoms participating in the reaction, ensuring that none are lost or gained in the process – after all, in chemistry, what goes in must come out. Balancing a chemical equation is not just a mathematical exercise; it reflects the fundamental law of conservation of mass.

Each reactant and product is represented with its corresponding chemical formula, and coefficients are adjusted so that the number of atoms of each element is the same on both sides of the equation. A postulated mechanism must ultimately yield a set of elementary steps that, when taken together, corroborate with the balanced equation provided for the overall reaction. If it does not, then the proposed mechanism is like a detective story that ends without revealing the culprit – it's incomplete and cannot be validated.

Chemical kinetics is a subfield of physical chemistry that deals with the speed or rate at which chemical reactions occur, and what factors influence this pace. It's a critical aspect of chemistry that answers not just the 'what' of a reaction occurring, but the 'how quickly' and 'under what conditions' as well. When studying chemical kinetics, you're delving into the narrative of a chemical reaction, from the first act where reactants meet, to the climax where they transform, and finally to the conclusion with products being formed.

Key parameters in kinetics include concentration, temperature, and the presence of catalysts or inhibitors. These elements can drastically change the speed of a reaction, revealing more about the underlying narrative – the mechanism. A true understanding of kinetics is not complete without connecting the dots between the experimental rate law and the balance of matter, as governed by the balanced chemical equation. When a proposed mechanism is being evaluated, one must ensure that it adheres to the principles of kinetics, striking harmony with both the experimental observations and the stoichiometry of the overall reaction.