Sketch a graph showing how the concentrations of the reactant \(A\) and product \(P\) of a typical chemical reaction \((A \rightleftharpoons P)\) vary with time during the course of the reaction. Assume that no products are present at the start of the reaction. Indicate on the graph where the system has reached equilibrium.

Chemical kinetics is the branch of chemistry that studies the rates of chemical reactions and the mechanisms by which they occur. Think of it as the step-by-step playbook detailing how molecules interact to form new products over time. It is a core concept in understanding the dynamic progression of reactions.
In the context of our exercise, we look at how the concentration of reactant A declines and how product P forms with time. Kinetics would not only consider the rates at these changes occur but also the factors that influence these rates, such as temperature, catalysts, and the concentrations of the reactants themselves. In your graph, the slope of the lines at any given point can provide insights into the kinetics of the reaction; a steeper slope means a faster rate of reaction. Understanding kinetics is essential for controlling reactions in industrial processes, developing new drugs, and even cleaning up the environment.

Concentrations of reactants and products are indicative of the evolving state of a chemical reaction. As the reaction commences, the concentration of the reactant A will be at its peak since it hasn't started converting to product P yet.
As time progresses, A molecules collide, interact, and transform into P, which is depicted by the descending curve for A's concentration on your graph. Concurrently, product P starts forming, reflected by the ascending curve from the origin. Initially, as there are more A molecules available to react, the rate of formation of P is rapid; thus, the P concentration curve rises steeply. Over time, as the amount of A decreases, the curve’s ascent lessens until it plateaus, indicating a decrease in the reaction rate. This demonstrates a direct relationship between reactant concentration and reaction rate, which is a fundamental aspect of reaction kinetics.

The equilibrium state is like a tug-of-war between the formation of reactants and products where neither side is winning. It's not a state of inactivity but rather a dynamic balance where the rate of the forward reaction (reactants converting to products) is equal to that of the reverse reaction (products reconverting to reactants).
In your graph, the equilibrium point is where the concentrations of A and P level off and the curves become parallel to the time axis. This does not necessarily mean that the concentrations of the reactant and product are equal, but that they do not change with time. It’s essential for students to recognize that equilibrium is about the balance of rates of the forward and reverse reactions, not the balance of concentrations. Hence, at equilibrium, there's a constant shuttling of A and P back and forth, yet their overall amounts in the reaction vessel remain constant, demonstrating the concept of dynamic equilibrium in a chemical system.