\(75 \%\) of a first-order reaction was completed in \(32 \mathrm{~min}\). When was \(50 \%\) of the reaction completed? (a) \(24 \mathrm{~min}\) (b) \(16 \mathrm{~min}\) (c) \(8 \mathrm{~min}\) (d) \(64 \mathrm{~min}\)

At its core, chemical kinetics is the study of how fast chemical reactions occur. It's a central part of understanding chemistry, providing insights into reaction mechanisms and the factors that influence the speed of reactions. For students diving into chemical kinetics, it's crucial to comprehend how various variables—such as temperature, concentration of reactants, and the presence of catalysts—can affect the reaction rate.

A first-order reaction, one of the basic reaction types in kinetics, is characterized by its reaction rate being directly proportional to the concentration of only one reactant. What makes this reaction type fascinating is its consistent half-life, which remains unchanged regardless of the initial concentration of the reactant. This property is incredibly useful in calculations and predictions regarding the reaction progress.

In educational settings like NEET chemistry preparation, grasping chemical kinetics is imperative as it lays the groundwork for more complex topics and practical applications in fields such as pharmacology and environmental science.

Understanding the reaction rate is essential for mastery in chemistry and succeeding in competitive exams like NEET. Reaction rate refers to the speed at which reactants are converted into products in a chemical reaction. Simplified, it's how quickly a reaction proceeds. For first-order reactions, the rule of thumb is straightforward—the rate is directly proportional to the concentration of one reactant.

To practically apply this knowledge, assume we're observing a colored chemical dissipate in a solution. The faster the color fades, the higher the reaction rate. In a first-order reaction, this fading would occur at a rate that, mathematically, is expressed as -\frac{{d[A]}}{{dt}} = k[A], where \([A]\) is the concentration of the reactant, \(t\) is time, and \(k\) is the rate constant.

For NEET aspirants, understanding how to use half-life, which for a first-order reaction is constant and independent of concentration, is a powerful tool for solving problems efficiently.

Preparing for competitive exams like the National Eligibility cum Entrance Test (NEET) demands a strong foundation in chemistry concepts. One must be well-versed in topics like chemical kinetics and the nature of different reactions to crack the chemistry section.

Focused practice on reaction rates and calculations involving half-life can significantly enhance your performance in the exam. Remember, for first-order reactions, the half-life is a consistent value—a critical point that simplifies complex problems.

For instance, when dealing with exercises related to the half-life of a reaction, it's essential to apply logical reasoning and mathematical skills. These problems are structured to test both your conceptual understanding and problem-solving approach—a balance NEET aims to assess in prospective medical students.

Regular revisions, solving past papers, and an in-depth grasp of the basic principles, like the steps demonstrated for the first-order reaction half-life problem, are strategies that can lead to success in NEET chemistry.