First-order reaction

Definition

A first-order reaction is a type of chemical reaction where the rate of the reaction is directly proportional to the concentration of one reactant. This means that if you double the concentration of that reactant, the rate of the reaction also doubles. First-order reactions are characterized by a specific mathematical relationship in their rate laws, which allows for straightforward predictions about how changes in concentration will affect reaction rates.

5 Must Know Facts For Your Next Test

1. In a first-order reaction, the unit of the rate constant (k) is typically s^-1 (inverse seconds), indicating how quickly the reaction proceeds.
2. The integrated rate law for a first-order reaction can be expressed as $$ ext{ln}[A]_t = -kt + ext{ln}[A]_0$$, where [A]_t is the concentration at time t and [A]_0 is the initial concentration.
3. For first-order reactions, plotting $$ ext{ln}[A]$$ versus time yields a straight line with a slope of -k, which is useful for determining reaction rates.
4. The half-life of a first-order reaction is independent of the initial concentration and can be calculated using the formula $$t_{1/2} = rac{0.693}{k}$$.
5. Many biological processes, including drug metabolism and enzyme kinetics, often follow first-order kinetics due to their dependency on substrate concentration.

Review Questions

• How does changing the concentration of a reactant affect the rate of a first-order reaction?
  • In a first-order reaction, the rate is directly proportional to the concentration of that specific reactant. This means that if you increase the concentration by a certain factor, such as doubling it, the reaction rate will also double. This linear relationship allows for predictable behavior in terms of how quickly products are formed as reactant concentrations change.
• Discuss how the half-life of a first-order reaction can provide insights into its kinetics and predict behavior over time.
  • The half-life of a first-order reaction is unique because it remains constant regardless of the initial concentration. This characteristic allows chemists to predict how long it will take for half of a reactant to be consumed during the reaction. The consistent half-life means that reactions can be modeled over time with reliability, making it easier to understand how quickly reactions will progress under varying conditions.
• Evaluate how understanding first-order reactions can influence drug design and administration in pharmacology.
  • Understanding first-order reactions is crucial in pharmacology because many drugs exhibit first-order kinetics when metabolized in the body. By recognizing that drug elimination follows this pattern, pharmacologists can design dosing regimens that optimize therapeutic effects while minimizing toxicity. Additionally, knowing that the half-life remains constant helps in predicting how long it takes for drugs to reach effective concentrations in patients, allowing for tailored medication plans based on individual needs and responses.

Related terms

Rate Constant: A constant that appears in the rate law equation, representing the proportionality factor between the rate of a reaction and the concentration of reactants.

Half-life: The time required for the concentration of a reactant to decrease to half of its initial value, which is constant for first-order reactions regardless of concentration.

Integrated Rate Law: An equation that relates the concentrations of reactants to time, allowing for the calculation of concentrations at any given time during a chemical reaction.