What is the half-life for this reaction at the initial concentration?

Verified step by step guidance

1. Identify the order of the reaction. The half-life formula depends on whether the reaction is zero-order, first-order, or second-order.
2. For a first-order reaction, use the formula for half-life: $t_{1/2} = \frac{0.693}{k}$, where $k$ is the rate constant.
3. For a second-order reaction, use the formula: $t_{1/2} = \frac{1}{k[A]_0}$, where $[A]_0$ is the initial concentration.
4. For a zero-order reaction, use the formula: $t_{1/2} = \frac{[A]_0}{2k}$.
5. Determine the rate constant $k$ and the initial concentration $[A]_0$ if needed, and apply the appropriate formula to find the half-life.

Key Concepts

Half-Life

Half-life is the time required for the concentration of a reactant to decrease to half of its initial value. It is a crucial concept in kinetics, particularly for first-order reactions, where the half-life remains constant regardless of concentration. Understanding half-life helps predict how long it will take for a reaction to reach a certain point, which is essential for various applications in chemistry and pharmacology.

Reaction Order

The order of a reaction refers to the power to which the concentration of a reactant is raised in the rate law. It determines how the rate of reaction changes with varying concentrations of reactants. For example, in first-order reactions, the rate is directly proportional to the concentration of one reactant, which directly influences the calculation of half-life.

Initial Concentration

Initial concentration is the concentration of a reactant at the start of a reaction. It plays a significant role in determining the rate of reaction and the half-life, especially in reactions of different orders. Knowing the initial concentration allows for accurate calculations of how long it will take for the concentration to decrease to half its value, which is essential for understanding the kinetics of the reaction.