A reaction of the form a A ⟶Products is second order with a half-life of 287 s. What is the ra

step 1 A moles of A gives product, it is found to be second order reaction given half life denoted by T

A reaction of the form a A ⟶Products is second order with a...

A reaction of the form $a \mathrm{~A} \longrightarrow$ Products is second order with a half-life of $287 \mathrm{~s}$. What is the rate constant of the reaction if the initial concentration of $\mathrm{A}$ is $1.87 \times$ $10^{-2} \mathrm{~mol} / \mathrm{L} ?$

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Second Order Reaction

A second order reaction is one where the rate depends on either the square of a single reactant's concentration or on the product of two different reactants' concentrations. In this problem, the reaction rate is proportional to [A]², making it a second order reaction overall.

Integrated Rate Law for Second Order Reactions

The integrated rate law for a second order reaction relates the concentration of a reactant to time with the expression 1/[A] = 1/[A]? + kt. This equation allows one to determine the rate constant if the initial concentration and the concentration at a given time (or the half-life) are known.

Half-Life in Second Order Reactions

For second order reactions, the half-life is not constant but depends inversely on the initial concentration. The half-life is given by t?/? = 1/(k[A]?), enabling the determination of the rate constant by rearranging the equation if the half-life and initial concentration are provided.

Rate Constant

The rate constant, k, is a proportionality constant that provides the relationship between the rate of reaction and the reactant concentrations in the rate law. It has specific units—in this case, L/mol·s for second order reactions—and can be calculated by using the integrated rate law and the measured half-life.

Transcript

Please give Ace some feedback