Chapter 16, Problem 16.48P

Interpretation Introduction

Interpretation: The concentration of $\left[\text{AB}\right]$ after $10.0\text{ s}$ should be calculated if the rate constant is $k\text{ = 0}\text{.2 L/mol}\text{.s}$ and the initial concentration of $\left[\text{AB}\right]$ is $1.50\text{ M}$ for the given reaction and rate law.

  $\begin{array}{l}\text{AB}\left(g\right)\to \text{A}\left(g\right)+\text{B}\left(g\right)\\ \text{Rate}=k{\left[\text{AB}\right]}^2\end{array}$

Concept Introduction: The area of chemistry that deals with the rate of the chemical reaction is known as chemical kinetics. The active masses of the reactants involved in the chemical reaction are expressed by the rate law. The order of the reaction can be determined with the help of rate law.

For a second-order reaction, the rate of reaction depends on the two power of the reactant molecule.