Chapter 16.6, Problem 16.12AFP

(a)

Interpretation Introduction

Interpretation : The intermediate needs to interpret the given mechanism of the decomposition of hydrogen peroxide.

  $\begin{array}{l}{\text{H}}_{\text{2}}{\text{O}}_{\text{2}}(aq)\to \text{2OH}(aq)\\ $ {\text{H}}_{\text{2}}{\text{O}}_{\text{2}}(aq)+\text{OH}(aq)\to {\text{H}}_{\text{2}}\text{O}(l)+\text{HO}(aq)$$ \text{HO}(aq)+\text{OH}(aq)\to {\text{H}}_{\text{2}}\text{O}(l)+\text{O}(g)$\end{array}$

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 rate constant is a constant of proportionality between the rate and the reactant's active mass. The total of the basic stages in the chemical equations can be the overall reactant.

(b)

Interpretation Introduction

Interpretation : The rate-determining step of the given mechanism should be determined if the rate law of the decomposition of hydrogen peroxide is given as:

  $Rate=k\left[{\text{H}}_{\text{2}}{\text{O}}_{\text{2}}\right]$

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 rate constant is a constant of proportionality between the rate and the reactant's active mass. The total of the basic stages in the chemical equations can be the overall reactant.