Chapter 16.6, Problem 16.12BFP

(a)

Interpretation Introduction

Interpretation : The intermediate needs to interpret the given mechanism of the reaction of $\text{NO}(aq)$ with ${\text{H}}_{\text{2}}(g)$ .

  $\begin{array}{l}2\text{NO}(aq)\to {\text{N}}_{\text{2}}{\text{O}}_{\text{2}}(g)\\ {\text{N}}_{\text{2}}{\text{O}}_{\text{2}}(g)+{\text{H}}_{\text{2}}(g)\to {\text{N}}_{\text{2}}\text{O}(g)+{\text{ H}}_{\text{2}}\text{O}(g)\\ {\text{N}}_{\text{2}}\text{O}(g)+{\text{H}}_{\text{2}}(g)\to {\text{N}}_{\text{2}}(g)+{\text{H}}_{\text{2}}\text{O}(g)\end{array}$

Concept Introduction :

Chemical kinetics is the branch of chemistry that deals with the rate of chemical reaction. The rate law is the expression of the active masses of the reactants involved in the chemical reaction. The rate constant is a proportionality constant between the rate and active mass of the reactant. The overall reactant can be the sum of the elementary steps of the chemical equations.

(b)

Interpretation Introduction

Interpretation : The consistency of the given mechanism must be interpreted with the given rate law.

  $Rate=k{\left[\text{NO}(aq)\right]}^2\left[{\text{H}}_{\text{2}}(g)\right]$

  $\begin{array}{l}2\text{NO}(aq)\to {\text{N}}_{\text{2}}{\text{O}}_{\text{2}}(g)\\ {\text{N}}_{\text{2}}{\text{O}}_{\text{2}}(g)+{\text{H}}_{\text{2}}(g)\to {\text{N}}_{\text{2}}\text{O}(g)+{\text{ H}}_{\text{2}}\text{O}(g)\\ {\text{N}}_{\text{2}}\text{O}(g)+{\text{H}}_{\text{2}}(g)\to {\text{N}}_{\text{2}}(g)+{\text{H}}_{\text{2}}\text{O}(g)\end{array}$

Concept Introduction :

Chemical kinetics is the branch of chemistry that deals with the rate of chemical reaction. The rate law is the expression of the active masses of the reactants involved in the chemical reaction. The rate constant is a proportionality constant between the rate and active mass of the reactant. The overall reactant can be the sum of the elementary steps of the chemical equations.