Chapter 16.6, Problem 16.11BFP

(a)

Interpretation Introduction

Interpretation : The balanced chemical equation for the overall reaction of the given mechanism should be interpreted.

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

Concept Introduction :

Chemical kinetics is the branch of chemistry that deals with the rate of chemical reactions. 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 molecularity of each step of the given mechanism should be interpreted.

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

Concept Introduction :

Chemical kinetics is the branch of chemistry that deals with the rate of chemical reactions. 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.

(c)

Interpretation Introduction

Interpretation : The rate law of the given mechanism should be interpreted.

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

Concept Introduction :

Chemical kinetics is the branch of chemistry that deals with the rate of chemical reactions. 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.